Equilibrium practice · Mixed difficulty

Aqueous solution of which salt has the lowest $pH$?

One litre of water contains ${10^{ - 7}}\;\mathrm{mole}\;{\mathrm{H}^ + }$ ions. Degree of ionisation of water is:

STATEMENT-1 : The endothermic reactions are favoured at lower temperature and the exothermic reactions are favoured at higher temperature.

STATEMENT-2 : When a system in equilibrium is disturbed by changing the temperature, it will tend to adjust itself so as to overcome the effect of change

The $\mathrm{pH}$ of $0.5 \mathrm{~L}$ of $1.0 \mathrm{MNaCl}$ after the electrolysis for $965 \mathrm{~s}$ using $5.0 \mathrm{~A}$ current ( $100 \%$ efficiency) is

If the pressure of ${\mathrm{N}_2}/{\mathrm{H}_2}$ mixture in a closed apparatus is 100 atm and $20\%$ of the mixture then reacts, the pressure at the same temperature would be :

The equilibrium constant for the reaction $\mathrm{N}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$ is $K_1$ and the equilibrium constant for the reaction $\mathrm{NO}(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{N}_2(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{g})$ is $K_2$ both at the same temperature. The value of $K_1$ and $K_2$ are related as

In the equilibrium, $AB\;\leftrightharpoons\;A + B,$ if the equilibrium concentration of $A$ is doubled, the equilibrium concentration of $B$ would become

Ionisation constant of $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ is $1.7 \times {10^{ - 5}}$ and $\left[ {{\mathrm{H}^ + }} \right]$ ions is $3.4 \times {10^{ - 4}}$. Then, initial concentration of $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ molecules is

In the reaction, $3A + 2B \to 2C$, the equilibrium constant ${K_c}$ is given by

In what manner will increase of pressure affect the following equation?

$\mathrm{C}\left( s \right) + {\mathrm{H}_2}\mathrm{O}\left( \mathrm{g} \right)\;\leftrightharpoons\;\mathrm{CO}\left( \mathrm{g} \right) + {\mathrm{H}_2}\mathrm{O}\left( \mathrm{g} \right)$

At a given temperature the ${K_c}$ for the reaction, $\mathrm{PC}{\mathrm{l}_5}\left( \mathrm{g} \right)\;\leftrightharpoons\;\mathrm{PC}{\mathrm{l}_3}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)$ is $2.4 \times {10^{ - 3}}$. At the same temperature, the ${K_c}$ for the reaction

$\mathrm{PC}{\mathrm{l}_3}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)\;\leftrightharpoons\;\mathrm{PC}{\mathrm{l}_5}\left( \mathrm{g} \right)$ is :

The concept that an acid is a proton donor and a base is a proton acceptor was introduced by:

A weak base $B \mathrm{OH}$ is titrated with a strong acid $\mathrm{H} A$. When $10 \mathrm{~mL}$ of $\mathrm{H} A$ is added, $\mathrm{pH}$ is found to be 9.00 and when $25 \mathrm{~mL}$ is added, $\mathrm{pH}$ is 8.00 . The volume of the acid required to reach the equivalence point is

Which equilibrium can be described as Lewis acid-base reaction but not Bronsted acid-base reaction?

Hydrogen and oxygen were heated together in a closed vessel. The equilibrium constant is found to decrease after $2000^\circ C$. Which is responsible for this?

Which is a buffer solution

The reaction quotient (Q) for the reaction ${N_2}(g) + 3{H_2}(g)2N{H_3}(g)$ is given by $Q = \frac{{{{\left[ {N{H_3}} \right]}^2}}}{{\left[ {{N_2}} \right]{{\left[ {{H_2}} \right]}^3}}}$ The reaction will proceed towards right side if

Which of the following equilibrium will shift in forward direction on applying pressure?

The equilibrium,

${\mathrm{P}_4}\left( s \right) + 6\mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)\;\leftrightharpoons\;4\mathrm{PC}{\mathrm{l}_3}\left( \mathrm{g} \right)$ attained by mixing equal moles of ${\mathrm{P}_4}$ and $\mathrm{C}{\mathrm{l}_2}$ in a evacuated vessel. Then, at equilibrium,

Degree of dissociation of$0.1\;\mathrm{ }N$ $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ is (dissociation constant $= 1 \times {10^{ - 5}}$)

Which of the following statements are true?

(A) $\left[\mathrm{H}^{+}\right]=\left[\mathrm{OH}^{-}\right]=\sqrt{\mathrm{K}_{\mathrm{w}}}$ for a neutral solution at all temperature.

(B) $\left[\mathrm{H}^{+}\right] > \sqrt{\mathrm{K}_{\mathrm{w}}}$ and $\left[\mathrm{OH}^{-}\right] < \sqrt{\mathrm{K}_{\mathrm{w}}}$ for an acidic solution.

(C) $\left[\mathrm{H}^{+}\right] < \sqrt{\mathrm{K}_{\mathrm{w}}}$ and $\left[\mathrm{OH}^{-}\right] > \sqrt{\mathrm{K}_{\mathrm{w}}}$ for an alkaline solution.

(D) $\left[\mathrm{H}^{+}\right]=\left[\mathrm{OH}^{-}\right]=10^{-7} \mathrm{M}$ for a neutral solution at all temperatures.

A certain sample of rainwater gives a yellow colour with methyl red [pH range 4.2 (red) - 6.2 (yellow)] and a yellow colour with phenol red [pH range 6.4 (yellow) - 8.0 (red)]. What is the approximate $\mathrm{pH}$ of the water? Is the rainwater acidic, neutral or basic?

Assertion :- $HCl$ is titrated with $NaOH$ using phenolphthalein as indicator, pink colour appears
in solution when ${OH}^–$ ion is present in excess in solution.

Reason :- At end point, both reacting species, neutralizes each other.

An aqueous solution of $\mathrm{1M }\;\mathrm{NaCl}\;\mathrm{ and}\;1\;\mathrm{M}\;\mathrm{ HCl }\;\mathrm{is}$

Value of equilibrium constant depends on

The degree of hydrolysis in hydraulic equilibrium

$A^{-}(a q)+\mathrm{H}_2 \mathrm{O}(l) \rightleftharpoons \mathrm{HA}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$

at salt concentration $0.0001 \mathrm{M}$ is ...... $\times 10^{-2}$ $\left(K_a=1.0 \times 10^{-6}\right)$

The $\mathrm{pH}$ of ${10^{ - 8}}\mathrm{M\; HCl}$ solution is

Pure ammonia is placed in a vessel at temperature where its dissociation constant ($\mathrm{\alpha }$) is appreciable. At equilibrium,

For the reaction,

${\mathrm{N}_2}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{NO}\left( \mathrm{g} \right)$, the value of ${K_c}$ at $800^\circ C$ is 0.1. When the equilibrium concentration of both the reactants is 0.5 mole, what is the value of ${K_p}$ at the same temperature?

Arrange the following in increasing order of solubility product:

$\mathrm{Ca}(\mathrm{OH})_2, \mathrm{AgBr}, \mathrm{PbS}, \mathrm{HgS}$