Equilibrium practice · Mixed difficulty

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

$pH$ for the solution of salt undergoing anionic hydrolysis (say $\mathrm{C}{\mathrm{H}_3}\mathrm{COONa}$ ) is given by:

For weak electrolyte, $\mathrm{AB},$ the degree of ionization would be ($V=$ volume of solution having $1 \mathrm{~mole}$ of electrolyte and $K$ is the ionization constant of the electrolyte)

The solubility of $\mathrm{AgCl}$ in $0.2 \mathrm{~M} \mathrm{~NaCl}$ is

$\left[\mathrm{K}_{\mathrm{sp}} \mathrm{AgCl}=1.8 \times 10^{-10}\right]$

An aqueous solution of aniline of concentration $0.24 \mathrm{~M}$ is prepared. What is concentration of sodium hydroxide is needed in this solution so that anilinium ion concentration remains at $1 \times 10^{-8} \mathrm{M}$ ? ( $K_b$ for $\left.\mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_3{ }^{+}=2.4 \times 10^{-5} \mathrm{M}\right)$

Solubility product principle can be applied when

A container of capacity $V \mathrm{~L}$ contains an equilibrium mixture that consists of 2 moles each of ${PCl}_5, {PCl}_3$ and ${Cl}_2$ (all as gases). The pressure is $30.3975 \mathrm{~kPa}$ and temperature is $T \mathrm{~K}.$ A certain amount ('$x$' mole) of ${Cl}_2(\mathrm{g})$ is now introduced keeping the pressure and temperature constant, until the equilibrium volume becomes $2 V \mathrm{~L}.$ The value of '$90 x$' is

Assertion :-For a reaction $A\left( g \right) + B\left( g \right) \rightleftarrows AB_{\left( g \right)}$ if inert gas is added in a container at
constant volume. The equilibrium shifts to left side.
Reason :- Because partial pressure of $A, B$ and $AB$ decreases.

A buffer solution is prepared by mixing $10\;mL$ of $1.0\;M$ acetic and $20\;mL$ of $0.5\;M$ sodium acetate and then diluted to $100\;mL$ with distilled water. If the $\mathrm{p}{\mathrm{K}_a}$ of $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ is $4.76$, what is the pH of the buffer solution prepared?

A white substance having alkaline nature in solution is

The $K_{s p}$ of $\mathrm{PbCrO}_4$ is $1.0 \times 10^{-16}$. Then the molar solubility of $\mathrm{PbCrO}_4$ is:

The value of $K_{\mathrm{P}}$ for the process: $\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O}(\mathrm{s})\rightleftharpoons \mathrm{CuSO}_4 \cdot 3 \mathrm{H}_2 \mathrm{O}(\mathrm{s})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$ is $1.21 \times 10^{-4} \mathrm{~atm}^2$ at certain temperature. If aqueous tension at that temperature is 40 torr, then at what relative humidity of air will $\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O}$ effloresces?

An acid solution of $\mathrm{pH}=5$ is diluted 1000 times, the $\mathrm{pH}$ of final solution becomes :-

Tribasic acid furnishes…type of anions.

The strength of an acid depends on its tendency to

A saturated solution of $\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}$ in water at $25^\circ C$ contains $0.11\;\mathrm{g}\;\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}$ per litre of solution. The solubility product of $\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}$ is:

The concentration of $\mathrm{KI }\;\mathrm{and}\;\mathrm{ KCl}$ in a certain solution containing both is 0.001 M each. If 20 mL of this solution is added to 20 mL of a saturated solution of AgI in water. What will happen?

$({K_{\mathrm{sp}}}\;\mathrm{AgCl} = {10^{ - 10}},\;{K_{\mathrm{sp}}}\;\mathrm{AgI} = {10^{ - 16}})$

The tendency of $B{F_3},\,BC{l_3}{\rm\,\,\,{ and}}\,\,\,\mathrm{ }BB{r_3}$ to behaves as Lewis acid decreases in the sequence

For the given reaction, $2 \mathrm{~A}(\mathrm{~s})+\mathrm{B}(\mathrm{g})=\mathrm{C}(\mathrm{g})+2 \mathrm{D}(\mathrm{s})+\mathrm{E}(\mathrm{s})$ the degree of dissociation of $\mathrm{B}$ was found to be $20 \%$ at $300 \mathrm{~K}$ and $24 \%$ at $500 \mathrm{~K}$. The rate of forward reaction

For the reactions

$\mathrm{I}_2(\mathrm{aq}) \rightleftharpoons \mathrm{I}_2$ (oil) Equilibrium constant is $\mathrm{K}_1$

$\mathrm{I}_2$ (oil) $\rightleftharpoons \mathrm{I}_2$ (ether) Equilibrium constant is $\mathrm{K}_2$

for the reaction

$\mathrm{I}_2(\mathrm{aq}) \rightleftharpoons \mathrm{I}_2$ (ether) Equilibrium constant is $\mathrm{K}_3$

The relation between $\mathrm{K}_1, \mathrm{K}_2, \mathrm{K}_3$ is

The solubility of $\mathrm{AgBr}$ having solubility product $5 \times10^{-13}$ in $0.1 \mathrm{~M} \mathrm{~CaBr}_2$ solution will be

The relationship between ${K_P}\mathrm{ \,\, and\,\, }{K_C}$ is given by

$\mathrm{pH}$ of the buffer solution formed by mixing acetic acid and sodium acetate taken in equimolar concentration will be [Given : $\mathrm{p} K_a$ value for $\mathrm{CH}_3 \mathrm{COOH}=4.76$ ]

What would be the $\mathrm{pH}$ of an ammonia solution if the $\mathrm{pH}$ of acetic acid solution of same strength is 3.2? The dissociation constants of ammonia and acetic acid are same.

The $K_a$ of a weak monobasic acid is $1 \times 10^{-5}$. The percentage of ionization in a decimolar acid solution is:

STATEMENT I: $\mathrm{pH}$ of $10^{-7} \mathrm{M}$ ${HCl}$ is less than 7 at $25^{\circ} \mathrm{C}$
STATEMENT II : At very low concentration of ${HCl}$, contribution of $\mathrm{H}^{+}$from water considerable.

The equilibrium constants for $\mathrm{A}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{A}(\mathrm{g})$ at $400 \mathrm{~K}$ and $600 \mathrm{~K}$ are $1 \times 10^{-8}$ and $1 \times 10^{-2}$ respectively. The reaction is

Equilibrium constants for some reactions are given. In which of the following case does the reaction go farthest to completion?

The hydronium ion concentration in an aqueous solution of $\mathrm{H}_2 \mathrm{SO}_4$ is $2.0 \times 10^{-4} \mathrm{M}$ at $25^{\circ} \mathrm{C}.$ The hydroxide ion concentration in the solution is

In the presence of excess of anhydrous ${SrCl}_2$, the amount of water taken up is governed by $K_p=10^{12} {~atm}^{-4}$ for the following reaction at $273 {~K}$
${SrCl}_2 \cdot 2 {H}_2 {O}({s})+4 {H}_2 {O}({g}) \rightleftharpoons {SrCl}_2 \cdot 6 {H}_2 {O}({s})$

What is equilibrium vapour pressure (in torr) of water in a closed vessel that contains ${SrCl}_2 \cdot 2 {H}_2 {O}(s)$ ?