Equilibrium practice · Medium

The solubility product of $\mathrm{Zn}(\mathrm{OH})_2$ is $10^{-14}$ at $25^{\circ} \mathrm{C}.$ What would be the concentration $\mathrm{Zn}^{+2}$ ion in $0.1 \, \mathrm{M}-\mathrm{NH}_4 \mathrm{OH}$ solution which is $50 \%$ ionized?

Statement (S): The $\mathrm{pH}$ of human blood at body temperature is found to be 6.9.

Explanation (E): Blood is alkaline in nature.

The solubility of $AgCN$ in a buffer solution of $pH = 3$ is $x$. The value of $X$ is…..
[Assume: No cyano complex is formed; ${K_{sp}}\left( {AgCN} \right) = 2.2 \times {10^{ - 16}}$ and ${K_a}\left( {HCN} \right) = 6.2 \times {10^{ - 10}}$]

3.2 moles of hydrogen iodide were heated in a sealed bulb at $444^\circ C$ till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be $22\% .$ The number of moles of hydrogen iodide present at equilibrium are

When acidified ${K_2}C{r_2}{O_7}$ solution is added to $S{n^{2 + }}$ salt then $S{n^{2 + }}$ changes to

A quantity of $\mathrm{PC}{\mathrm{l}_5}$ was heated in a 10 litre vessel at $250^\circ C$ to show $\mathrm{PC}{\mathrm{l}_5}\left( \mathrm{g} \right)\leftrightharpoons\mathrm{PC}{\mathrm{l}_3}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)$. At equilibrium the vessel contains 0.1 mole of $\mathrm{PC}{\mathrm{l}_5}$, 0.20 mole of $\mathrm{PC}{\mathrm{l}_3}$ and 0.20 mole of $\mathrm{C}{\mathrm{l}_2}$. The equilibrium constant of the reaction is :

Among the following which pair of solution can form buffer solution?

Two equilibria, ${AB} \rightleftharpoons {A}^{+}+{B}^{-}$and ${AB}+{B}^{-} \rightleftharpoons {AB}_2^{-}$are simultaneously maintained in a solution with equilibrium constants, ${K}_1$ and ${K}_2$ respectively. The ratio of $\left[{A}^{+}\right]$to $\left[{AB}_2^{-}\right]$in the solution is

In the decomposition of phosgene gas
$\mathrm{COCl}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g}) ; \mathrm{I}_2 \mathrm{O}_5$ is added at constant volume, then

Statement I : $A + B \rightleftharpoons C + D$,
${K_C} = 4$ for the above equilibrium at 300 K when $[B] = [C]$ and $\frac{{[D]}}{{[A]}} = 4$
Statement II : At dynamic equilibrium, rate of forward and backward direction are equal.

Statement I: If $Q_c$ (Reactionquotient) $< K_c$ ( equilabrium constant) reaction moves in direction of reactans.

Statement II : Equilitrium constant is defined in the same way as reaction quotient at end stage of the reaction.

Assertion (A) : $\mathrm{pH}$ of $\mathrm{x\,M} \mathrm{~HCl}$ is less than $\mathrm{pH}$ of $\mathrm{x} \mathrm{~M} \mathrm{~CH} \mathrm{H}_3 \mathrm{COOH}$.

Reason (R) : The degree of ionization of $\mathrm{HCl}$ and $\mathrm{CH}_3 \mathrm{COOH}$ are equal.

The molarity of ${H}_2 {SO}_4$ solution having ${pH}=2$ is

The equilibrium constants for the reaction $\mathrm{A}_2 \rightleftharpoons2 \mathrm{A}$ at $500 \mathrm{~K}$ and $1000 \mathrm{~K}$ are $1 \times 10^{-10}$ and $1 \times 10^{-5},$ respectively. The reaction is

Number of ${\mathrm{H}^ + }$ ions present in $10\;mL$ of a solution of $pH\; = \;3$ is:

Solid $\mathrm{BaF}_2$ is added to a solution containing 0.1 mole of $\mathrm{Na}_2 \mathrm{C}_2 \mathrm{O}_4$ solution $(1 \mathrm{~L})$ until equilibrium is reached. If the $K_{\mathrm{sp}}$ of $\mathrm{BaF}_2$ and $\mathrm{BaC}_2 \mathrm{O}_4$ is $10^{-6}$ $\mathrm{mol}^3 \mathrm{~L}^{-3}$ and $10^{-10} \mathrm{~mol}^2 \mathrm{~L}^{-2},$ respectively, then find the equilibrium concentration of $\mathrm{Ba}^{2+}$ in the solution. Assume that addition of $\mathrm{BaF}_2$ does not cause any change in volume.

3.2 moles of hydrogen iodide were heated in a sealed bulb at $444^\circ C$ till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be $22\% .$ The number of moles of hydrogen iodide present at equilibrium are

Which oxide of nitrogen is the most stable?

For a weak electrolyte $\alpha_1$ and $\alpha_2$ are in ratio of $1: 2$, for a given concentration $k_{\mathrm{a}_1}=2 \times 10^{-4}$. What will be value of $\mathrm{k}_{\mathrm{a}_2}$ ?

Buffer capacity of a buffer solution is x, the volume of 1M added to 100 ml of this solution if the change of ${P^H}$ by 1 is

Which may be added to one litre of water to act as a buffer?

The equivalent conductance of $\frac{M}{{32}}$ solution of a weak monobasic acid is $8.0\;\mathrm{mhos}\;\mathrm{c}{\mathrm{m}^2}$ and at infinite dilution is $400\;\mathrm{mhos}\;\mathrm{c}{\mathrm{m}^2}.$ The dissociation constant of this acid is:

For the reaction $C(s) + C{O_2}(g)2\,\,CO(g)$ the partial pressure of $C{O_2}$ and are 2.0 and 4.0 atm resp, at equilibrium. The ${K_p}$ for the reaction is

STATEMENT-1 : The equilibrium constant of the exothermic reaction at high temperature decreases.

STATEMENT-2 : Since $\ln \frac{K_2}{K_1}=\frac{\Delta H^{\circ}}{R}\left[\frac{1}{T_1}-\frac{1}{T_2}\right]$ and for exothermic reaction, $\Delta H^{\circ}=-$ ve and thereby; $\frac{K_2}{K_1} < 1$

The value of the equilibrium constant for the reaction: $2NO + {O_2} \rightleftharpoons 2N{O_2}$ is 0.25, then the value of equilibrium constant for $2N{O_2} \rightleftharpoons 2NO + {O_2}$ is

Statement-I: Ethyl chloride reacts with sodium ethoxide to from diethyl etber. Here ethoxide ion behaves as strong base.
Statement-II: $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$ is weak acid.

Molar solubility of Zirconium phosphate is ‘S’ moles/litre. Solubility product of Zirconium phosphate $\left[ {Z{r_3}{{\left( {P{O_4}} \right)}_4}} \right]$ is

Which will undergo cationic hydrolysis?

Consider the following reaction:

$\begin{aligned} & \mathrm{CuO}(\mathrm{s})+\mathrm{H}_2(\mathrm{g}) \rightleftharpoons \mathrm{Cu}(\mathrm{s})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) ; \mathrm{K}_1=2 \times 10^{15} \\ & \mathrm{H}_2(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{g}) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(\mathrm{g}) ; \mathrm{K}_2=5 \times 10^{22} \end{aligned}$

The equilibrium constant for the reaction : $\mathrm{CuO}(\mathrm{s}) \rightleftharpoons \mathrm{Cu}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{g})$ would be:

A sparingly soluble Iron (III) salt dissociates in solution as follows:

${Fe}_2 {X}_3(\mathrm{s}) \rightleftharpoons 2 {Fe}^{+3}(\mathrm{aq})+3 {X}^{2-}(\mathrm{aq})$

If the solubility product of the iron (III) salt is ${K}_{{sp}}$, then $\left[{Fe}^{+3}\right](\mathrm{aq})$ at equilibrium is: