Equilibrium practice · Medium

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.

$\mathrm{XeF}_6+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{XeOF}_4+2 \mathrm{HF};$ 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:

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

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.
$\mathrm{SO}_2+1 / 2 \mathrm{O}_2 \rightarrow \mathrm{SO}_3(\mathrm{g})$

Assertion :- Solubility of sparingly soluble salt increases with increase in temperature.

Reason :- Enthalpy of solution is negative for all salts.

A $0.1 \, \mathrm{M}$ solution of ammonium acetate is diluted by adding $100 \, \mathrm{ml}$ of water. The ${pH}$ of the resulting solution will be $\left({pK}_{{a}}\right.$ of acetic acid is equal to ${pK}_{{b}}$ of ${NH}_4{OH}$)

A volume of $20 \mathrm{~ml}$ of $0.8 \mathrm{~M}-\mathrm{HCN}$ solution is mixed with $80 \mathrm{~ml}$ of $0.4 \mathrm{~M}-\mathrm{NaCN}$ solution. Calculate the $\mathrm{pH}$ of the resulting solution. The value of $K_{{a}}$ of $\mathrm{HCN}=2.5 \times 10^{-10}(\log 2=0.3).$

$150 \mathrm{~mL}$ of $0.0008 \, \mathrm{M}$ ammonium sulphate is mixed with $150 \mathrm{~mL}$ of $0.04 \, \mathrm{M}$ calcium nitrate. The ionic product of ${CaSO}_4$ will be: $\left({K}_{{SP}}=2.4 \times 10^{-5}\right.$ for $\left.{CaSO}_4\right)$

What should be the $pH$ of solution to dissolve the $\mathrm{Cr}{\left( {\mathrm{OH}} \right)_3}\mathrm{\;precipitate}$
[Given, $\left[ {\mathrm{C}{\mathrm{r}^{3 + }}} \right] = 1.0\;\mathrm{mol/L},\;{K_{\mathrm{sp}}} = 6 \times {10^{ - 31}}$

$18\;\mathrm{mL}$ of mixture of acetic acid and sodium acetate required $6\;mL$ of $0.1\;M\;\mathrm{NaOH}$ for neutralization of the acid and $\mathrm{12}\;\mathrm{mL}$ of $\mathrm{p}{K_a}$ of the acid is $4.75,$ what is the $pH$ of the mixture?

$0.04\;\mathrm{g}$ of pure $\mathrm{NaOH}$ is dissolved in $10\;\mathrm{litre}$ of distilled water. The $\mathrm{pH}$ of the solution is:

Assertion (A): pH value of $HCl$ solution is less than that of acetic acid of the some concentration.
Reason (R): Inequimolar solution, the number of titrable protons present in $HCl$ is less than that present in acetic acid.

From a weak acid of $\mathrm{pK}_{\mathrm{a}}=6$, the $\mathrm{pH}$ range of practically possible buffer solution is

The solubility of $\mathrm{AgCl}$ in $0.1 \mathrm{~M} \mathrm{~CaCl} 2$ is $\left(\mathrm{K}_{\mathrm{sp}}\right.$ of $\mathrm{AgCl}=1 \times 10^{-10}$ )

The correct statement about buffer solution is:

According to Bronsted-Lowry concept, the correct order of relative strength of bases follows the order:

5 moles of $X$ are mixed with 3 moles of $Y$. At equilibrium for the reaction, $X + Y\;\leftrightharpoons\;Z,$ 2 moles of $Z$ are formed. The equilibrium constant for the reaction will be

If $K_c$ is in the range of _____ appreciable concentrations of both reactants and products are present.

(A): If solubility of $\mathrm{Ag}_2 \mathrm{CrO}_4$ is $\mathrm{S}$ mole/litre, its solubility product will be $S^2$

(R): Solubility product of $\mathrm{Ag}_2 \mathrm{CrO}_4$ is given by expression $K_{s p}=\left[\mathrm{Ag}^{+}\right]\left[\mathrm{CrO}_4^{2-}\right]$

What is the ${H}^{+}$ion concentration of a solution prepared by dissolving $4 {~g}$ of ${NaOH}$ (Atomic weight of ${Na}=23 \,{amu}$ ) in $1000\, {ml}$ ?

A buffer solution is prepared by mixing 0.1 M ammonia and 1.0 M ammonium chloride. At 298 K, the $\mathrm{p}{K_b}\;\mathrm{of}\;\mathrm{ N}{\mathrm{H}_4}\mathrm{OH }\;\mathrm{is}\;5.0.$ The pH of the buffer is

The equilibrium $\mathrm{PC}{\mathrm{l}_5}\left( \mathrm{g} \right)\;\;\leftrightharpoons\mathrm{PC}{\mathrm{l}_3}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)$ shows that ${K_p}$ is $24.63$ times the value of ${K_c}$ at a particular temperature $T$. Then $T$ (in $K$) is:

The number of ${H^ + }$ ions present in 1 ml of a solution having ${P^H} = 13$ is

At $30^{\circ} \mathrm{C}$, the solubility of ${Ag}_2{CO}_3\left({~K}_{\mathrm{sp}}=8 \times 10^{-2}\right)$ will be maximum in -

Assertion (A): The degree of dissociation of $\mathrm{CH}_3 \mathrm{COOH}$ is more in a solution which is basic than in water.

Reason (R): $\mathrm{K}_{\mathrm{a}}$ of $\mathrm{CH}_3 \mathrm{COOH}$ increases in basic solution.

When 0.5 mole of $\mathrm{N}_2 \mathrm{O}_4$ is placed in a $4.00 \mathrm{~L}$ reaction vessel and heated at $405 \mathrm{~K}, 79.3 \%$ of the $\mathrm{N}_2 \mathrm{O}_4$ decomposes to $\mathrm{NO}_2$. Calculate value of $\mathrm{K}_{\mathrm{P}}$ at $405 \mathrm{~K}$, for the reaction : $\mathrm{N}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{~g})$.

What are the product formed when Deuterium is added equilibrium reaction of ${H}_2$ and ${I}_2$ ?

(i) ${HD}$

(ii) ${DI}$

(iii) ${D}_2$

(iv) ${HI}$

Which of the following statements are correct ?

(i) The extent of dissociation of an acid depends on the strength and polarity of the ${H}-{A}$ bond (where ${A}$ is an electronegative element.)

(ii) As the strength of ${H}-{A}$ bond increases, the energy required to break the bond decreases.

(iii) As the electronegativity difference between the atoms ${H}$ and ${A}$ increases, acidity increases