Equilibrium practice · Easy

Which of the following pairs constitutes a buffer?

When sodium acetate is added to an aqueous solution of acetic acid :

Which of the following salts will give highest ${P^H}$ in water

The reaction $3Fe(s) + 4{H_2}O(l)\underset{{}}{\overset{{}}{\leftrightharpoons}}FeS{O_4}(s) + 4{H_2}(g)$ is reversible if it is carried out

Which of these is a Lewis acid?

Among $\mathrm{BM}{\mathrm{e}_3},\mathrm{B}{\mathrm{F}_3},\mathrm{BC}{\mathrm{l}_3}\;\mathrm{and}\;{\mathrm{B}_2}{\mathrm{H}_6}$ which one will be the best Lewis acid?

What is the minimum $\mathrm{pH}$ necessary to cause a precipitate of ${Pb}({OH})_2\left({~K}_{{sp}}=1.2 \times 10^{-5}\right)$ to form in a $0.12\, \mathrm{M}\,\, {PbCl}_2$ solution ?

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

In $\mathrm{100}\;\mathrm{mL}$ of an aqueous $\mathrm{HCl}$ of $\mathrm{pH}\;1.0,\;900\;\mathrm{mL}$ of distilled water is added, the pH of the resultant solution becomes:

Solution prepared by dissolving equal number of mole of $\mathrm{HOCl}\;\left( {{K_a} = 3.2 \times {{10}^{ - 8}}} \right)$ and $\mathrm{NaOCl}$ is a buffer of pH:

Which one of the molecular hydride acts as Lewis acid?

Which of the following mixture is a buffer solution?

Which of the following is Lewis acid?

For an equilibrium $\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(\mathrm{l})$ which of the following statements is true:

Assertion : ${pH}$ of hydrochloric acid solution is less than that of acetic acid solution of the same concentration.

Reason : In equimolar solutions, the number of titrable protons present in hydrochloric acid is less than that persent in acetic acid.

The equilibrium constants of the following are.

${\mathrm{N}_2} + 3{\mathrm{H}_\mathrm{2}}\leftrightharpoons2\mathrm{N}{\mathrm{H}_3}\mathrm{ }{\mathrm{K}_1}$

${\mathrm{N}_\mathrm{2}}\mathrm{ + }{\mathrm{O}_\mathrm{2}}\leftrightharpoons\mathrm{2NO }{\mathrm{K}_2}$

${\mathrm{H}_\mathrm{2}}\mathrm{ + }\frac{\mathrm{1}}{\mathrm{2}}{\mathrm{O}_\mathrm{2}} \to {\mathrm{H}_\mathrm{2}}\mathrm{O }{\mathrm{K}_3}$

The equilibrium constant $(K)$ of the reaction

$2\mathrm{N}{\mathrm{H}_3}\mathrm{ + }\frac{5}{2}{\mathrm{O}_2}\overset K \leftrightarrows \mathrm{2NO + 3}{\mathrm{H}_2}\mathrm{O,}$ will be

The pH of solution, whose hydrogen ion concentration is one mole per litre, will be:

The rate constant for forward reaction and backward reaction of hydrolysis of ester are ${1.1 \times {{10}^{ - 2}}}$ and ${1.5 \times {{10}^{ - 3}}}$ per minute respectively. Equilibrium constant for the reaction is

$\mathrm{C}{\mathrm{H}_3}\mathrm{COO}{\mathrm{C}_2}{\mathrm{H}_5} + {\mathrm{H}_2}\mathrm{O}\;\leftrightharpoons\;\mathrm{C}{\mathrm{H}_3}\mathrm{COOH} + {\mathrm{C}_2}{\mathrm{H}_5}\mathrm{OH}$

Which of the following is a Bronsted acid as well as Bronsted base:

Unit of equilibrium constant for the reversible reaction ${H}_2+{I}_2 \rightleftharpoons$ $2 {HI}$ is

pH of a $0.0001\;\mathrm{ }M\;\mathrm{ }HCl$ solution is

If acetic acid is mixed with sodium acetate then ${\mathrm{H}^ + }$ ion concentration will

Assertion(A) ${BF}_3$ is a Lewis acid as well as Bronsted-Lowry acid.

Reason(R) Any species which can accept a lone pair of electrons is a Lewis acid and the species that can lose a proton is Bronsted-Lowry acid.

Maximum possible $\mathrm{pH}$ of a solution of slaked lime is $\left[\mathrm{K}_{\mathrm{SP}}\right.$ of $\left.\mathrm{Ca}(\mathrm{OH})_2=32 \times 10^{-6}\right]$:

Given the reaction between 2 gases represented by ${A_2}$ and ${B_2}$ to give the compound $A{B_{\left( \mathrm{g} \right)}}\mathrm{.}$
${A_{2\left( \mathrm{g} \right)}} + {B_{2\left( \mathrm{g} \right)}}\;\leftrightharpoons\;2A{B_{\left( \mathrm{g} \right)}}$
At equilibrium, the concentration
of ${A_2} = 3.0 \times {10^{ - 3}}\;\mathrm{M}$
of ${B_2} = 4.2 \times {10^{ - 3}}\;\mathrm{M}$
of $AB = 2.8 \times {10^{ - 3}}\;\mathrm{M}$
If the reaction takes place in a sealed vessel at $527^\circ C$, then the value of ${K_c}$ will be :

For the reaction ${N}_2(\mathrm{g})+{O}_2(\mathrm{g}) \rightleftharpoons 2 {NO}(\mathrm{g})$, the value of ${K}_{{C}}$ at $800^{\circ} \mathrm{C}$ is $0.1.$ What is the value of ${K}_{{P}}$ at this temperature?

On doubling ${P}$ and ${V}$ with constant temperature the equilibrium constant will

Which one of the following statements is not true?

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 :

For which reaction Kp � Kc ?