Equilibrium practice · Medium

For the equilibrium:

(I) $\mathrm{C}_6 \mathrm{H}_5 \mathrm{COOH}+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{C}_6 \mathrm{H}_5 \mathrm{COO}^{-}+\mathrm{H}_3 \mathrm{O}^{+} ; K_1=6.30 \times 10^{-5}$

(II) $\mathrm{C}_6 \mathrm{H}_5 \mathrm{COOH}+\mathrm{OH}^{-} \rightleftharpoons \mathrm{C}_6 \mathrm{H}_5 \mathrm{COO}^{-}+\mathrm{H}_2 \mathrm{O} ; K_2=6.30 \times 10^9$

(III) $\mathrm{H}_2 \mathrm{O}+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{OH}^{-} ; K_3-?$

$K_3$ using above equilibria is

$20 \mathrm{~ml}, 0.1 \mathrm{M}$ HA $\left[\left(\mathrm{K}_{\mathrm{b}}\right)_{\mathrm{A}^{-}}=10^{-10}\right]$ is titrated against $0.2 \mathrm{M}, \mathrm{NaOH}$. Select the correct statement :[Given : $\log 2=0.3, \log 3=0.48$ ]

A dilute solution of $\mathrm{HCl}$ contains $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=5.4 \times 10^{-7} \mathrm{~mol} \mathrm{~L}^{-1}$ at $298 \mathrm{~K}$. What is the concentration of hydroxyl ions in this solution?

$pH$ of $0.1\;M\;\mathrm{N}{\mathrm{a}_2}\mathrm{HP}{\mathrm{O}_4}$ and $0.2\;M\;\mathrm{Na}{\mathrm{H}_2}\mathrm{P}{\mathrm{O}_4}$ solutions are respectively. $\mathrm{p}{K_a}$ for ${\mathrm{H}_3}\mathrm{P}{\mathrm{O}_4}$ are $2.12,7.21$ and $12.0$ for respective dissociation to ${\mathrm{H}_2}\mathrm{PO}_4^ - ,\mathrm{HPO}_4^{2 - }$ and $\mathrm{PO}_4^{3 - }.$

Morphine $\left(\mathrm{C}_{17} \mathrm{H}_{19} \mathrm{NO}_3\right)$ is administered medically to relieve pain. It is a naturally occurring base or alkaloid. What is the $\mathrm{pH}$ of a $0.0025 \mathrm{~M}$ solution of morphine at $25^{\circ} \mathrm{C}?$ The base-ionization constant $K_{{b}}$ is $1.6 \times 10^{-6}$ at $25^{\circ} \mathrm{C}.$ $(\log 2=0.3)$

The pH of a 0.1 M solution of $\mathrm{N}{\mathrm{H}_4}\mathrm{OH}$ (having ${K_b} = 1.0 \times {10^{ - 5}})$ is equal to

Assertion :- Solubility of ${AgBr}$ decreases in the presence of sodium bromide.

Reason :- Sodium bromide undergoes hydrolysis in water.

The best explanation for the solubility of $\mathrm{MnS}$ in dil.$\mathrm{HCl}$ is that:

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.

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

$\mathrm{pH}$ 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?

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 $448^{\circ} \mathrm{C}$

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,

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.

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

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

$\mathrm{pH}$ at which a basic indicator with $K_b=1.0 \times 10^{-10}$ changes colour when the indicator is $10^{-2} \mathrm{M}$ is

If ${HCl}$ is added into ${H}_2 {S}$ weak acid, then what will happen: