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Question: <p>Adding acids or bases to water, so that either pH or pOH decreases independently of the other, will that affect the auto-ionization of water? For example, pure water + auto-ionized state, with some base added to remove some protons, will it auto-ionize a bit more (create more H+ and OH-) or a bit less (rem... | https://chemistry.stackexchange.com/questions/129275/auto-ionization-equilibrium-of-water-shifted-with-acid-base-addition |
Question: <p>I learned that </p>
<p>a) the conjugate base to a weak acid is a strong base (and vice versa).</p>
<p>b) a buffer consists of a weak acid (base) and its conjugate base (acid). </p>
<p>However, <a href="http://chemcollective.org/activities/tutorials/buffers/buffers3" rel="nofollow">this</a> explanation o... | https://chemistry.stackexchange.com/questions/55059/confused-about-weak-strong-acids-conjugated-acid-base-pairs-and-buffers |
Question: <p>This question came up in figuring out what the fundamental differences are between redox chemistry and acid/base chemistry (if any).</p>
<p>In redox chemistry, strong oxidants and strong reductants can co-exist in solution because they react slowly with each other (or not at all). An example from biology ... | https://chemistry.stackexchange.com/questions/133203/are-there-acid-base-processes-in-aqueous-solution-that-are-so-slow-that-they-are |
Question: <p>I was looking at acid-base equilibria of weak acids and weak bases. To determine the equilibrium constant of a reaction of those, I found a formula on the libretexts page:</p>
<p><a href="https://i.sstatic.net/ndfSk.png" rel="nofollow noreferrer"><img src="https://i.sstatic.net/ndfSk.png" alt="enter image ... | https://chemistry.stackexchange.com/questions/168215/predicting-acid-base-equilibria |
Question: <p>I'm in high school chemistry and just learning about buffer solutions. For example, given a buffered solution of <span class="math-container">$\ce{CH3COOH}$</span> and <span class="math-container">$\ce{NaCH3COO}$</span> with <span class="math-container">$K_a = 1.8 \times 10^{-5}$</span>, we might want to f... | https://chemistry.stackexchange.com/questions/111957/which-acid-base-does-a-strong-base-acid-react-when-added-to-a-buffer-solution |
Question: <p>Fluorides such as <span class="math-container">$\ce{CaF2}$</span> or <span class="math-container">$\ce{LiF}$</span> are sparingly soluble in water. Does their solubility product constant <span class="math-container">$K_\text{sp}$</span> about the equilibrium of</p>
<p><span class="math-container">$$\ce{Ca... | https://chemistry.stackexchange.com/questions/188551/competing-solubility-and-acid-base-equilibria |
Question: <p>The system is an aqueous solution of sulfuric acid and sulfur dioxide. I know how much sulfur there is and I know the pH. The system is in equilibrium. I would like to use Octave to solve the system.</p>
<p>I set up the following equations, ignoring $\ce{SO3^2-}$ because the pH is around 1.5.</p>
<p>By... | https://chemistry.stackexchange.com/questions/34924/how-to-find-the-concentrations-of-the-acid-base-equilibrium-between-sulfuric-aci |
Question: <blockquote>
<p>Acetic acid has a <span class="math-container">$K_\mathrm{a}$</span> of <span class="math-container">$\pu{1.8e-5}$</span>. What is the equilibrium constant for the neutralization of this acid with <span class="math-container">$\ce{NaOH}$</span>?</p>
</blockquote>
<p>Given acetic acid</p>
<... | https://chemistry.stackexchange.com/questions/109948/equilibrium-constant-for-the-neutralization-of-weak-acid-by-strong-base |
Question: <p>Today I stumbled across a website which defined the titration of weak acid and strong base as the following:</p>
<p>"The titration of a weak acid with a strong base involves the direct transfer of protons from the weak acid to the hydoxide ion. The reaction of the weak acid, acetic acid, with a strong... | https://chemistry.stackexchange.com/questions/158751/understanding-weak-acid-strong-base-titration |
Question: <p>Since $\ce{HCl}$ is more acidic than $\ce{HF}$, the left hand side of a reaction has a stronger acid than the right hand side.</p>
<p>Since $\ce{NaF}$ is more basic than $\ce{NaCl}$, the left hand side has a stronger base relative to the right hand side.</p>
<p>$$\begin{align}\text{Stronger Acid/Base} &a... | https://chemistry.stackexchange.com/questions/39406/how-to-estimate-the-equilibrium-constant-of-the-reaction-between-naf-and-hcl |
Question: <p>To be honest, I just don't get it.
I had this question while reading a Chemguide article, on this topic:
<img src="https://i.sstatic.net/AMrse.jpg" alt="enter image description here"></p>
<p>I think my confusion is caused by the way I look at pKa of acid-base indicator. Should you think of it more as a re... | https://chemistry.stackexchange.com/questions/29697/why-does-pka-of-a-acid-base-indicator-equal-to-the-ph-when-the-equivalence-point |
Question: <p>a) Differences in solvent</p>
<p>b) Acid base equilibrium (differences of pH)</p>
<p>c) Parasitic or stray radiation</p>
<p>d) Monochromatic radiation</p>
<p>I have some doubts about pH in spectrophotometry. I'm not sure if it is correct but here is what I thought:</p>
<p>a)Differences in solvent. It can b... | https://chemistry.stackexchange.com/questions/145857/which-of-the-following-can-be-a-source-of-error-in-spectrophotometry-mark-the-w |
Question: <p>So we know that $K_\mathrm w$ is $10^{-14}$. But what if I am working with non-aqueous systems? Suppose I were to add LDA to liquid ammonia, or dissolve HCl in concentrated sulfuric acid. How would I calculate the percentage of dissociation? I have some inkling of how to do this but I don't really see disc... | https://chemistry.stackexchange.com/questions/85644/how-to-calculate-he-equilibrium-constant-change-for-acid-base-reactions-in-a-dif |
Question: <p>Take the following simple equilibrium:
$$\ce{CH3COOH + H2O <=> H3O+ + CH3COO-}$$</p>
<p>Ethanoic acid will act as a typical Brønsted-Lowry acid and donate a proton to water, forming a conjugate acid-base pair. In this case, H<sub>3</sub>O<sup>+</sup> is the conjugate acid, and CH<sub>3</sub>COO<sup>... | https://chemistry.stackexchange.com/questions/99890/a-simple-equilibrium-problem |
Question: <p>I'm going back through my notes from a chemistry class, which I did well in despite not having a very good conceptual understanding, in order to hopefully develop that understanding, but there's something I can't find in the book or online. Why is it that, when solving for the pH of a solution that results... | https://chemistry.stackexchange.com/questions/134540/what-actually-happens-in-strong-acid-weak-base-reactions |
Question: <p>For example, in the reaction $\ce{NaOH +HCl->NaCl +H_2O}$, the products are favoured by a factor of approximately $10^{24}$.
Is this a general rule? Is it because the products are more stable than the reactants?</p>
Answer: <p>Here is a simple intuitive explanation. In your above example, there is actu... | https://chemistry.stackexchange.com/questions/38831/why-does-equilibrium-favour-weak-acid-or-weak-base |
Question: <p>How would you know when an acid or base is paired with <span class="math-container">$\ce{H2O}$</span> that it will form an <span class="math-container">$\ce{OH-}$</span> ion or a <span class="math-container">$\ce{H3O+}$</span> ion? I just started the acid and base equilibrium unit, and I'm just confused on... | https://chemistry.stackexchange.com/questions/147865/determine-which-ion-h3o-or-oh-is-in-excess-at-the-end-of-the-reaction |
Question: <p>When a buffer (for example, a mixture of 100 mM acetic acid and 100 mM acetate), is diluted 10-fold, all the concentrations change drastically. Surprisingly, after re-establishment of equilibrium, the pH is not much different from the starting pH.</p>
<p>How can you visualize how diluting a buffer disturb... | https://chemistry.stackexchange.com/questions/109968/what-are-the-concentration-changes-when-diluting-an-equimolar-acetic-acid-aceta |
Question: <p>I have a question concerning acid/base reactions. Is it true that an alcohol is a better base than water?
My Professor listed the basicity (because we talked about E1/E2 and Sn1/Sn2 reactions) of the following compounds the following way: RO- > OH- > ROH > H2O (with stronger base being the RO- and... | https://chemistry.stackexchange.com/questions/145185/base-acid-reaction-alcohol-amphoteric-why-no-pkb-value |
Question: <p>Suppose I had an acid HA, and it reaches equilibrium in water. Then I remove the hydronium ions. I don't know how I would do this, maybe adding some hydroxide ions. My question is can I do this and will I be able to eventually create a 50/50 mixture of acid and conjugate base? Is this a very good buffer?</... | https://chemistry.stackexchange.com/questions/27146/what-happens-if-i-have-an-acid-base-equillibrium-and-remove-hydronium-ions-until |
Question: <blockquote>
<p>An example of a solution not in equilibrium<br>
(A) Chemical ph
indicator<br>
(B) Acid/base buffer<br>
(C) Anhydrous solution<br>
(D)
hypotonic solution<br>
(E) Supersaturated solution</p>
</blockquote>
<p>I eliminated A and B. Then, I chose E, which is a right answer. Noneth... | https://chemistry.stackexchange.com/questions/81550/what-solution-is-not-in-equilibrium |
Question: <p>For example, is 3M HCl a stronger acid than 1M HCl? </p>
<p>I would reason that the concentration of an acid/base does not influence its strength. Strength is determined by the pKa, and, as per Le Chatelier's Principle, the initial concentration does not influence the equilibrium constant. </... | https://chemistry.stackexchange.com/questions/105242/does-concentration-or-pka-define-acid-strength |
Question: <p>If I dissolve the weak acid HCN into water, I get a solution of oxonium and CN ions and since there is an equilibrium there is more HCN left.</p>
<p>So I thought CN ions can consequently react with water to form hydroxide-ions, which is a weak base-reaction, by which we also get the original HCN molecules... | https://chemistry.stackexchange.com/questions/123428/how-do-you-know-is-a-solution-is-acid-or-basic-when-you-dissolve-a-weak-acid-bas |
Question: <p>This is from Laitinen and Harris, "Chemical Analysis, An Advanced Text & Reference" which describes a simple acid-base equilibrium. They derive a relation in the end directly. I haven't seen this expression in many books which teach solution equilibria. The authors cite an article from the Journal of C... | https://chemistry.stackexchange.com/questions/131643/algebraic-treatment-of-equilibrium |
Question: <p>Some substances disproportionate. This means a species with an intermediate oxidation state yields two species with higher and lower oxidation state. For example:</p>
<p><span class="math-container">$$\ce{Hg2Cl2 -> Hg + HgCl2}$$</span></p>
<p>My question is if there are substance that have the analogo... | https://chemistry.stackexchange.com/questions/133202/in-acid-base-chemistry-are-there-amphoteric-substances-that-undergo-something-t |
Question: <p>You perform a titration of an acid (let's say <span class="math-container">$\pu{20 ml}$</span> <span class="math-container">$\ce{CH_3COOH}$</span>) with a base (let's say <span class="math-container">$\pu{0.5 M}$</span> <span class="math-container">$\ce{NaOH}$</span>). The burette is marked at <span class=... | https://chemistry.stackexchange.com/questions/171766/calculating-error-in-acid-base-titration |
Question: <p>Say you have Ammonium Formate in solution, the salt formed by the reaction of Formic Acid and Ammonia. Would both the Formate ion and Ammonium ion protonate and deprotonate, respectively, to form their conjugates until equilibrium is reached? I would also assume that one of the ions would form more of th... | https://chemistry.stackexchange.com/questions/82959/how-do-salts-of-a-weak-acid-weak-base-behave-in-solution |
Question: <p>When a neutralisation reaction happens, for example, <span class="math-container">$ \pu{100 mol l^-1}$</span> of <span class="math-container">$\ce{HCl}$</span> with <span class="math-container">$\pu{100 mol l^-1}$</span> <span class="math-container">$\ce{NH_3}$</span>, why does <em>all</em> of the base and... | https://chemistry.stackexchange.com/questions/22208/why-do-acids-usually-completely-react-with-bases |
Question: <blockquote>
<p>Which of the following statements best characterizes the difference between the titration of a strong acid with a strong base and that of the titration of a weak acid with a strong base?</p>
<p>A) Both the strong acid and the strong base are completely dissociated in solution whereas th... | https://chemistry.stackexchange.com/questions/4081/what-is-the-difference-between-the-titration-of-a-strong-acid-with-a-strong-base |
Question: <p>I'm wondering if reactions that involve a weak acid and a weak base go to completion. For example, say we have equal amounts and equal volumes of acetic acid and ammonia being mixed together. Would this neutralisation reaction go to completion or would it reach a state of equilibrium?</p>
<p>$\ce{NH_3 + C... | https://chemistry.stackexchange.com/questions/83429/do-weak-acid-weak-base-neutralisation-reactions-go-to-completion |
Question: <p>Compounds, commonly used as <a href="https://en.wikipedia.org/wiki/PH_indicator" rel="nofollow noreferrer">pH-indicators</a>, are soluble in aqueous media and polar solvents (DMSO, DMF, NMP etc.) and are functional pretty much across all these solvents. However, practically none these indicators are solubl... | https://chemistry.stackexchange.com/questions/87521/what-ph-indicators-are-commonly-used-for-non-polar-medium |
Question: <blockquote>
<p><strong>Question</strong><br>
Predict the products of the following acid-base reactions, and predict whether the equilibrium lies to the left or to the right of the equations
$$\ce{NO2- + H2O -> ?}$$</p>
</blockquote>
<p>I thought it would be $\ce{NO2- + H2O -> HNO2 + OH-}$, but m... | https://chemistry.stackexchange.com/questions/8862/why-isnt-nitrous-acid-a-product-of-nitrite-and-water |
Question: <p>Doesn’t the weak acid dissociate to produce the conjugate base on its own? </p>
<p>I understand that when a strong base is added to the buffer solution, the hydroxide ions will react with the hydrogen ions formed via the dissociation of the weak acid. The equilibrium position will shift rightwards to repl... | https://chemistry.stackexchange.com/questions/105646/why-must-a-buffer-solution-contain-both-a-weak-acid-and-a-salt-solution-of-its-c |
Question: <h2>Context</h2>
<p>The Henderson-Hasselbalch equation is as follows. $$pH=-\log\big(K_a\big)+\log\bigg(\frac{[A^-]}{[HA]}\bigg)$$ One may follow <a href="https://en.wikipedia.org/wiki/Henderson%E2%80%93Hasselbalch_equation#Derivation" rel="nofollow noreferrer">its derivation</a> in order to understand how i... | https://chemistry.stackexchange.com/questions/99538/eqpt-ph-of-a-monoprotic-acid-base-titration-product-of-molarites-over-their-sum |
Question: <p>Consider a solution which contains a weak acid and the salt of its conjugate base with a strong base.
e.g. $$\ce{CH3COOH + H2O <=>[$K_\rm{a}$] CH3COO- + H3O+}\tag1$$
$$\ce{CH3COO- + H2O <=>[$K_\rm{h}$] CH3COOH + OH-}\tag2$$</p>
<p>Now, $\displaystyle{K_\rm{a} = \frac{[\ce{H3O+}] [\ce{CH3COO-}... | https://chemistry.stackexchange.com/questions/82963/why-is-the-hydrolysis-of-the-conjugate-base-of-a-weak-acid-neglected-in-buffer-s |
Question: <p>While solving for weak acid and weak base salt hydrolysis, why do we take the degree of hydrolysis for both the anion and cation to be the same?</p>
<p>If we assume they are the same, when solving for $K_\mathrm{a}$ and $K_\mathrm{b}$ for the cation and anion using simultaneous equilibrium, I always get t... | https://chemistry.stackexchange.com/questions/85650/weak-acid-and-weak-base-salt-hydrolysis |
Question: <p>I was solving a question of salt hydrolysis for a mixture of Weak Acid-Base Salts, given the initial amount of salt and Equilibrium constants. I was trying to approach the problem in two ways, Assuming initially that we have all reactants and no products and move the reaction forward OR assuming all the re... | https://chemistry.stackexchange.com/questions/152689/is-equilibrium-point-for-a-coupled-equilibria-of-arbitary-number-of-coupled-reac |
Question: <p>Consider a buffer solution containing a weak acid and its conjugate base (<span class="math-container">$c_\mathrm{total} = \pu{0.1 mol L-1}$</span>):
<span class="math-container">$$\ce{HA <=> H^+ + A^-}$$</span></p>
<p>When <span class="math-container">$\ce{H+}$</span> ions are added (from a strong a... | https://chemistry.stackexchange.com/questions/153741/how-exactly-does-a-buffer-made-up-of-a-weak-acid-and-its-conjugate-base-work-upo |
Question: <p>Metals in low Oxidation states are usually reducing agents. Is there any example of a metal in zero Oxidation state acting as an oxidizing agent. </p>
Answer: <p>As with pretty much every "is there ______?" in chemistry, the answer is yes, there is.</p>
<p>Of course, using the pure <em>metal</em> itself ... | https://chemistry.stackexchange.com/questions/68558/oxidation-states |
Question: <p>which of the statements is true:</p>
<ol>
<li><p>looking at the electronic configuration of an element, can the possible oxidation states/oxidation number of an elemnet be predicted.
for example, the valence electronic configuration of nitrogen is 2s^2 2p^3. From this can we know all the possible oxidation... | https://chemistry.stackexchange.com/questions/147911/variable-oxidation-states |
Question: <p>I'm given a question:</p>
<blockquote>
<p>Oxidation number of $\ce{O}$ in $\ce{BaO2}$ is $x$ and in $\ce{OF2}$ is $y$; then the value of $x+y$
is what?</p>
</blockquote>
<p>Now my main question is that if $\ce{F}$ has $-1$ valency in $\ce{OF2}$ then $\ce{O}$ must have valency of $+2$. But is that po... | https://chemistry.stackexchange.com/questions/60961/oxidation-states-of-oxygen |
Question: <p>When I took high school chemistry many years ago, considerable effort was spent on teaching us to <em>compute</em> oxidation states of atoms in various compounds, following a set of rules that looked somewhat arbitrary to me at the time. As far as I remember, we were never told what benefits (other than pa... | https://chemistry.stackexchange.com/questions/61040/what-are-oxidation-states-used-for |
Question: <p>When going through list of oxidation states on <a href="https://en.m.wikipedia.org/wiki/List_of_oxidation_states_of_the_elements" rel="noreferrer">Wikipedia</a> I encounterd there that sodium, potassium, rubidium and caesium exhibit oxidation states of -1, but not lithium, even though its electronegativit... | https://chemistry.stackexchange.com/questions/109846/unusual-oxidation-states-of-alkali-metals |
Question: <p>I downloaded a periodic table app which gives detailed information for each element. The app shows some elements, however, have two different oxidation states. Hydrogen, for instance, can have either a 1+ or 1- state. What do these two states signify? Why do these elements have <em>more</em> than one oxida... | https://chemistry.stackexchange.com/questions/60679/elements-with-multiple-oxidation-states |
Question: <p>Palladium follows an exception to normal electron filling-up rules and so has the electron configuration of $\ce{[Kr] 4d^{10} 5s^0}$</p>
<p>The oxidation states of palladium are $\ce{+II}$ and $\ce{+IV}$.
How can these oxidation states be explained by looking at the special electron configuration of $\c... | https://chemistry.stackexchange.com/questions/7705/explaining-the-oxidation-states-of-palladium |
Question: <p><a href="https://i.sstatic.net/5huav.png" rel="nofollow noreferrer"><img src="https://i.sstatic.net/5huav.png" alt="enter image description here"></a></p>
<blockquote>
<p>I have noted down the available positive oxidation states of the first
row of transition elements (on the Periodic Table) from the ... | https://chemistry.stackexchange.com/questions/59926/anomalous-oxidation-states-of-transition-metals |
Question: <p><a href="https://i.sstatic.net/YjBmj.png" rel="nofollow noreferrer"><img src="https://i.sstatic.net/YjBmj.png" alt="enter image description here" /></a></p>
<p>I was given this question and don't understand why the two sulphur atoms have different oxidation states - and how to actually figure it out. Could... | https://chemistry.stackexchange.com/questions/178247/oxidation-states-of-thiosulphate |
Question: <p>Why does plutonium have more oxidation states than samarium?</p>
<p>Electron configuration of Pu: <span class="math-container">$\ce{[Rn] 5f^6 7s^2}$</span></p>
<p>Electron configuration of Sm: <span class="math-container">$\ce{[Xe] 4f^6 6s^2}$</span></p>
<p>I thought that only the valence electrons affecte... | https://chemistry.stackexchange.com/questions/7704/plutonium-having-more-oxidation-states-than-samarium |
Question: <p>According to <em><a href="https://en.wikipedia.org/wiki/List_of_oxidation_states_of_the_elements" rel="noreferrer">List of oxidation states of the elements</a></em>, silicon has a possible oxidation state of $-4$.</p>
<p><a href="https://i.sstatic.net/xpktm.jpg" rel="noreferrer"><img src="https://i.sstati... | https://chemistry.stackexchange.com/questions/37209/negative-oxidation-states-of-si |
Question: <p>Transition elements are good catalysts because they have multiple oxidation states?Why multiple oxidation states matter?</p>
Answer: <p>The answer has a lot to do with "what is a catalyst in the first place?"
A catalyst is a compound that can affect the rate of a chemical reaction
by providing an alternat... | https://chemistry.stackexchange.com/questions/28828/why-are-multiple-oxidation-states-useful-for-a-catalyst |
Question: <p>So, metal oxides are generally basic, right? But in higher oxidation states their covalent character is predominant. For example in
Mn2O7 the Mn - O bond is covalent. Why is that?</p>
Answer: <p>Metal oxides are not always basic. In many cases where the bonding is strongly ionic, the oxide ions do act as... | https://chemistry.stackexchange.com/questions/128634/covalency-of-metal-oxides-in-high-oxidation-states |
Question: <p>The CRC Elecrochemical Series and the solution to our exercise suggest that the oxidation states of borohydride are -V for Boron and +I for Hydrogen.</p>
<p>Since H (2.2) is more electronegativ than B (2.0), I would have expected the oxidation states to be +III for B and -I for H.</p>
<p>What am I missin... | https://chemistry.stackexchange.com/questions/14038/what-are-the-oxidation-states-in-borohydride-bh4 |
Question: <p>In p-block elements, higher oxidation states are less stable down the group due to the inert pair effect. This is not the case for transition metals.</p>
<p>Why do heavier transition metals show higher oxidation states than lighter ones? Is the inert pair effect not valid for transition metals also?</p>
... | https://chemistry.stackexchange.com/questions/67510/why-do-heavier-transition-metals-show-higher-oxidation-states |
Question: <p>USNCO 2004 Question 45 states:</p>
<blockquote>
<p>Which element exhibits the greatest number of oxidation
states in its compounds?</p>
<p>(A) Ca (B) V (C) Cu (D) As</p>
</blockquote>
<p>I ruled out Ca, as I know it only exists as +2. I then drew electron configurations for V, Cu and As. I ruled... | https://chemistry.stackexchange.com/questions/107718/comparing-the-number-of-oxidation-states-of-vanadium-and-arsenic |
Question: <p>For example, how could I calculate the oxidation state of lead in <span class="math-container">$\ce{PbS}$</span>? Or for that matter how would I calculate it for sulfur? Or I have two unknowns, for example sulfur in <span class="math-container">$\ce{PbSO4}$</span>? Do I assume that lead has a 2+ charge and... | https://chemistry.stackexchange.com/questions/129501/how-does-one-calculate-oxidation-states |
Question: <p>There are oxidation states from -4 to +8</p>
<p>Why do the negative oxidation states not go all the way down to -8? I mean if an atom is hypervalent meaning that it can have more than an octet than that means it can have potentially 8 bonds(counting a double bond as 2 bonds and a triple bond as 3 bonds re... | https://chemistry.stackexchange.com/questions/15337/why-do-negative-oxidation-states-not-extend-to-8 |
Question: <p>Why are fluorides of transition metals unstable in low oxidation states? </p>
<p>I would think that since fluorine and oxygen are highly electronegative, it's obvious that they be stable at high oxidation states. However, $\ce{Cl}$ is also highly electronegative, but it does exist in low oxidation state... | https://chemistry.stackexchange.com/questions/55778/why-are-fluorides-of-transition-metals-unstable-in-low-oxidation-states |
Question: <p>I have never seen anything other than a set of rules like these when textbooks present how to assign oxidation numbers. Such as these: </p>
<p><img src="https://i.sstatic.net/YlxeX.png" alt="enter image description here"></p>
<p>However, if we keep in mind that oxidation numbers are simply imaginary numb... | https://chemistry.stackexchange.com/questions/10944/electronegativity-considerations-in-assigning-oxidation-states |
Question: <p>How do you balance this using the ion-electron method;</p>
<p><span class="math-container">$\ce{CrO5 + H2SO4 -> Cr2(SO4)3 + H2O + O2}$</span></p>
<p>The oxygen has multiple oxidation states in <span class="math-container">$\ce{CrO5}$</span>, and none of the sites I looked this up on dealt with that.</... | https://chemistry.stackexchange.com/questions/129467/balancing-redox-equations-with-oxygens-in-multiple-oxidation-states |
Question: <p>As I understand, Roman numerals are used for oxidation states, whereas Arabic numerals are used for the charge of full ions, with some ambiguity allowed when a metal centre is all but ionised, such as in hexaaqua compounds.</p>
<p>But I have never seen a Roman numeral with a negative sign in front of it. ... | https://chemistry.stackexchange.com/questions/171876/can-you-write-oxidation-states-with-negative-roman-numerals |
Question: <p>I'm hoping someone can help me tighten up my understanding of the origins of the differences between Ni and Pd catalysis. </p>
<p>I understand that Ni has higher charge density and this is the reason for it's larger capacity for oxidative addition for say an aryl halide. It also has access to the oxidtaio... | https://chemistry.stackexchange.com/questions/111829/reactivity-of-ni-vs-pd-available-oxidation-states |
Question: <p>What are the oxidation states of the sulfur in the tetrathionate ion <span class="math-container">$\ce{S4O6^{2-}}$</span>?</p>
<p><a href="https://i.sstatic.net/l5kDW.png" rel="nofollow noreferrer"><img src="https://i.sstatic.net/l5kDW.png" alt="Structure"></a></p>
Answer: <p>Consider the structure of <a... | https://chemistry.stackexchange.com/questions/5643/what-are-the-oxidation-states-of-sulfur-in-the-tetrathionate-ion |
Question: <p><a href="https://i.sstatic.net/Szzjs.jpg" rel="nofollow noreferrer"><img src="https://i.sstatic.net/Szzjs.jpg" alt="enter image description here"></a></p>
<p>I) According to my logic, sulfur-sulfur linkage (linkage between same atoms) result in no charge separation.So, the oxidation number of the sulfur a... | https://chemistry.stackexchange.com/questions/71924/why-oxidation-states-of-suphur-atoms-of-disuphur-monoxide-is-2-and-0 |
Question: <p>In transition elements the oxidation states differ by one (+2 to +7 in Mn). However, in the p-block elements, the oxidation states differ by two (-1,+1,+3,+5 in the halogen group). Why is this so?</p>
Answer: <p>In d block, variable valency occurs due to small differences in successive ionization enthalpy... | https://chemistry.stackexchange.com/questions/44220/difference-in-the-change-in-oxidation-states-of-transition-elements-and-p-block |
Question: <p>Why do the elements in the middle of the transition series show more number of common oxidation states than others?</p>
<p><img src="https://2.bp.blogspot.com/-gl6AodOkf5c/VLPvPFYxBPI/AAAAAAAAA1M/YFFFFmXKHU0/s1600/variable-oxidation-states-of-transition-elements.JPG" alt="" /></p>
Answer: | https://chemistry.stackexchange.com/questions/168510/why-middle-elements-of-transition-series-show-more-number-of-oxidation-states |
Question: <p>Both osmium and iridium have 12 oxidation states. Indeed, iridium has the highest oxidation state of all elements at +9. see <a href="https://en.wikipedia.org/wiki/List_of_oxidation_states_of_the_elements" rel="nofollow">https://en.wikipedia.org/wiki/List_of_oxidation_states_of_the_elements</a></p>
<p>I... | https://chemistry.stackexchange.com/questions/61353/why-do-osmium-and-iridium-have-the-most-oxidation-states-of-all-the-elements |
Question: <blockquote>
<p>Why is it that there are fixed oxidation states for most elements out there, with no to very rare exceptions? </p>
</blockquote>
<p>I was taught that oxidation state is a totally artificial concept we have invented for book-keeping purposes. How is it that its applicable so widely? I unders... | https://chemistry.stackexchange.com/questions/70463/why-are-oxidation-states-such-a-fundamental-quantity-for-elements |
Question: <p>Paulings electronegativity is a relative scale, based on the difference in electronegativity between X and Y, <span class="math-container">$\Delta EN = 0.102 \sqrt {\Delta}$</span>, where <span class="math-container">$\Delta = (X-Y)_{measured}-(X-Y)_{theoretical}$</span> bond energies.</p>
<p>But what is t... | https://chemistry.stackexchange.com/questions/151759/which-oxidation-states-were-used-when-pauling-developed-his-electronegativity-sc |
Question: <p>Take propanoic acid for example. If I assign oxidation states to the 3 carbons in it using the idea that the more electronegative element gets all the electrons in the bonds it makes, the 3 carbons get -3( the one in the CH3), -2( the one in the middle), and +3( the one in the acid group). </p>
<p>Is this... | https://chemistry.stackexchange.com/questions/111748/can-an-element-have-variable-oxidation-states-in-a-compound |
Question: <p>Here a screenshot from our lecture on bioinorganic molybdenum complexes, dealing with the catalytic cycle of xanthine oxidase:</p>
<p><a href="https://i.sstatic.net/oSChf.png" rel="nofollow noreferrer"><img src="https://i.sstatic.net/oSChf.png" alt="enter image description here" /></a></p>
<p>It is said th... | https://chemistry.stackexchange.com/questions/180636/how-are-oxidation-states-of-bioinorganic-molybdenum-tungsten-complexes-determine |
Question: <p>I have just been looking at <a href="https://en.wikipedia.org/wiki/List_of_oxidation_states_of_the_elements" rel="nofollow noreferrer">https://en.wikipedia.org/wiki/List_of_oxidation_states_of_the_elements</a> and found that boron has a -5 oxidation state. I would like to know which boron compounds fo... | https://chemistry.stackexchange.com/questions/108521/oxidation-states-of-boron |
Question: <blockquote>
<p>For preservation of meat, sodium nitrite is usually added and as a result <span class="math-container">$\ce{NO}$</span> is then formed. Consequently, <span class="math-container">$\ce{NO}$</span> reacts with the sulfur and iron atoms from decomposition of proteins, forming <span class="math-... | https://chemistry.stackexchange.com/questions/53588/oxidation-states-of-iron-in-roussins-salts |
Question: <p>Halogens like $\ce{Cl,Br,I}$ generally show oxidation states between $-1$ and $+7$. However, is it possible that they can show an oxidation state beyond $-1$ (e.g. $-3$)?</p>
<p>I was thinking of some compound in which chlorine is bonded with a less electronegative element and forms more than one bond wit... | https://chemistry.stackexchange.com/questions/59146/is-it-possible-for-halogens-to-show-oxidation-states-less-than-1 |
Question: <p>It is observed that actinides do not exhibit +2 oxidation state, contrary to that of some of the lanthanide elements. Why?</p>
Answer: <p>See also: <a href="https://chemistry.stackexchange.com/q/48971/16683">Why is WF6 stable whereas CrF6 is unknown?</a></p>
<p>Whenever one wants to compare oxidation sta... | https://chemistry.stackexchange.com/questions/82722/oxidation-states-of-actinides |
Question: <p>I read that the fluorides of 3d metals in lower oxidation states, e.g. <span class="math-container">$\ce{VF2}$</span>, <span class="math-container">$\ce{TiF2}$</span>, and <span class="math-container">$\ce{CuF}$</span> are thermodynamically unstable. For example, <span class="math-container">$\ce{CuF}$</sp... | https://chemistry.stackexchange.com/questions/102326/stability-of-3d-metal-fluorides-and-iodides-in-different-oxidation-states |
Question: <p>A long time ago I was researching the effect of the self regulatory response in Fe and Co. I found that my results made sense based on the idea of the electronegativity of the ions considered. I found a webpage that listed the relationship between the different electronegativities for different oxidation ... | https://chemistry.stackexchange.com/questions/115469/reference-for-electronegativities-of-different-metal-oxidation-states |
Question: <p>To get the oxidation state of carbon (denoted $x$) in octane, $\ce{C8H18}$, I used the fact that hydrogen has an oxidation state of $+1$:</p>
<p>$$8x + 18\cdot 1 = 0 \qquad \Longrightarrow \qquad x = -\frac{18}{8} = -2.25$$</p>
<p>But in that way, I get an oxidation number that is fractional, or not an i... | https://chemistry.stackexchange.com/questions/5357/are-fractional-oxidation-states-possible |
Question: <p>How to determine the oxidation states of the metal atoms when both cation and anion are coordination complexes?</p>
<p>For example, how to determine the oxidation states of <span class="math-container">$\ce{Pt}$</span> in the following compound?:</p>
<p><span class="math-container">$[\ce{Pt(NH3)4}][\ce{P... | https://chemistry.stackexchange.com/questions/59089/how-to-determine-the-oxidation-states-of-the-metal-atoms-when-both-cation-and-an |
Question: <p><a href="https://i.sstatic.net/je5ua.png" rel="nofollow noreferrer"><img src="https://i.sstatic.net/je5ua.png" alt="enter image description here"></a></p>
<p>I was doing some research on Wikipedia and I came across the article on <a href="https://en.wikipedia.org/wiki/Non-innocent_ligand" rel="nofollow no... | https://chemistry.stackexchange.com/questions/91903/what-are-the-magnetic-properties-of-nis2c2ph22zs-3-oxidation-states |
Question: <p>I looked at the flames of copper (I) chloride and of copper (II) chloride through a spectroscope and they looked the same. The flame colour is the same too. But since they have different oxidation states, and therefore different electron configurations, should their emission spectra be slightly different?<... | https://chemistry.stackexchange.com/questions/119671/do-different-oxidation-states-of-the-same-element-have-the-same-emission-spectru |
Question: <p>I am a student in theoretical chemistry and I am confused about the paper: Trends in adsorption of electrocatalytic water splitting intermediates on cubic $\ce{ABO3}$ oxides (Montoya, J. H.; Doyle, A. D.; Nørskov, J. K.; Vojvodic, A.; <em>Phys. Chem. Chem. Phys.</em> <strong>2018,</strong> <em>20</em> (5),... | https://chemistry.stackexchange.com/questions/99065/are-such-high-oxidation-states-as-reported-by-vojovodic-et-al-possible |
Question: <p>I believe similar questions have been asked but this is different and the answers I have looked at don't answer this question. I have read that oxidation states of heavier transition elements (Ru, Os etc) are more <strong>stable</strong> than first row transition metals.</p>
<p>I understand how they can ge... | https://chemistry.stackexchange.com/questions/139680/why-heavier-transition-metals-can-stabilise-higher-oxidations-states |
Question: <p>I noticed that the metals I learned were "type 1" back in early chemistry class as they have one oxidation state including silver, aluminum, zinc, and cadmium. However, those metals weren't reported as "type 1" when I looked online. I noticed that although silver has three oxidative sta... | https://chemistry.stackexchange.com/questions/167988/why-is-silver-considered-a-type-1-metal-although-it-has-multiple-oxidation-sta |
Question: <p>Referring to the series of oxoacids of chlorine: <span class="math-container">$\ce{HClO, HClO2, HClO3},$</span> and <span class="math-container">$\ce{HClO4}$</span>, tabulated in <a href="https://en.wikipedia.org/wiki/Electronegativity#Variation_of_electronegativity_with_oxidation_number" rel="nofollow nor... | https://chemistry.stackexchange.com/questions/136697/is-there-an-error-in-a-wikipedia-article-explaining-the-influence-of-oxidation-s |
Question: <p>I have read that <span class="math-container">$\ce{NOCl}$</span> dissociates to <span class="math-container">$\ce{NO+}$</span> and <span class="math-container">$\ce{Cl-},$</span> and the various reasons stated as such seem fine.</p>
<p>But what I don't get is this: if we follow the actual rules of assigni... | https://chemistry.stackexchange.com/questions/127893/oxidation-states-the-elements-in-nitrosyl-chloride |
Question: <p>A well known experiment is where a basic sodium hydroxide and sucrose solution is added to a KMnO4 solution. The colors change from purple permanganate to green manganate to yellow/orange manganese dioxide (sometimes blue hypomanganate is formed as an intermediate). This common demo is called the 'Chemical... | https://chemistry.stackexchange.com/questions/181885/manganese-oxidation-states-reverse-chameleon |
Question: <p>I have read answer to this question on various sites, but was not satisfied by the answers, because I am not able to understand, that if we remove initially 1 electron from scandium, then 4s would be ome unstable, but if we remove 1 more electron, there remains only one electron in 3d subshell. But we have... | https://chemistry.stackexchange.com/questions/167718/why-scandium-sc-doesnt-show-variable-oxidation-states-especially-2-while |
Question: <p>From Sc, to Mn, the number of oxidation states increases from one (Sc) to seven (Mn). The explanation for this is because the unpaired 3d electrons can be lost along with the 4s electrons during bonding.</p>
<p>Should this be the case? Wouldn't it be easier to lose an electron when it is paired because of... | https://chemistry.stackexchange.com/questions/14539/explanation-for-increase-in-the-number-of-oxidation-states-for-transition-elemen |
Question: <blockquote>
<p>Consider the cell reaction</p>
<p><span class="math-container">$$\ce{2Ag+ + Pb <=> 2Ag + Pb^2+}$$</span>
If <span class="math-container">$\ce{H2S}$</span> gas is passed through the solution, what will be the effect on the EMF of the cell?</p>
</blockquote>
<p><strong>My attempt:</strong>... | https://chemistry.stackexchange.com/questions/49640/effect-of-passing-hydrogen-sulfide-gas-on-electrode-potential |
Question: <blockquote>
<p>For the galvanic cell: $\ce{Ag|AgCl(s)|KCl(0.2M)||KBr(0.001M)|AgBr(s)|Ag}$, calculate the electromotive force (EMF) generated.<br>
$K_\mathrm{sp}(\ce{AgCl}) = 2.8\times10^{-10}$;
$K_\mathrm{sp}(\ce{AgBr}) = 3.3\times10^{-13}$</p>
</blockquote>
<p>I have tried this forming the cell reac... | https://chemistry.stackexchange.com/questions/59383/how-to-calculate-the-electromotive-force-of-a-silver-chloride-silver-bromide-ce |
Question: <p>Reactions for the lead acid battery are: </p>
<p><span class="math-container">$$
\begin{array}{}
\text{Oxidation}&\ce {Pb(s) + HSO4^-(l) &-> PbSO4(s) + H+(l) + 2e-}\\
\text{Reduction}&\ce{PbO2 + HSO4^-(l) + 3H+(l) + 2e- &-> PbSO4(s) + 2H2O}\\
\text{Total reaction}&\ce{Pb(s) + PbO... | https://chemistry.stackexchange.com/questions/89562/cell-notation-for-the-lead-acid-battery |
Question: <p>Is the role of potassium hydroxide (<span class="math-container">$\ce{KOH}$</span>) in an alkaline battery to provide hydroxide for the reaction with zinc? Would the battery cease to work if <span class="math-container">$\ce{KOH}$</span> was removed and only <span class="math-container">$\ce{OH-}$</span> f... | https://chemistry.stackexchange.com/questions/135351/role-of-potassium-hydroxide-in-alkaline-battery |
Question: <p>A charged particle like an ion, does its repulsive or attractive effect on other particles change with temperature? Are electrostatic effects temperature dependent?</p>
Answer: <p>The strength of the electric charge does <em>not</em> change with temperature (unless approaching that of the Big Bang). Howev... | https://chemistry.stackexchange.com/questions/135373/are-electrostatic-effects-temperature-dependent |
Question: <p>For the last assignment of the school year, my science teacher gave the class questions about chem, physics, etc. The third question had me confused and I'll be thankful for all the help given. The question is:</p>
<blockquote>
<p>An ionic solution is created and tested to see how much current can go
throu... | https://chemistry.stackexchange.com/questions/135389/current-with-an-ionic-solution |
Question: <p>Activated carbon is less expensive than mercury . They are recyclable . Mercury is toxic. Nowadays activated carbon is being used in supercapacitors,Li-ion battery.</p>
Answer: <p>Reference electrodes must involve a well defined redox system with reproducible potential.</p>
<p>Mercury is an essential part... | https://chemistry.stackexchange.com/questions/139774/can-i-use-activated-carbon-electrod-as-a-reference-electrod-in-a-ph-meter-instea |
Question: <p>When we make an electrochemical cell, we dip the electrodes in the salt solution. How exactly does the electrode potential change as we dip the electrodes in the salt solutions? Would different salt solutions change the effect of the electrode potential?</p>
Answer: <p>The short answer is that we want a ... | https://chemistry.stackexchange.com/questions/123539/how-does-solution-which-electrodes-are-immersed-in-effect-electrode-potential |
Question: <p>As a part of a school investigation I constructed a voltaic cell experiment where for each run I added a different ligands to the copper (II) sulfate half-cell electrolyte in a daniell cell to see if there was a change in the output voltage Ecell. When plotting a graph of this, it seemed that Ecell increas... | https://chemistry.stackexchange.com/questions/141116/what-is-the-relationship-between-the-stability-constant-of-a-copper-ii-electro |
Question: <p>The general equation for liquid junction potential is given by <span class="math-container">$$E = {-RT\over F}\sum_i\int_a^b{t_i\over z_i}d ln(a_i)$$</span>
Where a and b are the two phases, <span class="math-container">$t_i$</span> is the transport number of the ions and <span class="math-container">$z_i$... | https://chemistry.stackexchange.com/questions/142862/how-to-derive-the-henderson-equation-for-liquid-junction-potentials-given-in-bar |
Question: <p>Ordinary Batteries will deplete most of their Power in a 10 year period. What happens to rechargeable Batteries? How long would they still functin properly?</p>
<p>Hope this is the right community for this question. If you need a specific example:</p>
<p>Powertoll Battery:
<a href="https://www.metabo.com/c... | https://chemistry.stackexchange.com/questions/143664/how-long-do-rechargeable-batteries-last-vs-standard-batteries |
Question: <p>In a <a href="https://en.wikipedia.org/wiki/Concentration_cell" rel="nofollow noreferrer">concentration cell</a>, one can measure a voltage because in one of the half cells (the one with lower concentration electrolyte), the atoms tend to dissipate more into the electrolyte as ions, leaving more electrons ... | https://chemistry.stackexchange.com/questions/145201/why-does-lower-concentration-cause-the-metal-atoms-to-dissipate-more |
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