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4,601 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.03087 M | A strong monoprotic acid is fully dissociated. At concentration 0.03087 mol/L, [H⁺] = 0.03087 M and pH = −log₁₀[H⁺] = 1.51. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,602 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.02415 M | A strong monoprotic acid is fully dissociated. At concentration 0.02415 mol/L, [H⁺] = 0.02415 M and pH = −log₁₀[H⁺] = 1.617. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,603 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.8719e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.8719e-04 mol/L, [H⁺] = 1.8719e-04 M and pH = −log₁₀[H⁺] = 3.728. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,604 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.0209 M | A strong monoprotic acid is fully dissociated. At concentration 0.0209 mol/L, [H⁺] = 0.0209 M and pH = −log₁₀[H⁺] = 1.68. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,605 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 5.9517e-04 M | A strong monoprotic acid is fully dissociated. At concentration 5.9517e-04 mol/L, [H⁺] = 5.9517e-04 M and pH = −log₁₀[H⁺] = 3.225. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,606 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.00253 M | A strong monoprotic acid is fully dissociated. At concentration 0.00253 mol/L, [H⁺] = 0.00253 M and pH = −log₁₀[H⁺] = 2.597. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,607 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.2426e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.2426e-04 mol/L, [H⁺] = 1.2426e-04 M and pH = −log₁₀[H⁺] = 3.906. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,608 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 2.2177e-04 M | A strong monoprotic acid is fully dissociated. At concentration 2.2177e-04 mol/L, [H⁺] = 2.2177e-04 M and pH = −log₁₀[H⁺] = 3.654. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,609 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.009441 M | A strong monoprotic acid is fully dissociated. At concentration 0.009441 mol/L, [H⁺] = 0.009441 M and pH = −log₁₀[H⁺] = 2.025. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,610 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 3.6247e-04 M | A strong monoprotic acid is fully dissociated. At concentration 3.6247e-04 mol/L, [H⁺] = 3.6247e-04 M and pH = −log₁₀[H⁺] = 3.441. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,611 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 2.6269e-04 M | A strong monoprotic acid is fully dissociated. At concentration 2.6269e-04 mol/L, [H⁺] = 2.6269e-04 M and pH = −log₁₀[H⁺] = 3.581. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,612 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.005761 M | A strong monoprotic acid is fully dissociated. At concentration 0.005761 mol/L, [H⁺] = 0.005761 M and pH = −log₁₀[H⁺] = 2.24. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,613 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001309 M | A strong monoprotic acid is fully dissociated. At concentration 0.001309 mol/L, [H⁺] = 0.001309 M and pH = −log₁₀[H⁺] = 2.883. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,614 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001361 M | A strong monoprotic acid is fully dissociated. At concentration 0.001361 mol/L, [H⁺] = 0.001361 M and pH = −log₁₀[H⁺] = 2.866. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,615 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.005823 M | A strong monoprotic acid is fully dissociated. At concentration 0.005823 mol/L, [H⁺] = 0.005823 M and pH = −log₁₀[H⁺] = 2.235. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,616 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.2634e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.2634e-04 mol/L, [H⁺] = 1.2634e-04 M and pH = −log₁₀[H⁺] = 3.898. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,617 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.0127 M | A strong monoprotic acid is fully dissociated. At concentration 0.0127 mol/L, [H⁺] = 0.0127 M and pH = −log₁₀[H⁺] = 1.896. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,618 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.007734 M | A strong monoprotic acid is fully dissociated. At concentration 0.007734 mol/L, [H⁺] = 0.007734 M and pH = −log₁₀[H⁺] = 2.112. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,619 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.04055 M | A strong monoprotic acid is fully dissociated. At concentration 0.04055 mol/L, [H⁺] = 0.04055 M and pH = −log₁₀[H⁺] = 1.392. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,620 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.0561e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.0561e-04 mol/L, [H⁺] = 1.0561e-04 M and pH = −log₁₀[H⁺] = 3.976. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,621 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001837 M | A strong monoprotic acid is fully dissociated. At concentration 0.001837 mol/L, [H⁺] = 0.001837 M and pH = −log₁₀[H⁺] = 2.736. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,622 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.00101 M | A strong monoprotic acid is fully dissociated. At concentration 0.00101 mol/L, [H⁺] = 0.00101 M and pH = −log₁₀[H⁺] = 2.996. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,623 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.008783 M | A strong monoprotic acid is fully dissociated. At concentration 0.008783 mol/L, [H⁺] = 0.008783 M and pH = −log₁₀[H⁺] = 2.056. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,624 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.9981e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.9981e-04 mol/L, [H⁺] = 1.9981e-04 M and pH = −log₁₀[H⁺] = 3.699. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,625 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.05488 M | A strong monoprotic acid is fully dissociated. At concentration 0.05488 mol/L, [H⁺] = 0.05488 M and pH = −log₁₀[H⁺] = 1.261. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,626 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 8.2952e-04 M | A strong monoprotic acid is fully dissociated. At concentration 8.2952e-04 mol/L, [H⁺] = 8.2952e-04 M and pH = −log₁₀[H⁺] = 3.081. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,627 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.002515 M | A strong monoprotic acid is fully dissociated. At concentration 0.002515 mol/L, [H⁺] = 0.002515 M and pH = −log₁₀[H⁺] = 2.599. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,628 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 3.6181e-04 M | A strong monoprotic acid is fully dissociated. At concentration 3.6181e-04 mol/L, [H⁺] = 3.6181e-04 M and pH = −log₁₀[H⁺] = 3.442. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,629 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.1621e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.1621e-04 mol/L, [H⁺] = 1.1621e-04 M and pH = −log₁₀[H⁺] = 3.935. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,630 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.02677 M | A strong monoprotic acid is fully dissociated. At concentration 0.02677 mol/L, [H⁺] = 0.02677 M and pH = −log₁₀[H⁺] = 1.572. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,631 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.002341 M | A strong monoprotic acid is fully dissociated. At concentration 0.002341 mol/L, [H⁺] = 0.002341 M and pH = −log₁₀[H⁺] = 2.631. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,632 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.005344 M | A strong monoprotic acid is fully dissociated. At concentration 0.005344 mol/L, [H⁺] = 0.005344 M and pH = −log₁₀[H⁺] = 2.272. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,633 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.002018 M | A strong monoprotic acid is fully dissociated. At concentration 0.002018 mol/L, [H⁺] = 0.002018 M and pH = −log₁₀[H⁺] = 2.695. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,634 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001578 M | A strong monoprotic acid is fully dissociated. At concentration 0.001578 mol/L, [H⁺] = 0.001578 M and pH = −log₁₀[H⁺] = 2.802. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,635 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.03179 M | A strong monoprotic acid is fully dissociated. At concentration 0.03179 mol/L, [H⁺] = 0.03179 M and pH = −log₁₀[H⁺] = 1.498. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,636 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 5.7243e-04 M | A strong monoprotic acid is fully dissociated. At concentration 5.7243e-04 mol/L, [H⁺] = 5.7243e-04 M and pH = −log₁₀[H⁺] = 3.242. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,637 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001317 M | A strong monoprotic acid is fully dissociated. At concentration 0.001317 mol/L, [H⁺] = 0.001317 M and pH = −log₁₀[H⁺] = 2.88. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,638 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001032 M | A strong monoprotic acid is fully dissociated. At concentration 0.001032 mol/L, [H⁺] = 0.001032 M and pH = −log₁₀[H⁺] = 2.986. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,639 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.01086 M | A strong monoprotic acid is fully dissociated. At concentration 0.01086 mol/L, [H⁺] = 0.01086 M and pH = −log₁₀[H⁺] = 1.964. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,640 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 7.9528e-04 M | A strong monoprotic acid is fully dissociated. At concentration 7.9528e-04 mol/L, [H⁺] = 7.9528e-04 M and pH = −log₁₀[H⁺] = 3.099. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,641 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.08171 M | A strong monoprotic acid is fully dissociated. At concentration 0.08171 mol/L, [H⁺] = 0.08171 M and pH = −log₁₀[H⁺] = 1.088. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,642 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.04288 M | A strong monoprotic acid is fully dissociated. At concentration 0.04288 mol/L, [H⁺] = 0.04288 M and pH = −log₁₀[H⁺] = 1.368. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,643 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.01948 M | A strong monoprotic acid is fully dissociated. At concentration 0.01948 mol/L, [H⁺] = 0.01948 M and pH = −log₁₀[H⁺] = 1.71. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,644 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.05042 M | A strong monoprotic acid is fully dissociated. At concentration 0.05042 mol/L, [H⁺] = 0.05042 M and pH = −log₁₀[H⁺] = 1.297. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,645 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.003318 M | A strong monoprotic acid is fully dissociated. At concentration 0.003318 mol/L, [H⁺] = 0.003318 M and pH = −log₁₀[H⁺] = 2.479. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,646 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001832 M | A strong monoprotic acid is fully dissociated. At concentration 0.001832 mol/L, [H⁺] = 0.001832 M and pH = −log₁₀[H⁺] = 2.737. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,647 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.021 M | A strong monoprotic acid is fully dissociated. At concentration 0.021 mol/L, [H⁺] = 0.021 M and pH = −log₁₀[H⁺] = 1.678. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,648 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.07277 M | A strong monoprotic acid is fully dissociated. At concentration 0.07277 mol/L, [H⁺] = 0.07277 M and pH = −log₁₀[H⁺] = 1.138. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,649 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001593 M | A strong monoprotic acid is fully dissociated. At concentration 0.001593 mol/L, [H⁺] = 0.001593 M and pH = −log₁₀[H⁺] = 2.798. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,650 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.2181e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.2181e-04 mol/L, [H⁺] = 1.2181e-04 M and pH = −log₁₀[H⁺] = 3.914. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,651 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.00344 M | A strong monoprotic acid is fully dissociated. At concentration 0.00344 mol/L, [H⁺] = 0.00344 M and pH = −log₁₀[H⁺] = 2.463. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,652 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.05849 M | A strong monoprotic acid is fully dissociated. At concentration 0.05849 mol/L, [H⁺] = 0.05849 M and pH = −log₁₀[H⁺] = 1.233. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,653 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.04569 M | A strong monoprotic acid is fully dissociated. At concentration 0.04569 mol/L, [H⁺] = 0.04569 M and pH = −log₁₀[H⁺] = 1.34. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,654 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.07865 M | A strong monoprotic acid is fully dissociated. At concentration 0.07865 mol/L, [H⁺] = 0.07865 M and pH = −log₁₀[H⁺] = 1.104. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,655 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.06738 M | A strong monoprotic acid is fully dissociated. At concentration 0.06738 mol/L, [H⁺] = 0.06738 M and pH = −log₁₀[H⁺] = 1.171. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,656 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 3.9390e-04 M | A strong monoprotic acid is fully dissociated. At concentration 3.9390e-04 mol/L, [H⁺] = 3.9390e-04 M and pH = −log₁₀[H⁺] = 3.405. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,657 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.08266 M | A strong monoprotic acid is fully dissociated. At concentration 0.08266 mol/L, [H⁺] = 0.08266 M and pH = −log₁₀[H⁺] = 1.083. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,658 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.01801 M | A strong monoprotic acid is fully dissociated. At concentration 0.01801 mol/L, [H⁺] = 0.01801 M and pH = −log₁₀[H⁺] = 1.744. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,659 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 2.4529e-04 M | A strong monoprotic acid is fully dissociated. At concentration 2.4529e-04 mol/L, [H⁺] = 2.4529e-04 M and pH = −log₁₀[H⁺] = 3.61. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,660 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 9.9871e-04 M | A strong monoprotic acid is fully dissociated. At concentration 9.9871e-04 mol/L, [H⁺] = 9.9871e-04 M and pH = −log₁₀[H⁺] = 3.001. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,661 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.07581 M | A strong monoprotic acid is fully dissociated. At concentration 0.07581 mol/L, [H⁺] = 0.07581 M and pH = −log₁₀[H⁺] = 1.12. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,662 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.08147 M | A strong monoprotic acid is fully dissociated. At concentration 0.08147 mol/L, [H⁺] = 0.08147 M and pH = −log₁₀[H⁺] = 1.089. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,663 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 8.4688e-04 M | A strong monoprotic acid is fully dissociated. At concentration 8.4688e-04 mol/L, [H⁺] = 8.4688e-04 M and pH = −log₁₀[H⁺] = 3.072. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,664 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.01984 M | A strong monoprotic acid is fully dissociated. At concentration 0.01984 mol/L, [H⁺] = 0.01984 M and pH = −log₁₀[H⁺] = 1.703. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,665 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.02538 M | A strong monoprotic acid is fully dissociated. At concentration 0.02538 mol/L, [H⁺] = 0.02538 M and pH = −log₁₀[H⁺] = 1.596. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,666 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.002378 M | A strong monoprotic acid is fully dissociated. At concentration 0.002378 mol/L, [H⁺] = 0.002378 M and pH = −log₁₀[H⁺] = 2.624. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,667 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 3.1335e-04 M | A strong monoprotic acid is fully dissociated. At concentration 3.1335e-04 mol/L, [H⁺] = 3.1335e-04 M and pH = −log₁₀[H⁺] = 3.504. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,668 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.0058e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.0058e-04 mol/L, [H⁺] = 1.0058e-04 M and pH = −log₁₀[H⁺] = 3.997. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,669 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 2.7700e-04 M | A strong monoprotic acid is fully dissociated. At concentration 2.7700e-04 mol/L, [H⁺] = 2.7700e-04 M and pH = −log₁₀[H⁺] = 3.558. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,670 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.04455 M | A strong monoprotic acid is fully dissociated. At concentration 0.04455 mol/L, [H⁺] = 0.04455 M and pH = −log₁₀[H⁺] = 1.351. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,671 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 8.0140e-04 M | A strong monoprotic acid is fully dissociated. At concentration 8.0140e-04 mol/L, [H⁺] = 8.0140e-04 M and pH = −log₁₀[H⁺] = 3.096. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,672 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.7423e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.7423e-04 mol/L, [H⁺] = 1.7423e-04 M and pH = −log₁₀[H⁺] = 3.759. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,673 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 5.1115e-04 M | A strong monoprotic acid is fully dissociated. At concentration 5.1115e-04 mol/L, [H⁺] = 5.1115e-04 M and pH = −log₁₀[H⁺] = 3.291. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,674 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 4.0735e-04 M | A strong monoprotic acid is fully dissociated. At concentration 4.0735e-04 mol/L, [H⁺] = 4.0735e-04 M and pH = −log₁₀[H⁺] = 3.39. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,675 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 1.8642e-04 M | A strong monoprotic acid is fully dissociated. At concentration 1.8642e-04 mol/L, [H⁺] = 1.8642e-04 M and pH = −log₁₀[H⁺] = 3.729. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,676 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 5.4225e-04 M | A strong monoprotic acid is fully dissociated. At concentration 5.4225e-04 mol/L, [H⁺] = 5.4225e-04 M and pH = −log₁₀[H⁺] = 3.266. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,677 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.01133 M | A strong monoprotic acid is fully dissociated. At concentration 0.01133 mol/L, [H⁺] = 0.01133 M and pH = −log₁₀[H⁺] = 1.946. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,678 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.03444 M | A strong monoprotic acid is fully dissociated. At concentration 0.03444 mol/L, [H⁺] = 0.03444 M and pH = −log₁₀[H⁺] = 1.463. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,679 | chemistry | acids_bases | strong_acid_ph | 4 | worked_example | pH of strong acid at concentration 0.001327 M | A strong monoprotic acid is fully dissociated. At concentration 0.001327 mol/L, [H⁺] = 0.001327 M and pH = −log₁₀[H⁺] = 2.877. This relation follows directly from the definition of pH and the complete dissociation assumption. | pH = -log10 [H+] | mole_concept; logarithmic functions | Calculate the pH of a strong monoprotic acid solution. |
4,680 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.7312 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.7312. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,681 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.117 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.117. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,682 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.668 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.668. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,683 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 13.2 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 13.2. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse react... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,684 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 15.58 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 15.58. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,685 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 299.9 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 299.9. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,686 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 10.25 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 10.25. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,687 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 97.29 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 97.29. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,688 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 17.27 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 17.27. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,689 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 37.87 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 37.87. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,690 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.003758 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.003758. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,691 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.005902 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.005902. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,692 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 37.87 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 37.87. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,693 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.006326 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.006326. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,694 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 43.61 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 43.61. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,695 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 244.4 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 244.4. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,696 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 82.94 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 82.94. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,697 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 24.11 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 24.11. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse reac... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,698 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.3528 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.3528. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,699 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.2307 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.2307. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse rea... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
4,700 | chemistry | equilibrium | equilibrium_constant | 6 | explanation | Meaning of equilibrium constant K = 0.002691 | For a reversible reaction at a fixed temperature, the equilibrium constant K is a thermodynamic quantity determined solely by the standard Gibbs free-energy change: K = exp(−ΔG° / R T). In the present illustration K = 0.002691. When Q (reaction quotient) < K the forward reaction is spontaneous; when Q > K the reverse r... | K = exp(-ΔG° / R T); ΔG = ΔG° + R T ln Q | thermodynamics_first_law; mole_concept | Interpret the magnitude of an equilibrium constant and its relation to ΔG°. |
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