Equilibrium practice · Mixed difficulty

Equilibrium constant for the following equilibrium,

$3 \mathrm{ClO}^{-}(a q) \rightleftharpoons 2 \mathrm{Cl}^{-}(a q)+\mathrm{ClO}_3^{-}(a q)$

is $10 \times 10^{28}$ at a temperature at which $R T=2500 \mathrm{~J} \mathrm{~mol}^{-1}$.
Gibbs free energy change $\left(\Delta G^{\circ}\right)$ is

Which can act as buffer:

The value of $K_{s p}$ of different salts $A B, A B_2, A_2 B$ and $A_2 B_3$ are $4 \times 10^{-10}, 8 \times 10^{-15}, 2 \times 10^{-14}$, $5 \times 10^{-18}$ respectively. The most soluble salt is

The degree of ionisation of an acid $HA$ is 0.00001 at $0.1 \, \mathrm{M}$ concentration. Its dissociation constant is

The equilibrium constant in a reversible reaction at a given temperature

Which species acts as stronger acid than formic acid in aqueous solution?

The equilibrium constant for ${A_2}\left( g \right)\leftrightharpoons\,2A\left( g \right)$ at 400 K and 600 K are $1 \times {10^{ - 8}}\,\,\mathrm{ and }\,\,1 \times {10^{ - 2}}$ respectively. The reaction is

A weak acid, ${HA}$, has a ${K}_{{a}}$ of $1.00 \times 10^{-5}$. If 0.100 mole of this acid dissolved in one litre of water, the percentage of acid dissociated at equilbrium is closest to

Ammonia under a pressure of $15\mathrm{ }atm$ at $27^\circ C$ is heated to $347^\circ C$ in a closed vessel in the presence of catalyst. Under the conditions, $\mathrm{N}{\mathrm{H}_3}$ is partially decomposed according to the equation, $2\mathrm{N}{\mathrm{H}_3}\leftrightharpoons{\mathrm{N}_2} + 3{\mathrm{H}_2}$. The vessel is such that the volume remains effectively constant whereas pressure increases to $50\mathrm{ }atm$. Calculate the percentage of $\mathrm{N}{\mathrm{H}_3}$ actually decomposed

Assertion :- Boric acid behaves as a weak monobasic acid.

Reason :- Boric acid contains hydrogen bonds in its structure.

Addition of sodium acetate to $0.1\;M$ acetic acid will cause

What mass of 95% pure $CaC{O_3}$ will be required to neutralise 50 mL of 0.5 m HCl solution according to the following reaction?
$CaC{O_3} + 2HC{l_{(aq)}} \to CaC{l_{2(aq)}} + C{O_{2(g)}} + 2{H_2}{O_{(l)}}$
[Calculate upto second place of decimal point]

For the reaction, ${\mathrm{H}_2} + {\mathrm{I}_2}\;\leftrightharpoons\;2\mathrm{HI}$, the equilibrium concentration of ${\mathrm{H}_2},{\mathrm{I}_2}\;\mathrm{and}\;\;\mathrm{ HI}$ are $8.0,\;3.0\mathrm{ }\;and\mathrm{ }\;28.0\mathrm{ }\;mol/L$ respectively. The equilibrium constant is

$1 \mathrm{~mol}$ of helium is added to the dissociation equilibrium $\mathrm{N}_2 \mathrm{O}_4(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{g})-x \mathrm{~kJ}$ set up in a cylinder fitted with a piston in such a way that the piston is moved outwards to keep the total equilibrium pressure constant

In the heterogeneous equilibrium:
${CaCO}_3({s}) \rightleftharpoons {NH}_3({g}) ; {K}_{{p}}=4.0 \times 10^4$
what would be the effect of addition of ${CaCO}_3$ on the equilibrium concentration of ${CO}_2?$

For preparing a buffer solution of $\mathrm{pH}=7.0$, which buffer system you will choose?

1M solution of $C{H_3}COOH$ should be diluted to…….. times so that pH is doubled.

Nature of 0.1 M solution of sodium bisulphite is

Equal volumes of two solutions of a strong acid having ${P^H} = 3\,and\,{P^H} = 4$ are mixed together. The ${P^H}$ of the resulting solution is $\left[ {\log 0.5 = - 0.3} \right]$

Which of the following salts when dissolved in water will hydrolyze?

Some solid ammonium carbonate $\mathrm{NH}_4 \mathrm{COONH}_4$ is take in a evacuated vessel and the vessel is sealed after a very long time a constant pressure of $0.6 \mathrm{~atm}$ is observed due to dissociation of the solid into $\mathrm{NH}_3$ and $\mathrm{CO}_2$ gas. Calculate the dissociation constant of solid.

The silver ion in a solution is precipitated by the addition of
chloride ion.
$\mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q) \rightleftharpoons \mathrm{AgCl}(s), K=1 \times 10^{10}$.
The final volume of the solution is $500 \mathrm{~mL}$. At a point when not more than $0.10 \mathrm{~mg}$ of $\mathrm{Ag}^{+}$ion remains unprecipitated $[\mathrm{Cl^-}]$ ion is

$\mathrm{XeF}_6+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{XeOF}_4+2 \mathrm{HF};$ equilibrium constant $=K_1.$

$\mathrm{XeO}_4+\mathrm{XeF}_6 \rightleftharpoons \mathrm{XeOF}_4+\mathrm{XeO}_3 \mathrm{F}_2;$ equilibrium constant $=K_2.$

The equilibrium constant for the following reaction will be:

$\mathrm{XeO}_4+2 \mathrm{HF} \rightleftharpoons \mathrm{XeO}_3 \mathrm{F}_2+\mathrm{H}_2 \mathrm{O}$

In a $10.0 \mathrm{~L}$ container, an equilibrium was established between $\mathrm{SO}_3, \mathrm{SO}_2$ and $\mathrm{O}_2$ gases, by starting with $\mathrm{SO}_3$ only. The density of equilibrium mixture was found to be $16 \mathrm{~g/litre}$ at a temperature of $\frac{900}{0.0821} \mathrm{~K}.$ If the degree of dissociation of $\mathrm{SO}_3$ is $40 \%,$ then the value of $K_{{P}}$ (in atm) for the reaction $2 \mathrm{SO}_3(\mathrm{g})\rightleftharpoons 2 \mathrm{SO}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{g})$ is

Assertion : The value of $K$ gives us a relative idea about the extent to which a reaction proceeds.

Reason : The value of $K$ is independent of the stochiometry of reactants and products at the point of equilibrium.

Which one of the following statement is not true?

What is the best description of the change that occurs when $\mathrm{N}{\mathrm{a}_2}\mathrm{O}\left( s \right)$ is dissolved in water?

Favorable condition for product formation in the given reaction.
$\mathrm{SO}_2+1 / 2 \mathrm{O}_2 \rightarrow \mathrm{SO}_3(\mathrm{g})$

The ${pH}$ value of ordinary water is :

The strongest Lewis base in the following is