Equilibrium practice · Mixed difficulty

STATEMENT I : A solution containing mixture of acetic acid and sodium acetate resist $\mathrm{pH}$ change on addition of small amount of acid or base.

STATEMENT II : A solution containing a mixture of acetic acid sodium acetate acts as buffer solution around pH.4.74

(A): $\mathrm{BaCO}_3$ is more soluble in $\mathrm{HNO}_3$ than in plain water.

(R): Carbonate is a weak base and reacts with $\mathrm{H}^{+}$from the strong acid, causing the barium salt to dissociate.

$A + B\,\leftrightharpoons\,\,C + D$

Initially moles of $A\;\;\mathrm{and}\;\;B$ are equal. At equilibrium, moles of $C$ are three times that of A. the equilibrium constant of the reaction will be

Which of the following statements about ${pH}$ and ${H}^{+}$ion concentration is incorrect?

Equilibrium constant ${K}$ is related to ${E}_{\text {cell }}^0$ and not ${E}_{\text {cell }}$ because

An aqueous solution of hydrogen sulphide shows the equilibrium,

${\mathrm{H}_2}\mathrm{S}\leftrightharpoons{\mathrm{H}^ + } + \mathrm{H}{\mathrm{S}^ - }$

If dilute hydrochloric acid is added to an aqueous solution of hydrogen sulphide without any change in temperature, then:

A solute undergoes complex formation with ions of sparingly soluble salt, the solubility of salt:

The correct order of increasing $\left[ {{\mathrm{H}_3}{\mathrm{O}^ + }} \right]$ in the following aqueous solutions is:

Which of the following has highest pH?

Tetramine copper (II) sulphate is an example of:

For the reactions, $A + B + Q\;\leftrightharpoons\;C + D$  if the temperature is increased then concentration of the products will

The standard Gibbs energy change at 300 K for the reaction, $2A\underset{{}}{\overset{{}}{\leftrightharpoons}}B + C$ is $2494.2 J.$ At a given time, the composition of the reaction mixture is $[A] = \frac{1}{2},\,\,\,[B] = 2\,\,\,\,\,\mathrm{and}\,\,\,\,[C] = \frac{1}{2}$ The reaction proceeds in the [R = 8.314 JK/mole, e = 2.718]

The equilibrium constant for the reaction,${\mathrm{N}_2}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right)\leftrightharpoons2\mathrm{NO}\left( \mathrm{g} \right)$ is $4 \times {10^{ - 4}}$ at 2000 K. In presence of a catalyst the equilibrium is attained ten times faster. Therefore, the equilibrium constant, in present of the catalyst, at 2000 K is:

For the reaction CO(g)$+ \frac{1}{2}{O_2}\left( g \right)C{O_2}(g),\,{K_P}/{K_C}$ will be

The equilibrium constant for ${N_2}(g) + {O_2}(g)\leftrightharpoons2NO\left( g \right)$ is ${K_1}$ and that for $NO(g)\leftrightharpoons\frac{1}{2}{N_2}(g) + \frac{1}{2}{O_2}(g)$ is ${K_2}$, then ${K_1}$ and ${K_2}$ related as

In a lime kiln, to get higher yield of $\mathrm{C}{\mathrm{O}_2}$, the measure that can be taken is

Phenolphthalein can’t be used in the titration of

A white salt is readily soluble in water and gives a colourless solution with a pH of about 9. The salt would be:

In a reaction $PC{l_5}PC{l_3} + C{l_2}$, degree of dissociation is 30%, If initial moles of $PC{l_5}$ is one then total moles at equilibrium is

0.1 mole of ${\mathrm{N}_2}{\mathrm{O}_4}\left( \mathrm{g} \right)$ was sealed in a tube under one atmospheric conditions at $25^\circ C$. Calculate the number of moles of $\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)$ present, if the equilibrium ${\mathrm{N}_2}{\mathrm{O}_4}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)\left( {{K_p} = 0.14} \right)$ is reached after some times

Which of the following relation represents correct relation between standard electrode potential and equilibrium constant?

I. $\log {K}=\frac{{nFE}^{\circ}}{2.303 {RT}}$

II. ${K}={e}^{\frac{{nFE}^{\circ}}{{RT}}}$

III. $\log {K}=\frac{-{nFE}^{\circ}}{2.303 {RT}}$

IV. $\log {K}=0.4342 \frac{-{nFE}^{\circ}}{{RT}}$

Choose the correct statement(s).

A saturated solution of $\mathrm{A}{\mathrm{g}_2}\mathrm{S}{\mathrm{O}_4}\;\mathrm{is}\;2.5 \times {10^{ - 2}}\;\mathrm{M}$ The value of its solubility product is

For the equilibrium ${A}(\mathrm{g}) \rightleftharpoons {nB}(\mathrm{g}),$ the equilibrium constant $K_{{P}}$ is related with the degree of dissociation $\alpha,$ and the total pressure of gases at equilibrium $P$ is

The auto protonation constant of ${\mathrm{H}_2}\mathrm{O}$ is:

Which is decreasing order of strength of bases?
$\mathop \mathrm{O}\limits^\_ \mathrm{H},\mathop \mathrm{N}\limits^\_ {\mathrm{H}_2},\mathrm{HC} \equiv {\mathrm{C}^ - }\mathrm{and C}{\mathrm{H}_3}\mathrm{CH}_2^ -$

$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}) ; \mathrm{K}_1$

$\mathrm{~N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g}) ; \mathrm{K}_2$

$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(\mathrm{g}) ; \mathrm{K}_3$

The equilibrium constant for $2 \mathrm{NH}_3(\mathrm{~g})+\frac{5}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+3 \mathrm{H}_3 \mathrm{O}(\mathrm{g})$ will be

Which of the following is Lewis acid?

For the reaction
$2S{O_2}(g) + {O_2}(g) \to 2S{O_3}(g),\Delta H = - 57.2\mathrm{kJ}\,\mathrm{mo}{\mathrm{l}^{ - 1}}\mathrm{ and }{K_c} = 1.7 \times {10^{16}}$
Which of the following statement is incorrect?

The equilibrium which remains unaffected by change in pressure of the reactants is

A precipitate is formed when