Equilibrium practice · Mixed difficulty

Assertion (A): At an equilibrium $\mathrm{A}(\mathrm{g})+2 \mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})$ if substantial amount of water is added to the mixture and stated that only $\mathrm{A}(\mathrm{g})$ gets dissolved to a certain extent in water then equilibrium shifts towards forward direction.

Reason (R): On decreasing the volume of reaction mixture and keeping rest of things same the equilibrium shifts to a direction having more number of gaseous molecules.

The solubility products of $\mathrm{Mg}(\mathrm{OH})_2, \mathrm{Cd}(\mathrm{OH})_2, {Al}(\mathrm{OH})_3$ and $\mathrm{Zn}(\mathrm{OH})_2$ are $4 \times 10^{-11}, 8 \times 10^{-6},8.5 \times 10^{-23}$ and $1.8 \times 10^{-14},$ respectively. The cation that will precipitate first as hydroxide, on adding limited quantity of $\mathrm{NH}_4 \mathrm{OH}$ in a solution containing equimolar amount of metal cations, is

The $\mathrm{pH}$ of a buffer solution containing $2.0 \mathrm{~mol}$ per litre $\mathrm{CH}_3 \mathrm{COONa}$ and $1.5 \mathrm{~mol}$ per litre $\mathrm{CH}_3 \mathrm{COOH}$ is: $\left(K_a\right.$ for acetic acid is $1.8 \times 10^{-5}$ )

Assertion : In the titration of ${Na}_2 {CO}_3$ with ${HCl}$ using methyl orange indicator, the volume required at the equivalence point is twice that of the acid required using phenolphthalein indicator.

Reason : Two moles of ${HCl}$ are required for the complete neutralization of one mole of ${Na}_2 {CO}_3$

The ${pK}_{{b}}$ value of ammonium hydroxide is 4.75. An aqueous solution of ammonium hydroxide is titrated with ${HCl}$. The ${pH}$ of the solution at the point where half of ammonium hydroxide has been neutralised will be

For the reaction, $PC{l_3}(g) + C{l_2}(g)PC{l_5}(g)$ at ${250^0}C$, the value of ${K_C}$ is 26, then the value of ${K_P}$ at the same temperature will be

For the gaseous phase reaction, $2NO\leftrightharpoons{N_2} + \mathrm{ }{O_2}$, $\Delta {H^ \circ } = \mathrm{ } - \mathrm{ }43.5\mathrm{ }\;k\;cal\mathrm{ }\;mo{l^{ - 1}},$  which statement is correct for, ${N_2}\left( g \right)\mathrm{ } + \mathrm{ }{O_2}\left( g \right)\mathrm{ }\leftrightharpoons\mathrm{ }2NO\left( g \right)?$

Tetramine copper (II) sulphate is an example of:

For the reaction $A({~g})+3 B({~g}) \rightleftharpoons 2 C({~g})$ at $27^{\circ} {C}, 2$ moles of $A, 4$ moles of $B$ and 6 moles of $C$ are present in 2 litre vessel. If $K_c$ for the reaction is 1.2 , the reaction will proceed in :

Consider the reactions
(i) $\mathrm{CO}(g)+\mathrm{H}_2 \mathrm{O}(g) \stackrel{K_1}{\rightleftharpoons} \mathrm{CO}_2(g)+\mathrm{H}_2(g)$
(ii) $\mathrm{CH}_4(g)+\mathrm{H}_2 \mathrm{O}(g) \stackrel{K_2}{\rightleftharpoons} \mathrm{CO}(g)+3 \mathrm{H}_2(g)$

(iii) $\mathrm{CH}_4(g)+2 \mathrm{H}_2 \mathrm{O}(g) \stackrel{K_3}{\rightleftharpoons} \mathrm{CO}_2(g)+4 \mathrm{H}_2(g)$

Which of the following is correct relation?

Aqueous solution of which salt has the lowest $pH$?

Statement I: For the reaction $\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g}),$ equilibrium moles of $\text{A}$ and $\text{B}$ are, respectively, '$a$' and ' $b$ ' in $1 \mathrm{~L}$ container. If 5 moles of $\mathrm{A}$ and 3 moles of $\mathrm{B}$ are added, then reaction must move in forward direction.

Statement II: Even if the amount of reactant added to a system at equilibrium is more than the amount of product added at the same time, the equilibrium can shift in any direction.

What is the $\mathrm{pH}$ of the resulting solution when equal volumes of $0.1\,m\,NaOH\,and\,0.01\,M\,HCl$ are mixed?

For the hypothetical reaction, $A(g) \rightleftharpoons B(g)+C(g)$ the correct relation between ${Kp}$ and ${Kc}$ at $12.18 \mathrm{~Kelvin}$ is

Of the following which change will shift the reaction towards the product?

${I}_2({~g}) \rightleftharpoons 2 {I}({g}), \Delta H_r^0(298 {~K})=+150 {~kJ}$

Which of the following ions can exist in solution?

In a $5.76 \mathrm{~L}$ vessel, 0.5 moles of $\mathrm{H}_2$ gas and 0.5 moles of $\mathrm{I}_2$ vapours are allowed to react to form $\mathrm{HI}(\mathrm{g})$ at $447^{\circ} \mathrm{C},$ then the total pressure of gases at equilibrium would be $(R=0.08 \mathrm{~L}-\mathrm{atm} / \mathrm{K}-\mathrm{mol})$

If solubility of gas 'x' in water is 0.5 g/L at 1 bar pressure then solubility at 4 bar pressure will be

The concentration of ${CH}_3 {COO}^{-}$ ion in a solution prepared by adding 0.1 mole of ${CH}_3 {COOAg}(\mathrm{s})$ in 1 L of $0.1 \mathrm{~M}-{HCl}$ solution is $\left[\text{Given: }K_{\mathrm{a}}\left({CH}_3 {COOH}\right)=10^{-5} ; K_{\mathrm{sp}}({AgCl})=10^{-10} ; K_{\mathrm{sp}}\left({CH}_3 {COOAg}\right)=10^{-8}\right]$

When ${NaNO}_3$ is heated in a closed vessel, oxygen is liberated and ${NaNO}_2$ is left behind, then which of the following statements is correct at equilibrium?

${NaNO}_3({~s}) \rightleftharpoons {NaNO}_2({~s})+\frac{1}{2} {O}_2({~g}), \Delta {H}=+{ve}$

Statement I 1 mole $A(g)$ and 1 mole $B(g)$ give 0.5 mole of $C(g)$ and 0.5 mole $D(g)$ at equilibrium.

$A(g)+B(g) \rightleftharpoons C(g)+D(g)$

On taking 2 moles each of $A(g)$ and $B(g)$, percentage dissociation $A(g)$ and $B(g)$ is also doubled.

Statement II Equilibrium constant, $K_c=1$

The $\mathrm{pH}$ of $\frac{\mathrm{M}}{100} \mathrm{Ca}(\mathrm{OH})_2$ is

The $\mathrm{pH}$ of $0.1\;M\;\mathrm{HCl}$ is approximately 1. The approximate $\mathrm{pH}$ of $0.05\;M\;{\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ is:

Determine the degree of dissociation of $0.05 \mathrm{~M} \, {NH}_4 {OH}$ at $25^{\circ} \mathrm{C}$ in a solution of $\mathrm{pH}=10$.

In $2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_2(\mathrm{g})+\mathrm{I}_2(\mathrm{g}), 2$ mole $\mathrm{HI}, 4 \mathrm{~mole}\, \mathrm{H}_2$ and 4 mole of $\mathrm{I}_2$ are found at equilibrium. If some hydrogen is now introduced into the container such that at equilibrium concentration of $\mathrm{HI}$ and $\mathrm{I}_2$ become equal. Find the Number of mole of $\mathrm{H}_2$ added.

Nitric oxide reacts with bromine and give nitrosyl bromide as per the reaction given below.

$2 \mathrm{NO}(\mathrm{g})+\mathrm{Br}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{NOBr}(\mathrm{g})$

when 0.087 mol of NO and 0.0437 mol of $\mathrm{Br}_2$ are mixed in a closed container at constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate the equilibrium amount of nitric oxide:

For the reaction: $\mathrm{NH}_4 \mathrm{HS{(s})} \rightleftharpoons \mathrm{NH}_{3}(\mathrm{g})+\mathrm{H}_2 \mathrm{S{(g})}$
The unit of $\mathrm{Kp}$ for the reactions is

At $25^\circ C$, the equilibrium ${K_1},{K_2}$ and ${K_3}$ of three reactions are :

${\mathrm{N}_2} + 3{\mathrm{H}_2}\;\leftrightharpoons\;2\mathrm{N}{\mathrm{H}_3};\;{K_1}$

${\mathrm{N}_2} + {\mathrm{O}_2}\;\leftrightharpoons\;2\mathrm{NO};\;{K_2}$

${\mathrm{H}_2} + \frac{1}{2}{\mathrm{O}_2}\;\leftrightharpoons\;{\mathrm{H}_2}\mathrm{O};\;{K_3}$

The equilibrium constants for the oxidation of $\mathrm{N}{\mathrm{H}_3}$ by oxygen to give $\mathrm{NO}$ is :

$0.365\;g$ of $\mathrm{HCl}$ gas was passed through $100\;\mathrm{c}{\mathrm{m}^3}$ of $0.2\;M\;\mathrm{NaOH}$ solution. The $pH$ of the resulting solution would be

The ${K_C}$ for ${H_2}(g) + {I_2}(g)2HI(g)$ is 64, if the volume of the container is reduced to one-half of its
original volume, the value of equilibrium constant will be