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14. 4 • hydrolysis of salts 719 however, the aluminum ( iii ) ion actually reacts with six water molecules to form a stable complex ion, and so the more explicit representation of the dissolution process is as shown in figure 14. 13, the ions involve bonds between a central al atom and the o atoms of the six water mole... | openstax_chemistry2e-web | [
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as equal to the hydronium ion concentration, and so the ph is calculated to be check your learning what is in a 0. 15 - m solution of al ( no3 ) 3 that contains enough of the strong acid hno3 to bring [ h3o + ] to 0. 10 m? answer : 2. 1 10−5 m 14. 5 polyprotic acids learning objectives by the end of this section, you w... | openstax_chemistry2e-web | [
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14. 5 • polyprotic acids 721 similarly, monoprotic bases are bases that will accept a single proton. diprotic acids contain two ionizable hydrogen atoms per molecule ; ionization of such acids occurs in two steps. the first ionization always takes place to a greater extent than the second ionization. for example, sulfu... | openstax_chemistry2e-web | [
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##s, h2co3 is a much stronger acid than so the stepwise 722 14 • acid - base equilibria access for free at openstax. org ionization reactions may be treated separately. the first ionization reaction is using provided information, an ice table for this first step is prepared : substituting the equilibrium concentrations... | openstax_chemistry2e-web | [
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14. 5 • polyprotic acids 723 a triprotic acid is an acid that has three ionizable h atoms. phosphoric acid is one example : as for the diprotic acid examples, each successive ionization reaction is less extensive than the former, reflected in decreasing values for the stepwise acid ionization constants. this is a gener... | openstax_chemistry2e-web | [
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14. 6 buffers learning objectives by the end of this section, you will be able to : • describe the composition and function of acid – base buffers • calculate the ph of a buffer before and after the addition of added acid or base a solution containing appreciable amounts of a weak conjugate acid - base pair is called a... | openstax_chemistry2e-web | [
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base added to this solution will neutralize hydronium ion, causing the acetic acid ionization equilibrium to shift to the right and generate additional amounts of the weak conjugate base ( acetate ion ) : likewise, strong acid added to this buffer solution will shift the above ionization equilibrium left, producing add... | openstax_chemistry2e-web | [
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14. 6 • buffers 725 substituting the equilibrium concentration terms into the ka expression, assuming x < < 0. 10, and solving the simplified equation for x yields ( b ) calculate the ph after 1. 0 ml of 0. 10 m naoh is added to 100 ml of this buffer. adding strong base will neutralize some of the acetic acid, yielding... | openstax_chemistry2e-web | [
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ph ( from 4. 74 to 10. 99 ) compared with the very slight increase observed for the buffer solution in part ( b ) ( from 4. 74 to 4. 75 ). check your learning show that adding 1. 0 ml of 0. 10 m hcl changes the ph of 100 ml of a 1. 8 10−5 m hcl solution from 4. 74 to 3. 00. answer : initial ph of 1. 8 10−5 m hcl ; ph =... | openstax_chemistry2e-web | [
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0. 0010 l = 1. 0 10−4 moles ; final ph after addition of 1. 0 ml of 0. 10 m hcl : buffer capacity buffer solutions do not have an unlimited capacity to keep the ph relatively constant ( figure 14. 16 ). instead, the ability of a buffer solution to resist changes in ph relies on the presence of appreciable amounts of it... | openstax_chemistry2e-web | [
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14. 6 • buffers 727 acid and its conjugate base that are in a buffer mixture. for example, 1 l of a solution that is 1. 0 m in acetic acid and 1. 0 m in sodium acetate has a greater buffer capacity than 1 l of a solution that is 0. 10 m in acetic acid and 0. 10 m in sodium acetate even though both solutions have the sa... | openstax_chemistry2e-web | [
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is removed primarily by the reaction : an added hydroxide ion is removed by the reaction : the added strong acid or base is thus effectively converted to the much weaker acid or base of the buffer pair ( h3o + is converted to h2co3 and oh - is converted to hco3 - ). the ph of human blood thus remains very near the valu... | openstax_chemistry2e-web | [
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obtained a medical degree from harvard and then spent 2 years studying in strasbourg, then a part of germany, before returning to take a lecturer position at harvard. he eventually became a professor at harvard and worked there his entire life. he discovered that the acid - base balance in human blood is regulated by a... | openstax_chemistry2e-web | [
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14. 6 • buffers 729 the concentration of carbonic acid, h2co3 is approximately 0. 0012 m, and the concentration of the hydrogen carbonate ion, is around 0. 024 m. using the henderson - hasselbalch equation and the pka of carbonic acid at body temperature, we can calculate the ph of blood : the fact that the h2co3 conce... | openstax_chemistry2e-web | [
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14. 7 acid - base titrations learning objectives by the end of this section, you will be able to : • interpret titration curves for strong and weak acid - base systems • compute sample ph at important stages of a titration • explain the function of acid - base indicators as seen in the chapter on the stoichiometry of c... | openstax_chemistry2e-web | [
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. the solution ph is due to the acid ionization of hcl. because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0. 100 m. the ph of the solution is then ( b ) titrant volume = 12. 50 ml. since the acid sample and the base titrant are both monoprotic and equally concentrated, this tit... | openstax_chemistry2e-web | [
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: 1. 000 ; 15. 0 : 1. 5111 ; 25. 0 : 7 ; 40. 0 : 12. 523 example 14. 22 titration of a weak acid with a strong base consider the titration of 25. 00 ml of 0. 100 m ch3co2h with 0. 100 m naoh. the reaction can be represented as : calculate the ph of the titration solution after the addition of the following volumes of n... | openstax_chemistry2e-web | [
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14. 7 • acid - base titrations 731 ( d ) 37. 50 ml solution ( a ) the initial ph is computed for the acetic acid solution in the usual ice approach : and ( b ) the acid and titrant are both monoprotic and the sample and titrant solutions are equally concentrated ; thus, this volume of titrant represents the equivalence... | openstax_chemistry2e-web | [
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##tion between 50. 0 ml of 0. 100 m hcooh ( aq ) ( formic acid ) and 0. 200 m naoh ( titrant ) at the listed volumes of added base : 0. 00 ml, 15. 0 ml, 25. 0 ml, and 30. 0 ml. 732 14 • acid - base equilibria access for free at openstax. org answer : | openstax_chemistry2e-web | [
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0. 00 ml : 2. 37 ; 15. 0 ml : 3. 92 ; 25. 00 ml : 8. 29 ; 30. 0 ml : 12. 097 performing additional calculations similar to those in the preceding example permits a more full assessment of titration curves. a summary of ph / volume data pairs for the strong and weak acid titrations is provided in table 14. 2 and plotted... | openstax_chemistry2e-web | [
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. 00050 1. 18 4. 14 10. 0 0. 00100 1. 37 4. 57 15. 0 0. 00150 1. 60 4. 92 20. 0 0. 00200 1. 95 5. 35 22. 0 0. 00220 2. 20 5. 61 24. 0 0. 00240 2. 69 6. 13 24. 5 0. 00245 3. 00 6. 44 24. 9 0. 00249 3. 70 7. 14 25. 0 0. 00250 7. 00 8. 72 25. 1 0. 00251 10. 30 10. 30 25. 5 0. 00255 11. 00 11. 00 26. 0 0. 00260 11. 29 11. ... | openstax_chemistry2e-web | [
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12. 52 table 14. 2 figure 14. 18 ( a ) the titration curve for the titration of 25. 00 ml of 0. 100 m hcl ( strong acid ) with 0. 100 m naoh ( strong base ) has an equivalence point of 7. 00 ph. ( b ) the titration curve for the titration of 25. 00 ml of 0. 100 m acetic acid ( weak acid ) with 0. 100 m naoh ( strong ba... | openstax_chemistry2e-web | [
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equilibrium towards the yellow form. this behavior is completely analogous to the action of buffers. the perceived color of an indicator solution is determined by the ratio of the concentrations of the two species in−and hin. if most of the indicator ( typically about 60−90 % or more ) is present as in−, the perceived ... | openstax_chemistry2e-web | [
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14. 7 • acid - base titrations 735 figure 14. 19 this chart illustrates the color change intervals for several acid - base indicators. 736 14 • acid - base equilibria access for free at openstax. org figure 14. 20 titration curves for strong and weak acids illustrating the proper choice of acid - base indicator. any of... | openstax_chemistry2e-web | [
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orange - to - yellow color change over a relatively large volume interval ( 0 – 6 ml ), completing the color change well before the equivalence point ( 25 ml ) has been reached. use of litmus would show a color change that begins after adding 7 – 8 ml of titrant and ends just before the equivalence point. phenolphthale... | openstax_chemistry2e-web | [
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14. 7 • acid - base titrations 737 key terms acid ionization reaction involving the transfer of a proton from an acid to water, yielding hydronium ions and the conjugate base of the acid acid ionization constant ( ka ) equilibrium constant for an acid ionization reaction acid - base indicator weak acid or base whose co... | openstax_chemistry2e-web | [
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ionization constant expression, conveniently formatted for calculating the ph of buffer solutions ion - product constant for water ( kw ) equilibrium constant for the autoionization of water leveling effect observation that acid - base strength of solutes in a given solvent is limited to that of the solvent ’ s charact... | openstax_chemistry2e-web | [
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14. 1 brønsted - lowry acids and bases a compound that can donate a proton ( a hydrogen ion ) to another compound is called a brønsted - lowry acid. the compound that accepts the proton is called a brønsted - lowry base. the species remaining after a brønsted - lowry acid has lost a proton is the conjugate base of the ... | openstax_chemistry2e-web | [
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14. 2 ph and poh concentrations of hydronium and hydroxide ions in aqueous media are often represented as logarithmic ph and poh values, respectively. at 25 °c, the autoprotolysis equilibrium for water requires the sum of ph and poh to equal 14 for any aqueous solution. the relative concentrations of hydronium and hydr... | openstax_chemistry2e-web | [
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14. 3 relative strengths of acids and bases the relative strengths of acids and bases are reflected in the magnitudes of their ionization constants ; the stronger the acid or base, the larger its ionization constant. a reciprocal relation exists between the strengths of a conjugate acid - base pair : the stronger the a... | openstax_chemistry2e-web | [
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contain appreciable amounts of a weak conjugate acid - base pair are called buffers. a buffered solution will experience only slight changes in ph when small amounts of acid or base are added. addition of large amounts of acid or base can exceed the buffer capacity, consuming most of one 14 • summary 739 conjugate part... | openstax_chemistry2e-web | [
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14. 1 brønsted - lowry acids and bases 1. write equations that show nh3 as both a conjugate acid and a conjugate base. 2. write equations that show acting both as an acid and as a base. 3. show by suitable net ionic equations that each of the following species can act as a brønsted - lowry acid : ( a ) ( b ) hcl ( c ) ... | openstax_chemistry2e-web | [
0.005522498395293951,
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0.06247871369123459,
0.012007113546133041,
0.012479620054364204,
0.06053546071052551,
-0... |
e ) ( f ) ( g ) h4n2 ( h ) ch3oh 9. identify and label the brønsted - lowry acid, its conjugate base, the brønsted - lowry base, and its conjugate acid in each of the following equations : ( a ) ( b ) ( c ) ( d ) ( e ) ( f ) ( g ) 10. identify and label the brønsted - lowry acid, its conjugate base, the brønsted - lowr... | openstax_chemistry2e-web | [
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0.041725512593984604,
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14. 2 ph and poh 15. explain why a sample of pure water at 40 °c is neutral even though [ h3o + ] = 1. 7 10−7 m. kw is 2. 9 10−14 at 40 °c. 16. the ionization constant for water ( kw ) is 2. 9 10−14 at 40 °c. calculate [ h3o + ], [ oh− ], ph, and poh for pure water at 40 °c. 17. the ionization constant for water ( kw )... | openstax_chemistry2e-web | [
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useful information. 24. the hydronium ion concentration in a sample of rainwater is found to be 1. 7 10−6 m at 25 °c. what is the concentration of hydroxide ions in the rainwater? 25. the hydroxide ion concentration in household ammonia is 3. 2 10−3 m at 25 °c. what is the concentration of hydronium ions in the solutio... | openstax_chemistry2e-web | [
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14. 3 relative strengths of acids and bases 26. explain why the neutralization reaction of a strong acid and a weak base gives a weakly acidic solution. 27. explain why the neutralization reaction of a weak acid and a strong base gives a weakly basic solution. 28. use this list of important industrial compounds ( and f... | openstax_chemistry2e-web | [
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. milk of magnesia, a suspension of solid mg ( oh ) 2 in an aqueous medium, is sometimes used to neutralize excess stomach acid. write a complete balanced equation for the neutralization reaction, and identify the conjugate acid - base pairs. 34. nitric acid reacts with insoluble copper ( ii ) oxide to form soluble cop... | openstax_chemistry2e-web | [
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) nh3 or ph3 ( e ) h2s or hbr 42. rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. ( a ) acidity : hcl, hbr, hi ( b ) basicity : h2o, oh−, h−, cl− ( c ) basicity : mg ( oh ) 2, si ( oh ) 4, clo3 ( oh ) ( hint : formula could a... | openstax_chemistry2e-web | [
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). 46. are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in water directly proportional or inversely proportional? explain your answer. 47. what two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak acid or base? 48. which of the... | openstax_chemistry2e-web | [
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) clo− : [ oh− ] = 4. 0 10−4 m ; [ hclo ] = 2. 38 10−4 m ; [ clo− ] = 0. 273 m ; ( c ) hco2h : [ hco2h ] = 0. 524 m ; = 9. 8 10−3 m ; = 9. 8 10−3 m ; ( d ) = 0. 233 m ; [ c6h5nh2 ] = 2. 3 10−3 m ; = 2. 3 10−3 m 54. from the equilibrium concentrations given, calculate ka for each of the weak acids and kb for each of the... | openstax_chemistry2e-web | [
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constant of its conjugate base or conjugate acid : ( a ) f− ( b ) ( c ) ( d ) ( e ) ( f ) ( as a base ) 58. calculate the ionization constant for each of the following acids or bases from the ionization constant of its conjugate base or conjugate acid : ( a ) hte− ( as a base ) ( b ) ( c ) ( as a base ) ( d ) ( as a ba... | openstax_chemistry2e-web | [
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an acid found in the blood after strenuous exercise, is 1. 36 10−4. if 20. 0 g of lactic acid is used to make a solution with a volume of 1. 00 l, what is the concentration of hydronium ion in the solution? 64. nicotine, c10h14n2, is a base that will accept two protons ( kb1 = 7 10−7, kb2 = 1. 4 10−11 ). what is the co... | openstax_chemistry2e-web | [
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14. 4 hydrolysis of salts 69. determine whether aqueous solutions of the following salts are acidic, basic, or neutral : ( a ) al ( no3 ) 3 ( b ) rbi ( c ) khco2 ( d ) ch3nh3br 70. determine whether aqueous solutions of the following salts are acidic, basic, or neutral : ( a ) fecl3 ( b ) k2co3 ( c ) nh4br ( d ) kclo4 ... | openstax_chemistry2e-web | [
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14. 5 polyprotic acids 72. which of the following concentrations would be practically equal in a calculation of the equilibrium concentrations in a 0. 134 - m solution of h2co3, a diprotic acid : [ oh− ], [ h2co3 ], no calculations are needed to answer this question. 73. calculate the concentration of each species pres... | openstax_chemistry2e-web | [
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4. 2 10−13 for the −oh group. what is the ph of a saturated solution of the acid ( solubility = 1. 8 g / l ). ( b ) aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. aspirin is acetylsalicylic acid, ch3co2c6h4co2h. the −co2h funct... | openstax_chemistry2e-web | [
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14. 6 buffers 77. explain why a buffer can be prepared from a mixture of nh4cl and naoh but not from nh3 and naoh. 78. explain why the ph does not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the acid h3po4 and a salt of its conjugate base nah2po4. ... | openstax_chemistry2e-web | [
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) nh3 ( c ) hi ( d ) naoh ( e ) nh4cl 86. what will be the ph of a buffer solution prepared from 0. 20 mol nh3, 0. 40 mol nh4no3, and just enough water to give 1. 00 l of solution? 87. calculate the ph of a buffer solution prepared from 0. 155 mol of phosphoric acid, 0. 250 mole of kh2po4, and enough water to make 0. 5... | openstax_chemistry2e-web | [
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1. 80 10−5 as ka for acetic acid. ( a ) what is the ph of the solution? ( b ) is the solution acidic or basic? ( c ) what is the ph of a solution that results when 3. 00 ml of 0. 034 m hcl is added to 0. 200 l of the original buffer? 91. a 5. 36 – g sample of nh4cl was added to 25. 0 ml of 1. 00 m naoh and the resultin... | openstax_chemistry2e-web | [
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... |
14. 7 acid - base titrations 92. explain how to choose the appropriate acid - base indicator for the titration of a weak base with a strong acid. 93. explain why an acid - base indicator changes color over a range of ph values rather than at a specific ph. 94. calculate the ph at the following points in a titration of ... | openstax_chemistry2e-web | [
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15. 3 coupled equilibria the mineral fluorite, caf2 figure 15. 1, is commonly used as a semiprecious stone in many types of jewelry because of its striking appearance. deposits of fluorite are formed through a process called hydrothermal precipitation in which calcium and fluoride ions dissolved in groundwater combine ... | openstax_chemistry2e-web | [
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15. 1 precipitation and dissolution learning objectives by the end of this section, you will be able to : • write chemical equations and equilibrium expressions representing solubility equilibria • carry out equilibrium computations involving solubility, equilibrium expressions, and solute concentrations solubility equ... | openstax_chemistry2e-web | [
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concentration of its dissolved ions in the solution is relatively low. figure 15. 2 silver chloride is a sparingly soluble ionic solid. when it is added to water, it dissolves slightly and produces a mixture consisting of a very dilute solution of ag + and cl – ions in equilibrium with undissolved silver chloride. the ... | openstax_chemistry2e-web | [
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may be simply related to its measured solubility provided the dissolution process involves only dissociation and solvation, for example : for cases such as these, one may derive ksp values from provided solubilities, or vice - versa. calculations of this sort are most conveniently performed using a compound ’ s molar s... | openstax_chemistry2e-web | [
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8. 99 10 – 12 example 15. 3 determination of molar solubility from ksp the ksp of copper ( i ) bromide, cubr, is 6. 3 10 – 9. calculate the molar solubility of copper bromide. solution the dissolution equation and solubility product expression are following the ice approach to this calculation yields the table substitu... | openstax_chemistry2e-web | [
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1. 2 10 – 8 m 752 15 • equilibria of other reaction classes access for free at openstax. org example 15. 4 determination of molar solubility from ksp the ksp of calcium hydroxide, ca ( oh ) 2, is 1. 3 10 – 6. calculate the molar solubility of calcium hydroxide. solution the dissolution equation and solubility product e... | openstax_chemistry2e-web | [
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15. 1 • precipitation and dissolution 753 figure 15. 3 oil paints contain pigments that are very slightly soluble in water. in addition to chrome yellow ( pbcro4 ), examples include prussian blue ( fe7 ( cn ) 18 ), the reddish - orange color vermilion ( hgs ), and green color veridian ( cr2o3 ). ( credit : sonny abesam... | openstax_chemistry2e-web | [
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1. 69 10 – 4 example 15. 6 calculating the solubility of hg2cl2 calomel, hg2cl2, is a compound composed of the diatomic ion of mercury ( i ), and chloride ions, cl –. although most mercury compounds are now known to be poisonous, eighteenth - century physicians used calomel as a medication. their patients rarely suffer... | openstax_chemistry2e-web | [
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1. 2 10 – 3 m how sciences interconnect using barium sulfate for medical imaging various types of medical imaging techniques are used to aid diagnoses of illnesses in a noninvasive manner. one such technique utilizes the ingestion of a barium compound before taking an x - ray image. a suspension of barium sulfate, a ch... | openstax_chemistry2e-web | [
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15. 1 • precipitation and dissolution 755 figure 15. 4 a suspension of barium sulfate coats the intestinal tract, permitting greater visual detail than a traditional x - ray. ( credit modification of work by “ glitzy queen00 ” / wikimedia commons ) medical imaging using barium sulfate can be used to diagnose acid reflu... | openstax_chemistry2e-web | [
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predictive strategy and related calculations are demonstrated in the next few example exercises. 756 15 • equilibria of other reaction classes access for free at openstax. org example 15. 7 precipitation of mg ( oh ) 2 the first step in the preparation of magnesium metal is the precipitation of mg ( oh ) 2 from sea wat... | openstax_chemistry2e-web | [
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the mixture of agno3 and nacl is greater than ksp. because the volume doubles when equal volumes of agno3 and nacl solutions are mixed, each concentration is reduced to half its initial value the reaction quotient, q, is greater than ksp for agcl, so a supersaturated solution is formed : agcl will precipitate from the ... | openstax_chemistry2e-web | [
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15. 1 • precipitation and dissolution 757 answer : no, q = 4. 0 10 – 3, which is less than ksp = 1. 05 10 – 2 example 15. 9 precipitation of calcium oxalate blood will not clot if calcium ions are removed from its plasma. some blood collection tubes contain salts of the oxalate ion, for this purpose ( figure 15. 5 ). a... | openstax_chemistry2e-web | [
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6. 7 10 – 5 m example 15. 10 concentrations following precipitation clothing washed in water that has a manganese [ mn2 + ( aq ) ] concentration exceeding 0. 1 mg / l ( 1. 8 10 – 6 m ) may be stained by the manganese upon oxidation, but the amount of mn2 + in the water can be decreased by adding a base to precipitate m... | openstax_chemistry2e-web | [
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10. 97 in solutions containing two or more ions that may form insoluble compounds with the same counter ion, an experimental strategy called selective precipitation may be used to remove individual ions from solution. by increasing the counter ion concentration in a controlled manner, ions in solution may be precipitat... | openstax_chemistry2e-web | [
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15. 1 • precipitation and dissolution 759 example 15. 11 precipitation of silver halides a solution contains 0. 00010 mol of kbr and 0. 10 mol of kcl per liter. agno3 is gradually added to this solution. which forms first, solid agbr or solid agcl? solution the two equilibria involved are : chemistry in everyday life t... | openstax_chemistry2e-web | [
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used for the removal of phosphates by precipitation, including iron ( iii ) chloride and aluminum sulfate. view this site ( http : / / openstax. org / l / 16wastewater ) for more information on how phosphorus is removed from wastewater. 760 15 • equilibria of other reaction classes access for free at openstax. org if t... | openstax_chemistry2e-web | [
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= 1. 0 10 – 11 m ; agbr precipitates first common ion effect compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion ( one also produced by dissolution of the ionic compound ). this is an example of a phenomenon known as the common ion effect, which is a conseq... | openstax_chemistry2e-web | [
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15. 1 • precipitation and dissolution 761 example 15. 12 common ion effect on solubility what is the effect on the amount of solid mg ( oh ) 2 and the concentrations of mg2 + and oh – when each of the following are added to a saturated solution of mg ( oh ) 2? ( a ) mgcl2 ( b ) koh ( c ) nano3 ( d ) mg ( oh ) 2 solutio... | openstax_chemistry2e-web | [
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appreciable effect ; ( c ) no effect except to increase the amount of solid nico3 ; ( d ) mass of nico3 ( s ) increases, [ ni2 + ] decreases, increases ; 762 15 • equilibria of other reaction classes access for free at openstax. org example 15. 13 common ion effect calculate the molar solubility of cadmium sulfide ( cd... | openstax_chemistry2e-web | [
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15. 2 lewis acids and bases learning objectives by the end of this section, you will be able to : • explain the lewis model of acid - base chemistry • write equations for the formation of adducts and complex ions • perform equilibrium calculations involving formation constants in 1923, g. n. lewis proposed a generalize... | openstax_chemistry2e-web | [
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15. 2 • lewis acids and bases 763 reactions involving the formation of coordinate covalent bonds are classified as lewis acid - base chemistry. the species donating the electron pair that compose the bond is a lewis base, the species accepting the electron pair is a lewis acid, and the product of the reaction is a lewi... | openstax_chemistry2e-web | [
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a pair of electrons to the central atom. these types of lewis acid - base reactions are examples of a broad subdiscipline called coordination chemistry — the topic of another chapter in this text. the equilibrium constant for the reaction of a metal ion with one or more ligands to form a coordination complex is called ... | openstax_chemistry2e-web | [
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15. 2 • lewis acids and bases 765 product of agcl : more silver chloride then dissolves. if the concentration of ammonia is great enough, all of the silver chloride dissolves. example 15. 14 dissociation of a complex ion calculate the concentration of the silver ion in a solution that initially is 0. 10 m with respect ... | openstax_chemistry2e-web | [
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15. 3 coupled equilibria learning objectives by the end of this section, you will be able to : • describe examples of systems involving two ( or more ) coupled chemical equilibria • calculate reactant and product concentrations for coupled equilibrium systems as discussed in preceding chapters on equilibrium, coupled e... | openstax_chemistry2e-web | [
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food chain starts to collapse. ( credit a : modification of work by noaa photo library ; credit b : modification of work by | openstax_chemistry2e-web | [
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15. 3 • coupled equilibria 767 “ prilfish ” / flickr ) link to learning learn more about ocean acidification ( http : / / openstax. org / l / 16acidicocean ) and how it affects other marine creatures. this site ( http : / / openstax. org / l / 16coralreef ) has detailed information about how ocean acidification specifi... | openstax_chemistry2e-web | [
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##oride : the weak base fluoride ion reacts only partially with the bacterial acid waste, resulting in a less extensive shift in the solubility equilibrium and an increased resistance to acid dissolution. see the chemistry in everyday life feature on the role of fluoride in preventing tooth decay for more information. ... | openstax_chemistry2e-web | [
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9 fluoride, found in many toothpastes, helps prevent tooth decay ( credit : kerry ceszyk ). unfortunately, excess fluoride can negate its advantages. natural sources of drinking water in various parts of the world have varying concentrations of fluoride, and places where that concentration is high are prone to certain ... | openstax_chemistry2e-web | [
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15. 3 • coupled equilibria 769 solution ( a ) the molar solubility of aluminum hydroxide in water is computed considering the dissolution equilibrium only as demonstrated in several previous examples : ( b ) the concentration of hydroxide ion of the buffered solution is conveniently calculated by the henderson - hassel... | openstax_chemistry2e-web | [
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0. 1 m example 15. 16 multiple equilibria unexposed silver halides are removed from photographic film when they react with sodium thiosulfate ( na2s2o3, called hypo ) to form the complex ion ( kf = 4. 7 1013 ). what mass of na2s2o3 is required to prepare 1. 00 l of a solution that will dissolve 1. 00 g of agbr by the f... | openstax_chemistry2e-web | [
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. 7 107. what mass of nh3 is required to prepare 1. 00 l of solution that will dissolve 2. 00 g of agcl by formation of answer : 1. 00 l of a solution prepared with 4. 81 g nh3 dissolves 2. 0 g of agcl. | openstax_chemistry2e-web | [
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15. 3 • coupled equilibria 771 key terms common ion effect effect on equilibrium when a substance with an ion in common with the dissolved species is added to the solution ; causes a decrease in the solubility of an ionic species, or a decrease in the ionization of a weak acid or base complex ion ion consisting of a ce... | openstax_chemistry2e-web | [
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15. 1 precipitation and dissolution the equilibrium constant for an equilibrium involving the precipitation or dissolution of a slightly soluble ionic solid is called the solubility product, ksp, of the solid. for a heterogeneous equilibrium involving the slightly soluble solid mpxq and its ions mm + and xn – : the sol... | openstax_chemistry2e-web | [
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free at openstax. org exercises | openstax_chemistry2e-web | [
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15. 1 precipitation and dissolution 1. complete the changes in concentrations for each of the following reactions : ( a ) ( b ) ( c ) ( d ) ( e ) 2. complete the changes in concentrations for each of the following reactions : ( a ) ( b ( c ) ( d ) ( e ) 3. how do the concentrations of ag + and in a saturated solution a... | openstax_chemistry2e-web | [
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##3 ( c ) ag2so4 ( d ) pb ( oh ) 2 10. the handbook of chemistry and physics ( http : / / openstax. org / l / 16handbook ) gives solubilities of the following compounds in grams per 100 ml of water. because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate th... | openstax_chemistry2e-web | [
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of each of the following from its solubility product : ( a ) khc4h4o6 ( b ) pbi2 ( c ) ag4 [ fe ( cn ) 6 ], a salt containing the ion ( d ) hg2i2 14. assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product : ( a ) ag2so4 ( b ) ... | openstax_chemistry2e-web | [
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##cro4 ( d ) cd ( oh ) 2 ( s ) in a solution buffered at a ph of 10. 995 17. assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. show that it is not appropriate ... | openstax_chemistry2e-web | [
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1. 00 l of water saturated with baso4. 23. public health service standards for drinking water set a maximum of 250 mg / l ( 2. 60 10 – 3 m ) of because of its cathartic action ( it is a laxative ). does natural water that is saturated with caso4 ( “ gyp ” water ) as a result or passing through soil containing gypsum, c... | openstax_chemistry2e-web | [
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e ) the mineral brucite, mg ( oh ) 2 15 • exercises 775 28. the following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. from the concentrations given, calculate ksp for each of the slightly soluble solids indicated : ( a ) agbr : [ ag + ] = 5. 7 10 – 7 m, [ br – ] = 5. 7 10 –... | openstax_chemistry2e-web | [
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6 10−8 m 30. which of the following compounds precipitates from a solution that has the concentrations indicated? ( see appendix j for ksp values. ) ( a ) kclo4 : [ k + ] = 0. 01 m, = 0. 01 m ( b ) k2ptcl6 : [ k + ] = 0. 01 m, = 0. 01 m ( c ) pbi2 : [ pb2 + ] = 0. 003 m, [ i – ] = 1. 3 10 – 3 m ( d ) ag2s : [ ag + ] = ... | openstax_chemistry2e-web | [
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0. 0758 m in ba2 +. 34. calculate the concentration of sr2 + when srcro4 starts to precipitate from a solution that is 0. 0025 m in cro42 –. 35. calculate the concentration of when ag3po4 starts to precipitate from a solution that is 0. 0125 m in ag +. 36. calculate the concentration of f – required to begin precipitat... | openstax_chemistry2e-web | [
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staining. what [ oh – ] is required to reduce [ fe2 + ] to this level by precipitation of fe ( oh ) 2? 43. a solution is 0. 010 m in both cu2 + and cd2 +. what percentage of cd2 + remains in the solution when 99. 9 % of the cu2 + has been precipitated as cus by adding sulfide? 44. a solution is 0. 15 m in both pb2 + an... | openstax_chemistry2e-web | [
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0.006439453922212124,
0.053265150636434555,
0.010245449841022491,
-0.07455913722515106,
0.0023755268193781376,
0.0033020400442183018,
0.00524178659543395,
0.02053641527891159,
0.04284154996275902,
0.015786945819854736,
-0.01960194669663906,
0.034578729420900345,
-0.02... |
anticoagulant when a blood sample is drawn for laboratory tests because it removes the calcium as a precipitate of cac2o4 · h2o. it is necessary to remove all but 1. 0 % of the ca2 + in serum in order to prevent coagulation. if normal blood serum with a buffered ph of 7. 40 contains 9. 5 mg of ca2 + per 100 ml of serum... | openstax_chemistry2e-web | [
-0.014527284540235996,
0.019582664594054222,
0.052900198847055435,
0.03040642850100994,
-0.08247212320566177,
0.02673080377280712,
0.005408519878983498,
0.03882482275366783,
0.020045340061187744,
0.03124920465052128,
0.045795686542987823,
-0.02326357550919056,
0.01164707075804472,
-0.02824... |
mg2 + ( aq ) by mass. what mass, in kilograms, of ca ( oh ) 2 is required to precipitate 99. 9 % of the magnesium in 1. 00 103 l of sea water? 52. hydrogen sulfide is bubbled into a solution that is 0. 10 m in both pb2 + and fe2 + and 0. 30 m in hcl. after the solution has come to equilibrium it is saturated with h2s (... | openstax_chemistry2e-web | [
0.019109230488538742,
0.045263536274433136,
0.05282782018184662,
0.02559337392449379,
-0.06119213253259659,
-0.0028121713548898697,
0.013997011817991734,
0.02896040864288807,
0.01957026869058609,
0.02197999879717827,
0.0016165082342922688,
0.0040371231734752655,
0.03744301572442055,
-0.038... |
777 57. how many grams of milk of magnesia, mg ( oh ) 2 ( s ) ( 58. 3 g / mol ), would be soluble in 200 ml of water. ksp = | openstax_chemistry2e-web | [
0.007835015654563904,
0.0029995457734912634,
0.032011739909648895,
0.05826667696237564,
-0.046253230422735214,
0.010471685789525509,
0.04063543304800987,
0.046671055257320404,
-0.013570901937782764,
0.04425773769617081,
0.03254294767975807,
0.01572497747838497,
-0.0015427072066813707,
-0.0... |
7. 1 10 – 12. include the ionic reaction and the expression for ksp in your answer. ( kw = 1 10 – 14 = [ h3o + ] [ oh – ] ) 58. two hypothetical salts, lm2 and lq, have the same molar solubility in h2o. if ksp for lm2 is 3. 20 10 – 5, what is the ksp value for lq? 59. the carbonate ion concentration is gradually increa... | openstax_chemistry2e-web | [
-0.005555855575948954,
0.04405934736132622,
0.06559193879365921,
0.04439633712172508,
-0.06947392225265503,
0.020873306319117546,
0.003310962114483118,
0.009369712322950363,
-0.006186401937156916,
0.034484509378671646,
0.021352238953113556,
0.009463449008762836,
0.007612001150846481,
-0.03... |
15. 2 lewis acids and bases 61. even though ca ( oh ) 2 is an inexpensive base, its limited solubility restricts its use. what is the ph of a saturated solution of ca ( oh ) 2? 62. under what circumstances, if any, does a sample of solid agcl completely dissolve in pure water? 63. explain why the addition of nh3 or hno... | openstax_chemistry2e-web | [
0.012277795933187008,
0.02528280019760132,
0.07073022425174713,
0.019392233341932297,
-0.07409752160310745,
0.010270285420119762,
-0.01189229916781187,
0.03737277537584305,
0.0077023920603096485,
0.062386639416217804,
0.042934171855449677,
-0.0009910749504342675,
0.02664315700531006,
-0.04... |
the dissociation constant, kd = 1 10 – 44, calculate the equilibrium concentrations of fe3 + and cn – in a 0. 333 m solution of 72. calculate the mass of potassium cyanide ion that must be added to 100 ml of solution to dissolve 2. 0 10 – 2 mol of silver cyanide, agcn. 73. calculate the minimum concentration of ammonia... | openstax_chemistry2e-web | [
0.006668151821941137,
0.005627068690955639,
0.021702228114008904,
0.010239960625767708,
-0.05455140769481659,
0.004939439706504345,
0.014732910320162773,
0.013484190218150616,
-0.0070709954015910625,
0.04272712767124176,
0.036432329565286636,
-0.006026383023709059,
-0.0014967918395996094,
... |
the following equations, and identify the lewis acid and the lewis base in each : ( a ) ( b ) ( c ) ( d ) ( e ) 78. using lewis structures, write balanced equations for the following reactions : ( a ) ( b ) ( c ) ( d ) 79. calculate in a solution prepared by adding 0. 0200 mol of nacl to 0. 250 l of a 0. 100 - m hgcl2 ... | openstax_chemistry2e-web | [
0.03456033766269684,
0.03668989986181259,
0.06062405928969383,
0.01605081371963024,
-0.04150358587503433,
0.005137828644365072,
0.020097222179174423,
0.01818145252764225,
-0.005901542026549578,
0.06388408690690994,
0.030388163402676582,
0.026385784149169922,
0.008503985591232777,
-0.056779... |
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