Equilibrium practice · Mixed difficulty

Which one of the following statement is not true?

The buffering action of an acidic buffer is maximum when its $pH$ is equal to

For which of the following reactions,${K_p} = {K_c}$ ?

Which is a basic salt?

The pH of millimolar $\mathrm{HCl}$ is

If the value of equilibrium constant for a particular reaction is $1.6 \times {10^{12}}$, then at equilibrium the
system will contain

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

For a homogeneous chemical reaction, $K_p=K_C$ when

Aqueous solution of which of the following boron compounds will be strongly basic in nature?

Calculate the $pH$ of a solution in which hydrogen ion concentration is $0.005\mathrm{ }\;g - equi/L?$

For the equilibrium, $2{H_2}O\underset{{}}{\overset{{}}{\leftrightharpoons}}{H_3}{O^ + } + O{H^ - }$, the value of $\Delta {G^ \circ }$ at 298 K is approximately

The concentration of fluroacetic acid (${K_a}$ of acid $= 2.6 \times {10^{ - 3}}$) which is required to get $\left[ {{\mathrm{H}^ + }} \right] = 1.50 \times {10^{ - 3}}M$ is:

In the following reaction $H{C_2}O_4^ - \left( {aq} \right) + PO_4^{ - 3}\left( {aq} \right)HPO_4^{2 - }\left( {aq} \right) + {C_2}O_4^{2 - }\left( {aq} \right)$ which are Bronsted bases

Select the correct expression

Consider the reaction,
${N_2}\left( g \right) + 3{H_2}\left( g \right)\underset{{}}{\overset{{}}{\leftrightharpoons}}2N{H_3}\left( g \right)$
The equilibrium constant of the above reaction is ${K_p}.$ If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that ${p_{N{H_3}}} < < {p_{\mathrm{total}}}$ at equilibrium)

In the titration of $\mathrm{N}{\mathrm{a}_2}\mathrm{C}{\mathrm{O}_3}\;\mathrm{and}\;\mathrm{ HCl}$, the indicator used is

Consider the following reaction, $\mathrm{C}(\mathrm{s}$, diamond $)=\mathrm{C}(\mathrm{s}$, graphite $)+$ heat and choose the correct option.

Which may be added to one litre of water to act as a buffer?

${K_c}$ for ${m_1}A + {m_2}B = {n_1}C + {n_2}D$ is given by:

Consider the following statements.
I) The pH of a mixture containing 400 mL of $\;0.1\;M\;{H_2}S{O_4}$ and 400 mL of $\;0.1\;M\;NaOH$ will be approximately 1.3
II) Ionic product of water is temperature dependent.
III) A monobasic acid with ${K_a} = {10^{ - 5}}$ has a $pH = 5.$ The degree of dissociation of this acid is 50%.
IV) The Le-Chatelier’s principle is not applicable to common-ion effect.
The correct statements are

Ammonium carbonate decomposes as

$\mathrm{N}{\mathrm{H}_2}\mathrm{COON}{\mathrm{H}_4}\left( s \right)\leftrightharpoons2\mathrm{N}{\mathrm{H}_3}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right)$

For the reaction, ${K_p} = 2.9 \times {10^{ - 5}}\;\mathrm{at}{\mathrm{m}^{ - 3}}$ If we start with 1 mole of the compound, the total pressure at equilibrium would be

Which of the following is the strongest conjugate base?

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

Boric acid is a

In which of the following reaction ${K_p} > {K_c}$?

An aqueous solution of ammonium acetate is:

In the reaction, ${\mathrm{H}_2}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)\leftrightharpoons2\mathrm{HCl}\left( \mathrm{g} \right)$

The equivalent conductance of $\frac{M}{{32}}$ solution of a weak monobasic acid is $8.0\;\mathrm{mhos}\;\mathrm{c}{\mathrm{m}^2}$ and at infinite dilution is $400\;\mathrm{mhos}\;\mathrm{c}{\mathrm{m}^2}.$ The dissociation constant of this acid is:

The molar solubility of $Cd\,{\left( {OH} \right)_2}$ is $1.84 \times {10^{ - 5}}\,m$ in water. The expected solubility of $Cd\,{\left( {OH} \right)_2}$ in a buffer solution of $pH = 12$ is

STATEMENT I: When aqueous, solution of $\mathrm{CH}_3 \mathrm{COONH}_4$ is diluted, then its degree of hydrolysis increase.

STATEMENT II : Ammonium acetate is the salt of weak acid and weak base, its degree of hydrolysis depend on the concentration.