Equilibrium practice · Mixed difficulty

Solubility of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$ in $100 \mathrm{~ml}$ of pure water is $\mathrm{w~gm}$. Find out $\mathrm{k_{s p}}$ of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2\,(\mathrm{M}=$ molecular mass of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2)$

What will be the final $\mathrm{pH}$ if $0.2 \mathrm{~mol}$ of $\mathrm{NaOH}$ is added to $1 \mathrm{~L}$ of buffer solution consisting of $0.4 \mathrm{~M} \mathrm{~CH}_3 \mathrm{COOH}$ and $0.3 \mathrm{~M} \mathrm{~CH}_3 \mathrm{COONa}?$ $\left(\mathrm{pK}_{\mathrm{a}} \text{ of } \mathrm{CH}_3 \mathrm{COOH}=4.75\right)$

The pH indicators are

The $\mathrm{pH}$ value of $10^{-7} \mathrm{~M}$ solution ${HCl}$ is

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

In an evacuated rigid vessel of volume $V$ litre, one mole of solid ammonium carbonate $\left(\mathrm{NH}_2 \mathrm{CONH}_4\right)$ is taken and the vessel is heated to $T \mathrm{~K}.$ The equilibrium total pressure of gases is found to be $P$ atm. The percentage dissociation of solid into $\mathrm{NH}_3(\mathrm{g})$ and $\mathrm{CO}_2(\mathrm{g})$ is

A $0.01 \mathrm{M}$ ammonia solution is $5 \%$ ionized, its $\mathrm{pH}$ will be

Assertion :- The value of $K$ increases when concentration of the reactants are increased.

Reason :- With increases of concentration of reactants the equilibrium shifts in forward direction.

The equilibrium ${SOCl}_2(\mathrm{g}) \rightleftharpoons {SO}_2(\mathrm{g})+{Cl}_2(\mathrm{g})$ is attained at $25^{\circ} \mathrm{C}$ in a closed rigid container and helium gas is introduced. Which of the following statements is correct?

The degree of dissociation of acetic acid in a $0.1 \mathrm{~M}$ solution is $1.32 \times 10^{-2}.$ Calculate dissociation constant of acid and its $\text{pK}_\text{a}$ value:

The partial pressure of ethane over a solution containing $6.56 \times 10^{-3} \mathrm{~g}$ of ethane is $1\,\mathrm{bar}$. If the solution contains $5.00 \times 10^{-2} \mathrm{~g}$ of ethane, then what will be the partial pressure of gas?

Assertion (A) : $\mathrm{HCl}$ and $\mathrm{NaCl}$ cannot form buffer solution.

Reason (R) : Buffer solution is formed by a weak acid and its conjugate salt.

An equilibrium mixture of the reaction, $2\mathrm{NO}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)$ contains 0.120 mole of $\mathrm{N}{\mathrm{O}_2}$, 0.080 mole of $\mathrm{NO}$ and 0.640 mole of ${\mathrm{O}_2}$ in a 4 litre flask at constant temperature. The value of ${K_c}$ for the reaction at this temperature is:

For reaction $\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}$
Some amount of A, B, C and D are added for reaction, then reaction quotient ' $\mathrm{Q}$ '

The dissociation constant of $\mathrm{N}{\mathrm{H}_4}\mathrm{OH}$ is $1.8 \times {10^{ - 5}}.$ The hydrolysis constant of $\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}$ would be:

The unit of ${K_c}$ from the reaction ${N_2} + 3{H_2} \rightleftharpoons 2N{H_3} + Q$ is

STATEMENT I : $\mathrm{pH}$ of $10^{-8} \mathrm{M}$ $\mathrm{HCl}$ lies between 6 and 7.

STATEMENT II : For very dilute solutions of acids, $\mathrm{H}^{+}$ion contribution form water is also taken into consideration.

The solubility product constant $\mathrm{K}_{\text {sp }}$ of $\mathrm{Mg}(\mathrm{OH})_2$ is $9.0 \times 10^{-12}$. If a solution is $0.010 \mathrm{M}$ with respect to $\mathrm{Mg}^{2+}$ ion, what is the maximum hydroxide ion concentration which could be present without causing the precipitation of $\mathrm{Mg}(\mathrm{OH})_2$.

Calculate ${pH}$ of $0.1 \, \mathrm{M}$ solution of ${NH}_4 {Cl}?$ $\left({K}_{{b}}\right.$ for ${NH}_3$ is $2.5 \times 10^{-6}$)

Given ${N_2}\left( g \right) + 3{H_2}\left( g \right) \rightleftharpoons 2N{H_3}\left( g \right);\,\,{K_1}$
${N_2}\left( g \right) + {O_2}\left( g \right) \rightleftharpoons 2NO\left( g \right);\,\,{K_2}$
${H_2}\left( g \right) + \frac{1}{2}{O_2}\left( g \right) \rightleftharpoons {H_2}O\left( g \right);\,\,{K_3}$
The equilibrium constant for $2N{H_3}\left( g \right) + \frac{5}{2}{O_2}\left( g \right) \rightleftharpoons 2NO\left( g \right) + 3{H_2}O\left( g \right)$ will be

Statement-I: $\mathrm{HNO}_3$ is not a Bronsted acid in $\mathrm{CHCl}_3$.

Statement-II: $\mathrm{CHCl}_3$ is not an example for protophilic solvent.

${O}_2$ is kept in a vessel at $300 \mathrm{~K}$. Following equilibrium is established $3 {O}_2(\mathrm{g}) \rightleftharpoons 2 {O}_3(\mathrm{g})$. At equilibrium partial pressure of ${O}_2=10^5$ bar & partial pressure of ${O}_3=10^{-10}$ bar. Calculate $\Delta {G}^{\circ}$ (in kcal) of the above reaction. [Given: ${R}=2 \mathrm{~cal ~K}^{-1} \mathrm{~mol}^{-1} ; \log _{{e}} 10=2.3$]

$0.1\;\mathrm{millimole}$ of $\mathrm{CdS}{\mathrm{O}_4}$ are present in $10\;\mathrm{mL}$ acid solution of $0.08\;N\;\mathrm{HCl}\mathrm{.}$ Now ${\mathrm{H}_2}\mathrm{S}$ is passed to precipitate all the $\mathrm{C}{\mathrm{d}^{2 + }}$ ions. The $\mathrm{pH}$ of the solution after filtering off precipitate, boiling of ${\mathrm{H}_2}\mathrm{S}$ and making the solution $100\;\mathrm{mL}$ by adding ${\mathrm{H}_2}O$ is:

The $\left[ {{\mathrm{H}^ + }} \right]$ ion concentration in $0.001\;M$ acetic acid is $1.34 \times {10^{ - 4}}\;\mathrm{g}\;\mathrm{ ion}\;/\mathrm{litre}\mathrm{.}$ The $\left[ {{\mathrm{H}^ + }} \right]$ ion concentration of $0.164\;\mathrm{g}\;\mathrm{ of}\;\mathrm{ C}{\mathrm{H}_3}\mathrm{COONa}$ is added to a litre of $0.001\;M$ $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ will be:

If $\mathrm{\alpha }$ is the degree of ionisation, $C$ the concentration of a weak electrolyte and ${{K_a}}$ the acid ionisation constant then the correct relationship between $\mathrm{\alpha },C\;and\;{K_a}$ is

For the reaction, $F{e_2}N(s) + \frac{3}{2}{H_2}(g)\underset{{}}{\overset{{}}{\leftrightharpoons}}2Fe(s) + N{H_3}(g)$

At the state of dynamic equilibrium, for solute $+$ solvent $\leftrightharpoons$ solution.

The highest pH value is of:

The equilibrium constant for the reversible reaction ${N}_{{2}}+3 {H}_{{2}} \rightleftharpoons 2 {NH}_3$ is $K$ and for reaction $\frac{1}{2} {N}_2+\frac{3}{2} {H}_2 \rightleftharpoons {NH}_3,$ the equilibrium constant is ${K}^{\prime}$

The $K$ and $K^{\prime}$ will be related as:

$S{O_2}\left( s \right) + 2{H_2}\left( g \right) \rightleftharpoons Sn\left( s \right) + 2{H_2}O\left( g \right)$ in equilibrium mixture 40% water vapour is present by volume. Then find ${K_p}$ if total pressure at equilibrium is 5 atm.