Equilibrium practice · Mixed difficulty

The solubility product of $\mathrm{SrF}_2$ in water is $8 \times 10^{-10}$. Find its solubility in $0.1 \mathrm{~M} \mathrm{~NaF}$ aqueous solution.

For the reaction $AB\left( g \right) \rightleftharpoons A\left( g \right) + B\left( g \right),\,\,\,\,AB$ is 33% dissociated at a total pressure of $P$. Therefore, $P$ is related to ${K_P}$ by one of the following options.

Statement (S): The solubility of $\mathrm{HgI}_2$ in water decreases in presence of $\mathrm{KI}$.

Explanation (E): $\mathrm{HgI}_2$ is insoluble in water but it becomes soluble in $\mathrm{KI}(a q)$.

(A): $\mathrm{pH}$ of blood is maintained inspite of acidic foods.

(R): Acidity of foods is not so large to change the $\mathrm{pH}$ of blood.

For an equilibrium reaction involving gases, the forward reaction is 1st order while the reverse reaction is 2nd order. The units of ${{K_b}}$ for the forward equilibrium is:

The equilibrium constant for a reaction $A+2 B \rightleftharpoons 2 C$ is 40. The equilibrium constant for reaction $C \rightleftharpoons B+\frac{1}{2} A$ is

If equilibrium constants of reactions $AB\,and\,\,CD\,are\,{K_1}\,and\,\,{K_2}$ respectively, then the equilibrium constant for the reaction $D + BA + C$ will be

$\mathrm{pH}$ of $\mathrm{Ca}(\mathrm{OH})_2$ solution is $\left(\mathrm{K}_{\mathrm{sp}}=4 \times 10^{-15}\right)$

One litre of an aqueous solution contain 0.15 moles of $C{H_3}COOH\left( {pka = 4.8} \right)$ and 1.5 mole of $C{H_3}COONa$ . The pH of solution is:

Assertion :- Addition of ${NH}_4 {OH}$ to an aqueous solution of ${BaCl}_2$ in the presence of ${NH}_4 {Cl}$ (excess) precipitates ${Ba}({OH})_2.$

Reason :- ${Ba}({OH})_2$ is insoluble in water.

Which of the following set of an acid $\&$ base (one equivalent each) on neutralization will release maximum energy?

The hydroxide with highest solubility product is:

The total number of different kind of buffers obtained during the titration of ${\mathrm{H}_3}\mathrm{P}{\mathrm{O}_4}$ with $\mathrm{NaOH}$ are:

The ionization constant of HCN is $4.5\mathrm{ } \times \mathrm{ }{10^{ - 10}}$ at 298 K. Hydrolysis constant of sodium cyanide is

Solid $\mathrm{Ba}{\left( {\mathrm{N}{\mathrm{O}_3}} \right)_2}$ is gradually dissolved in a $1.0 \times {10^{ - 4}}\;M\;\mathrm{N}{\mathrm{a}_2}\mathrm{C}{\mathrm{O}_3}$ solution. At what concentration of $\mathrm{B}{\mathrm{a}^{2 + }}$ will a precipitate begin to form?

$({K_{sp}}\;\mathrm{for}\;\mathrm{BaC}{\mathrm{O}_3} = 5.1 \times {10^{ - 9}})$

$K_{\mathrm{P}}$ for formation of ethane from hydrogen and ethylene is $5.5 \times 10^{18} \mathrm{~atm}^{-1}$ and $K_{\mathrm{P}}$ for formation of ethylene from hydrogen and acetylene is $5 \times10^{26} \mathrm{~atm}^{-1}$ at $323 \mathrm{~K}.$ What is $K_{\mathrm{p}}$ for the reaction between hydrogen and acetylene to form ethane at $323 \mathrm{~K}?$

The $\mathrm{pH}$ of $0.01(\mathrm{M}) \mathrm{KOH}$ is 12 ; if the temperature of the given $\mathrm{KOH}$ solution is increased which of the following would occur?

If the $pH$ of a solution is 2, its normality will be:

At $448^{\circ} \mathrm{C}$, the equilibrium constant $\left(K_C\right)$ for the reaction $\mathrm{H}_2(\mathrm{g})+\mathrm{I}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})$ is $50.5 .$ If we start with $2 \times 10^{-2}$ mol of $\mathrm{HI}, 1 \times 10^{-2} \mathrm{~mol}$ of $\mathrm{H}_2$ and $3 \times 10^{-2} \mathrm{~mol} \, \mathrm{I}_2$ in a $2 \mathrm{~L}$ vessel, then at $448^{\circ} \mathrm{C}$

A cylinder provided with a piston has some $\mathrm{PCl}_5$ which is in equilibrium with $\mathrm{PCl}_3$ and $\mathrm{Cl}_2$. The system is compressed with the help of piston. Indicate the correct statement.

What is the molarity of $\mathrm{F}^{-}$in a saturated solution of $\operatorname{InF}_3$ ? $\left(K_{s p}=7.9 \times 10^{-10}\right)$

Which one of the following species acts as both Bronsted acid and base?

At $273 \mathrm{~K}$ and $1 \mathrm{~atm}, 1 \mathrm{~L}$ of $\mathrm{N}_2 \mathrm{O}_4(g)$ decomposes to $\mathrm{NO}_2(g)$ as given,

$\mathrm{N}_2 \mathrm{O}_4(g) \rightleftharpoons 2 \mathrm{NO}_2(g)$

At equilibrium, original volume is $25 \%$ less than the existing volume. Percentage decomposition of $\mathrm{N}_2 \mathrm{O}_4(g)$ is thus,

Soda water has a pH value:

What is the solubility product of ${Al}({OH})_3$ in water? Given:

${Al}({OH})_4^{-}(\mathrm{aq}) \rightleftharpoons {Al}^{3+}(\mathrm{aq})+4 {OH}^{-}(\mathrm{aq}); K=1.3 \times 10^{-34}$

${Al}({OH})_3(\mathrm{s})+{OH}^{-}(\mathrm{aq}) \rightleftharpoons {Al}({OH})_4^{-}(\mathrm{aq}) ; K=38.5$

Choose the correct statement(s)

A) If the solubility of ${Sb}_2 S_3$ is $1.0 \times 10^{-5} {~mol} / {L}$ at $298 {~K}$, its solubility product will be $108 \times 10^{-25}$

B) ${pH}$ of an aqueous solution having $\left[{H}^{+}\right]=10^{-8} {M}$ is 8 .

C) Ammonia is a leveling solvent for stronger acids like ${HCl}, {HBr}, {HI}$ while glacial acetic acid is differentiating solvent.

According to Le-chatelier's principle, adding heat to a solid $\rightleftharpoons$ liquid equilibrium will cause the

When 0.01 moles of sodium hydroxide are added to a buffer solution, its $\mathrm{pH}$ changes from 4.745 to 4.815 . The buffer capacity of the buffer solution is

Which of the following will not function as a buffer solution?

(i) $\mathrm{NaCl}$ and $\mathrm{NaOH}$

(ii) $\mathrm{NaOH}$ and $\mathrm{N}{\mathrm{H}_4}\mathrm{OH}$

(iii) $\mathrm{C}{\mathrm{H}_3}\mathrm{COON}{\mathrm{H}_4}$ and $\mathrm{HCl}$

(iv) Borax and boric acid

${K_{sp}}$ for sodium chloride is $36\;\mathrm{mo}{\mathrm{l}^2}/\mathrm{litr}{\mathrm{e}^2}$. The solubility of sodium chloride is: