Equilibrium practice · Mixed difficulty

${\mathrm{C}_2}{\mathrm{H}_5}\mathrm{ONa}$ acts as … in ${\mathrm{C}_2}{\mathrm{H}_5}\mathrm{OH}$.

The formation of $\mathrm{S}{\mathrm{O}_3}$ takes place according to the following reaction, $2\mathrm{S}{\mathrm{O}_2} + {\mathrm{O}_2}\leftrightharpoons2\mathrm{S}{\mathrm{O}_3},\;\Delta H = - 45.2\;\mathrm{kcal}$. The formation of $\mathrm{S}{\mathrm{O}_3}$ is favoured by

Conjugate acid and conjugate base of $HPO_4^{2 - }$ respectively are

$Xe{F_6} + {H_2}O\underset{{}}{\overset{{}}{\leftrightharpoons}}XeO{F_4} + 2HF$ equilibrium constant ${K_1}$ $Xe{O_4} + Xe{F_6}\underset{{}}{\overset{{}}{\leftrightharpoons}}XeO{F_4} + Xe{O_3}{F_2}$ equilibrium constant ${K_2}$ then equilibrium constant for the reaction $Xe{O_4} + 2HF\underset{{}}{\overset{{}}{\leftrightharpoons}}Xe{O_3}{F_2} + {H_2}O$ will be

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

The $\mathrm{pH}$ of $\mathrm{0}\mathrm{.1}\;\mathrm{M}$ solution of the following salts increases in the order

Inert gas has been added to the following equilibrium system at constant volume $S{O_2}(g) + \frac{1}{2} {O_2}(g) \to S{O_3}(g)$
To which direction will the equilibrium shift?

For a concentrated solution of a weak electrolyte ${A_x}{B_y}$ of concentration ‘$C$’, the degree of dissociation 'α' is given as

The Henderson Hasselbalch equation explains the relationship between

What is the correct representation for the solubility product of $\mathrm{Sn}{\mathrm{S}_2}$?

${P^H}$ of water is 7.0 at ${25^0}C$. If water is heated to ${70^0}C$, then

Assertion : The equilibrium constant for the reaction

$\begin{aligned} & {CaSO}_4 \cdot 5 {H}_2 {O}({s})={CaSO}_4 \cdot 3 {H}_2 {O}({s})+2 {H}_2 {O}({g}) \\ & \text { is } {K}_{{C}}=\frac{\left[{CaSO}_4 \cdot 3 {H}_2 {O}\right]\left[{H}_2 {O}\right]^2}{\left[{CaSO}_4 \cdot 5 {H}_2 {O}\right]} \end{aligned}$

Reason : Equilibrium constant is the ratio of the product of molar concentration of the substances produced to the product of the molar concentrations of reactants with each concentrations term raised to the power equal to the respective stoichiometric constant.

Which of the following is not a buffer solution?

(A): Benzene is amphiprotic solvent.

(R): Amphiprotic solvents are those which neither donate nor accept protons

For reaction $A(g) + B(g)AB(g)$, We start with 2 moles of A and B each. At equilibrium 0.8 moles of AB is formed. Then how much of A changes to AB.

What happens to $\mathrm{pH}$ of a solution when $\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}$ crystal is added to a dilute solution of $\mathrm{N}{\mathrm{H}_4}\mathrm{OH}$?

Liquid ammonia ionises to a slight extent. At $- 50^\circ C,$  its self ionisation constant, ${K_{\mathrm{N}{\mathrm{H}_3}}} = \left[ {\mathrm{NH}_4^ + } \right]\left[ {\mathrm{NH}_2^ - } \right] = {10^{ - 30}}.$  How many amide ions, are present per $\mathrm{c}{\mathrm{m}^3}$ of pure liquid ammonia? (Assume $N = 6.0 \times {10^{23}}$)

Statement (S): Metal oxides are usually either acidic or amphoteric but $\mathrm{Mn}_2 \mathrm{O}_7$ is acidic.

Explanation (E): On dissolution in water, $\mathrm{Mn}_2 \mathrm{O}_7$ forms per manganic acid.

In which case ${p^H}$ will not change on dilution

The $pH$ of a solution is $5.0$. To this solution sufficient acid is added to decrease the $pH\;to\;2.0$. The increase in hydrogen ion concentration is:

$10\,\mathrm{mL}$ of a solution contains $0.1\,M\,\mathrm{N}{\mathrm{H}_4}\mathrm{Cl} + 0.01\,M\,\mathrm{N}{\mathrm{H}_4}\mathrm{OH}\mathrm{.}$ Which addition would not change the $\mathrm{pH}$ of the solution?

Assertion :- Boric acid behaves as a weak monobasic acid.

Reason :- Boric acid contains hydrogen bonds in its structure.

Assuming complete dissociation which of the following aqueous solutions will have the same pH value?

(i)100 mL of 0.01 M HCl
(ii)100 mL of 0.01 M ${\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$
(iii)50 mL of 0.01 M HCl
(iv)Mixture of 50 mL of 0.02 M ${\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ and 50 mL of 0.02 M $\mathrm{NaOH}$

The dissociation constant for acetic acid and $\mathrm{HCN}$ at $25^\circ C$ are $1.5 \times {10^{ - 3}}$ and $4.5 \times {10^{ - 10}}$ respectively. the equilibrium constant for the equilibrium,

$\mathrm{C}{\mathrm{N}^ - } + \mathrm{C}{\mathrm{H}_3}\mathrm{COOH}\;\leftrightharpoons\;\mathrm{HCN} + \mathrm{C}{\mathrm{H}_3}\mathrm{CO}{\mathrm{O}^ - }$

The percentage of pyridine $({C_5}{H_5}N)$ that forms pyridinium ion $({C_5}{H_5}{N^ + }H)$ in a 0.10 M aqueous pyridine solution $({K_b}\,\mathrm{for}\,{C_5}{H_5}N = 1.7 \times {10^{ - 9}})$ is

Change in pH of a solution from 1 to 2, indicates

Which among the following is an electron deficient compound?

The equilibrium constant, $K$ for the reaction

$2\mathrm{HI}\left( \mathrm{g} \right)\;\leftrightharpoons\;{\mathrm{H}_2}\left( \mathrm{g} \right) + {\mathrm{I}_2}\left( \mathrm{g} \right)$

At room temperature is 2.85 and that at $698\;K$, it is $1.4 \times {10^{ - 2}}$. This implies that

Which of the following molecules acts as a Lewis acid?

A solution of sodium borate has a $\mathrm{pH}$ of approximately: