Equilibrium practice · Mixed difficulty

The Henderson’s equation used to calculate the $\mathrm{pOH}$ of basic buffer is:

Which addition would not change the $\mathrm{pH}$ of $10\,\mathrm{mL}$ of dilute hydrochloric acid?

For the equilibrium $\alpha$-(D) glucose $\rightleftharpoons \beta$-(D) glucose $K_c=18$ The percentage of $\alpha$-(D)-glucose at equilibrium is

In the following equilibrium amount of $\mathrm{CO}(g)$ can be decreased by

$2 \mathrm{CO}(g)+\mathrm{O}_2(g) \rightleftharpoons 2 \mathrm{CO}_2(g)$

Statement-I: $\mathrm{ClO}_4^{-}$is the weakest acid.

Statement-II: In $\mathrm{ClO}_4$; ion chlorine is $\mathrm{sp}^3$ hybridized.

The dissociation constants of acids $\mathrm{HA}, \mathrm{HB}, \mathrm{HC}$ and $\mathrm{HD}$ are $2.6 \times 10^{-3}, 5.3 \times 10^{-9}, 1.1 \times 10^{-2}, 7.5 \times 10^{-5}$ respectively. The weakest acid among these acids is

Molar conductance of $0.01 \mathrm{~M}$ weak monoprotic acid $\text{(HA)}$ is $40 \mathrm{~mho} \mathrm{~cm}^2 \mathrm{~mol}^{-1}.$ $\mathrm{p}^{\mathrm{H}}$ of the solution is (Limiting molar conductance of $\text{HA}$ is $400 \mathrm{~mho} \mathrm{~cm}^2 \mathrm{~mol}^{-1})$

$\mathrm{pH}$ of a mixture of $1 \mathrm{M}$ benzoic acid $\left(\mathrm{p} K_a=4.20\right)$ and $1 \mathrm{M}\, {C}_6 {H}_5 {COONa}$ is 4.5 . In $300 \mathrm{~mL}$ buffer, benzoic acid is $[\log 2=0.3]$

What will be the value of ${P^H}$ of $0.01\,\,\,{\text{mol}}\,\,\,{\text{d}}{{\text{m}}^{ - 3}}\,\,C{H_3}COOH\,\,\,\,\,\left( {{K_a} = 1.74 \times {{10}^{ - 5}}} \right)?$

Statement I : When a 10 L flask contains 4 moles each of $PC{l_5}(g) \rightleftharpoons PC{l_3}(g) + C{l_2}(g)\,\,({K_C} = 5)$ equilibrium proceeds in backward side.
Statement II : Reaction quotient, ${Q_C} > {K_C}$

${10^{ - 6}}\;M\;\mathrm{HCl}$ is diluted to 100 times. Its $pH$ is:

Assertion :- At $25^{\circ} \mathrm{C}$ the pH of $10^{-8} \mathrm{~M} \, {HCl}$ is 8.

Reason :- pH of acidic solution is always below 7 at $25^{\circ} \mathrm{C}.$

In the reaction, $\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})=2 \mathrm{CO}(\mathrm{g})$, the following amounts of substances were formed in 0.2 litre flask at equilibrium, $\mathrm{C}=0.1$ mole, $\mathrm{CO}=0.05$ mole, $\mathrm{CO}_2=0.06$ mole. The equilibrium constant is

The pH of $1\,M\,C{H_3}COONa$ solution in water will be nearly $\left( {p{K_a}\,\,for\,C{H_3}COOH = 4.74} \right)$

What will be the resultant ${pH}$ when $150 \mathrm{~mL}$ of an aqueous solution of ${HCl} \, ({pH}=2.0)$ is mixed with $350 \mathrm{~mL}$ of an aqueous solution of ${NaOH} \, ({pH}=12.0)?$

Acetic acid and propionic acid have ${K_a}$ values $1.75 \times {10^{ - 5}}$ and $1.3 \times {10^{ - 5}}$ respectively at a certain temperature. An equimolar solution of a mixture of the two acids is partially neutralized by$\mathrm{NaOH}\mathrm{.}$. How is the ratio of the contents of acetate and propionate ions related to the ${K_a}$ values and the molarity?

Statement (S): The acidic nature of some cations is :
$\mathrm{Al}^{3+}>\mathrm{Be}^{2+}>\mathrm{Na}^{+}>\mathrm{K}^{+}$

Explanation (E): More is the effective nuclear charge on cation more is its acidic nature.

${K_{SP}}$ of $M{X_4}$ and solubility of $M{X_4}$ (S mol/L), is related by

${\mathrm{H}_3}\mathrm{B}{\mathrm{O}_3}$ is:

If $K_{s p}$ of $\mathrm{ZnS}$ is $1.0 \times 10^{-21}$, the minimum volume of water is required for the dissolution of $0.097 \mathrm{~g} \mathrm{~ZnS}$ is :

The $pOH$ of a solution obtained by mixing $25 \mathrm{~mL}$ of $0.2 \mathrm{~M} \mathrm{~HCl}$ with $50 \mathrm{~mL}$ of $0.25 \mathrm{~M} \mathrm{~NaOH}$ is $\left(Kw=1.0 \times 10^{-14}\right)$

(A): A very dilute acidic solution of $\mathrm{Cd}^{2+}$ and $\mathrm{Ni}^{2+}$ gives yellow precipitate of $\mathrm{CdS}$ on passing hydrogen sulphide.
(R): Solubility product of CdS is more than that of NiS.

pH of ${10^{ - 2}}\mathrm{M}\,\,\,Ca{(OH)_2}$ aqueous solution is nearly

In the decomposition reaction of ammonia: $2 \mathrm{NH}_3(\mathrm{g}) \rightleftharpoons \mathrm{N}_2(\mathrm{g})+3 \mathrm{H}_2(\mathrm{g}). 2$ moles of $\mathrm{NH}_3$ are introduced in the vessel of 1 litre. At equilibrium, 1 mole $\mathrm{NH}_3$ was left, the value of $\mathrm{K_c}$ will be:

Dissociation constants of two acids HA and HB are $4 \times {10^{ - 10}}$ and $1.8 \times {10^{ - 5}}$ resp. Whose ${P^H}$ value will be higher for a given molarity

pH of solution can be expressed as

If pressure increases then its effect on given equilibrium

$2\mathrm{NO}\left( \mathrm{g} \right)\leftrightharpoons{\mathrm{N}_2}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right)$ is shift in

Consider the reaction equilibrium

$\begin{array}{ll} \text { Ice } \rightleftharpoons & \text { Water }-\,{x} \, {kcal} \\ \left(\begin{array}{l} \text { Greater } \\ \text { volume } \end{array}\right) & \left(\begin{array}{l} \text { Lesser } \\ \text { volume } \end{array}\right) \end{array}$

The favorable conditions for forward reaction are

For the reaction taking place at certain temperature $\mathrm{NH}_2 \mathrm{COONH}_4(\mathrm{s}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{g})+\mathrm{CO}_2(\mathrm{g})$ If equilibrium pressure os $3 \mathrm{X}$ bar then $\Delta_\mathrm{t} \mathrm{G}^{\circ}$ would be

$A\left( g \right) + 3B\left( g \right) \rightleftharpoons 4C\left( g \right)$ starting concentration of $A$ is equal to $B$, equilibrium concentration of $A$ and $C$ are same then ${K_C} =$