Equilibrium practice · Mixed difficulty

The $\mathrm{pH}$ of mixture having $0.5 \mathrm{~M} \mathrm{~NH}_4 \mathrm{OH}$ and $1.0 \mathrm{~M} \mathrm{~NH}_4 \mathrm{Cl}$ is $\left(\mathrm{K}_{\mathrm{b}} \mathrm{~NH}_4 \mathrm{OH}=1 \times 10^{-5}\right)$

The indicator used in the titration of sodium carbonate with sulphuric acid is

What is the pH of a neutral solution at $37^{\circ} \mathrm{C},$ where $K_{{w}}$ equals $2.5 \times 10^{-14}?$ $(\log 2=0.3)$

According to Le-Chatelier principle, adding heat a solid and liquid in equilibrium will cause the

Which statement is wrong about $\mathrm{pH}$?

Statement (S): The $\left[\mathrm{H}^{+}\right]$in $10^{-8} \mathrm{~N} \mathrm{HCl}$ is $1.05 \times 10^{-7} \mathrm{M}$.

Explanation(E): The $\mathrm{H}^{+}$is obtained from $\mathrm{HCl}$ and $\mathrm{H}_2 \mathrm{O}$; the later furnishes less $\mathrm{H}^{+}$than $10^{-7}$ due to common ion effect.

If the solubility of $A{g_2}Cr{O_4}$ is $S\,\,\,{\text{mol/litre}}{\text{.}}$ Its solubility product is

The $K_{\mathrm{sp}}$ of $\mathrm{Ag}_2 \mathrm{CrO}_4=1.2 \times 10^{-11}.$ What concentration of $\mathrm{Ag}^{+}$ ion in aqueous solution will just fail to give a precipitate of $\mathrm{Ag}_2 \mathrm{CrO}_4$ with a solution in which $\left[\mathrm{CrO}_4^{-2}\right]=3 \times 10^{-4} \mathrm{M}?$

Statement I : For the reaction, $A + B \rightleftharpoons C;\,\,{K_C} = 2$
If we start with 1 mole each of A, B and C in 5 L flask, then at equilibrium, molar concentration of A and B increases and that of B decreases
Statement II : Reaction quotient $Q > {K_C}$ with given quantity of A, B and C, hence reaction is reversed.

The correct increasing order of solubility of the following substances in $\mathrm{g} / 100 \mathrm{~ml}$ is $\mathrm{PbSO}_4\left(K_{\mathrm{sp}}=2 \times 10^{-9}\right), \operatorname{ZnS}\left(K_{\mathrm{sp}}=1 \times 10^{-22}\right), \operatorname{AgBr}\left(K_{\mathrm{sp}}=4 \times 10^{-13}\right),$ $\mathrm{CuCO}_3\left(K_{\mathrm{sp}}=1 \times 10^{-8}\right).$

(Atomic masses: $\mathrm{Pb}=208, \mathrm{Zn}=65, \mathrm{Ag}=108, \mathrm{Br}=80, \mathrm{Cu}=63)$

For the reaction, ${N_2}(g) + 3{H_2}(g)\,\leftrightharpoons\,2N{H_3}(g),\,$ If the value of equilibrium constant is $K,$ then the equilibrium constant for the reaction, $N{H_3}(g)\,\leftrightharpoons\,\frac{1}{2}{N_2}(g) + \frac{3}{2}{H_2}(g)\,$ will be

A saturated solution prepared by dissolved $\mathrm{Ca}{\mathrm{F}_2}\left( s \right)$ in water, has $\left[ {\mathrm{C}{\mathrm{a}^{2 + }}} \right] = 3.3 \times {10^{ - 4}}$ M. What is the ${K_{\mathrm{sp}}}$ of $\mathrm{Ca}{\mathrm{F}_2}$?

The total number of different kind of buffers obtained during the titration of ${\mathrm{H}_3}\mathrm{P}{\mathrm{O}_4}$ with $\mathrm{NaOH}$ are:

The $\mathrm{pH}$ value of $0.1 \mathrm{~M}$ solutions of $\mathrm{CH}_3 \mathrm{COONa} \text{(I)}, \mathrm{CH}_3 \mathrm{COOH} \text{(II)}, \mathrm{CH}_3 \mathrm{COONH}_4 \text{(III)}, \mathrm{NaOH} \text{(IV)}$ and ${HCl}(\mathrm{V})$ is in the order

In the reaction, ${\mathrm{N}_2}{\mathrm{O}_4}\;\leftrightharpoons\;2\mathrm{N}{\mathrm{O}_2}$, $\mathrm{\alpha }$ is that part of ${\mathrm{N}_2}{\mathrm{O}_4}$ which dissociates, then the number of moles at equilibrium will be

The total number of different kind of buffers obtained during the titration of ${\mathrm{H}_3}\mathrm{P}{\mathrm{O}_4}$ with $\mathrm{NaOH}$ are:

STATEMENT I : $\mathrm{pH}$ of a aqueous solution of acetic acid remains unchanged on the addition of sodium acetate.

STATEMENT II : Dissociation of acetic acid is increased by the addition of sodium acetate due to common ion effect.

A gaseous phase reaction taking place in $1 \mathrm{~L}$ flask at $400 \mathrm{~K}$ is given, $\mathrm{N}_2(g)+3 \mathrm{H}_2(g) \rightleftharpoons 2 \mathrm{NH}_3(g)$.
Starting with 1 mole $\mathrm{N}_2$ and 3 moles $\mathrm{H}_2$, equilibrium mixture required $250 \mathrm{~mL}$ of $1 \mathrm{~M} \mathrm{~H}_2 \mathrm{SO}_4$. Thus, $K_c$ is

An aqueous solution contains $\mathrm{N}{\mathrm{i}^{2 + }},\mathrm{C}{\mathrm{o}^{2 + }}\;\mathrm{and}\;\mathrm{ P}{\mathrm{b}^{2 + }}$ ions at equal concentrations. The solubility product of $\mathrm{NiS},\mathrm{PbS}\;\mathrm{ and }\;\mathrm{CoS}$ in water at $25^\circ C$ are $1.4 \times {10^{ - 24}},\;3.4 \times {10^{ - 28}}\;\mathrm{and}\;3 \times {10^{ - 26}}$, respectively. Indicate which of these ions will be precipitated first and last when sulphide concentration is progressively increased from zero?

Assertion : Mixture of ${CH}_3 {COOH}$ and ${CH}_3 {COONH}_4$ is an example of acidic buffer.

Reason: Acidic buffer contains equimolar mixture of a weak acid and its salt with weak base.

The solubility of $\mathrm{CaCO}_3$ is $7 \mathrm{~mg/litre}.$ Calculate the solubility product of $\mathrm{BaCO}_3$ from this information and from the fact that when $\mathrm{Na}_2 \mathrm{CO}_3$ is added slowly to a solution containing equimolar concentration of $\mathrm{Ca}^{2+}$ and $\mathrm{Ba}^{2+},$ no precipitate of $\mathrm{CaCO}_3$ is formed until $90 \%$ of $\mathrm{Ba}^{2+}$ has been precipitated as $\mathrm{BaCO}_3.$

$\mathrm{pH}$ of an acidic buffer is 7 and $\mathrm{pKa}$ is 5 then the ratio of $\frac{[\text { salt }]}{[\text { Acid }]}$ is:-

A 0.2 molar solution of formic acid is $3.2 \%$ ionised, its ionisation constant is

Assertion :- For the reaction $A \rightleftharpoons B + C + D$ at equilibrium state $[A]=[B]=[C]=3 \times 10^{-4} \mathrm{M}$ and equilibrium constant is $3 \times 10^{-4}.$
Reason :- Given reaction is exothermic.

Statement I : For the equilibrium $H_{2(g)}+I_{2(g)} \rightleftharpoons 2 H I_{(g)}, K_C$ is doubled if volume of the vessel is reduced to half its initial volume.
Statement II : Decrease in volume proportionately decrease the concentrations of both reactants & products.

The values of $\mathrm{K}_{\mathrm{sp}}$ of $\mathrm{CaCO}_3$ and $\mathrm{CaC}_2 \mathrm{O}_4$ are $4.7 \times 10^{-9}$ and $1.3 \times 10^{-9}$ respectively at $25^{\circ} \mathrm{C}$. If the mixture of these two is washed with water, what is the concentration of $\mathrm{Ca}^{2+}$ ions in water?

The pH of an aqueous solution having hydroxide ion concentration as $1 \times {10^{ - 5}}$ is

Find change in $\mathrm{pH}$ of water when $1 \mathrm{~mL}$ of $10^{-3} \mathrm{M}$ $\mathrm{KOH}$ is added to $99 \mathrm{~mL}$ of $\mathrm{H}_2 \mathrm{O}$ at $25^{\circ} \mathrm{C}$.

Hydrolysis of sucrose gives

sucrose + ${H_2}O\underset{{}}{\overset{{}}{\leftrightharpoons}}$ Glucose + Fructose

Equilibrium constant ${K_C}$ for the reaction is $2 \times {10^{13}}$ at 300 K. calculate $\Delta {G^\mathrm{o}}$ at 300 K

Which statement is false? (Assume complete dissociation in each case)