Equilibrium practice · Easy

Tribasic acid furnishes…type of anions.

The relationship between ${K_P}\mathrm{ \,\, and\,\, }{K_C}$ is given by

Equilibrium constants for some reactions are given. In which of the following case does the reaction go farthest to completion?

The hydronium ion concentration in an aqueous solution of $\mathrm{H}_2 \mathrm{SO}_4$ is $2.0 \times 10^{-4} \mathrm{M}$ at $25^{\circ} \mathrm{C}.$ The hydroxide ion concentration in the solution is

Calculate the$\;\mathrm{pOH}$ of a solution at $25^\circ C$ that contains $1 \times {10^{ - 10}}\;M$ of hydronium ions $i.e.,\;\;\mathrm{H}_3^ + \mathrm{O}$:

Statement-I: Acids and bases are conductors of electricity in aqueous solutions

Statement-II: Acids and bases ionise in water

Consider the following reaction at equilibrium
${N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g)$
if small amount of Helium gas is added to the reaction mixture at constant pressure then

The oxo-acid of anhydride ${\mathrm{P}_2}{\mathrm{O}_5}$ is:

Strongest acid is

For the reaction, ${C_2}{H_4}(g) + {H_2}(g)\underset{{}}{\overset{{}}{\leftrightharpoons}}{C_2}{H_6}\left( g \right)$ the equilibrium constant has the units

At $600\,,\,{K_p}$ for the following reaction is 1 atm.

$X\left( \mathrm{g} \right)\,\,\,\leftrightharpoons\,\,\,Y\left( \mathrm{g} \right) + Z\left( \mathrm{g} \right)$

At equilibrium, $50\,\%$ of $X\left( \mathrm{g} \right)$ is dissociated. The total pressure of the equilibrium system is $p$ atm. What is the partial pressure (in atm) of $X\left( \mathrm{g} \right)$ at equilibrium?

The conjugate base of ${\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ in the following reaction is:

${\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4} + {\mathrm{H}_2}\mathrm{O}\;\leftrightharpoons\;{\mathrm{H}_3}{\mathrm{O}^ + } + \mathrm{HSO}_4^ -$

The ${pH}$ of a $10^{-3} \,{M} \,{HCl}$ solution at $25^{\circ} {C}$ if it is diluted 1000 times, will be-

Which of the following has concentration dependent $\mathrm{pH}$ ?

The indicator used in the titration of sodium carbonate with sulphuric acid is

According to Le-Chatelier principle, adding heat a solid and liquid in equilibrium will cause the

For the reaction, ${N_2}(g) + 3{H_2}(g)\,\leftrightharpoons\,2N{H_3}(g),\,$ If the value of equilibrium constant is $K,$ then the equilibrium constant for the reaction, $N{H_3}(g)\,\leftrightharpoons\,\frac{1}{2}{N_2}(g) + \frac{3}{2}{H_2}(g)\,$ will be

In the reaction, ${\mathrm{N}_2}{\mathrm{O}_4}\;\leftrightharpoons\;2\mathrm{N}{\mathrm{O}_2}$, $\mathrm{\alpha }$ is that part of ${\mathrm{N}_2}{\mathrm{O}_4}$ which dissociates, then the number of moles at equilibrium will be

For the reaction, $PC{l_3}(g) + C{l_2}(g)PC{l_5}(g)$ at ${250^0}C$, the value of ${K_C}$ is 26, then the value of ${K_P}$ at the same temperature will be

Tetramine copper (II) sulphate is an example of:

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

Statement I: For the reaction $\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g}),$ equilibrium moles of $\text{A}$ and $\text{B}$ are, respectively, '$a$' and ' $b$ ' in $1 \mathrm{~L}$ container. If 5 moles of $\mathrm{A}$ and 3 moles of $\mathrm{B}$ are added, then reaction must move in forward direction.

Statement II: Even if the amount of reactant added to a system at equilibrium is more than the amount of product added at the same time, the equilibrium can shift in any direction.

What is the $\mathrm{pH}$ of the resulting solution when equal volumes of $0.1\,m\,NaOH\,and\,0.01\,M\,HCl$ are mixed?

For the hypothetical reaction, $A(g) \rightleftharpoons B(g)+C(g)$ the correct relation between ${Kp}$ and ${Kc}$ at $12.18 \mathrm{~Kelvin}$ is

The $\mathrm{pH}$ of $\frac{\mathrm{M}}{100} \mathrm{Ca}(\mathrm{OH})_2$ is

The $\mathrm{pH}$ of $0.1\;M\;\mathrm{HCl}$ is approximately 1. The approximate $\mathrm{pH}$ of $0.05\;M\;{\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ is:

For the reaction: $\mathrm{NH}_4 \mathrm{HS{(s})} \rightleftharpoons \mathrm{NH}_{3}(\mathrm{g})+\mathrm{H}_2 \mathrm{S{(g})}$
The unit of $\mathrm{Kp}$ for the reactions is

The ${K_C}$ for ${H_2}(g) + {I_2}(g)2HI(g)$ is 64, if the volume of the container is reduced to one-half of its
original volume, the value of equilibrium constant will be

The Henderson’s equation used to calculate the $\mathrm{pOH}$ of basic buffer is:

Which addition would not change the $\mathrm{pH}$ of $10\,\mathrm{mL}$ of dilute hydrochloric acid?