Equilibrium practice · Mixed difficulty

The conjugate acid of $HCO_3^ -$ is

Statement I: In the dissociation of $\mathrm{PCl}_5$ at constant pressure and temperature addition of helium at equilibrium increases the dissociation of $\mathrm{PCl}_5$.

Statement II : Helium removes $\mathrm{Cl}_2$ from the field of action.

$1 \mathrm{~mol}$ of ${N}_2$ and $4 \mathrm{~mol}$ of ${H}_2$ are allowed to react in a vessel to form ${NH}_3$ gas as only product and after reaction, water is added. Aqueous solution required $1 \mathrm{~mol}$ of ${HCl}$ for complete reaction. Mol fraction of ${H}_2$ in the gas mixture after reaction is

Select the anion which is the weakest conjugate base:

Which of the following affects the value of equilibrium constant?

The solids dissociate as follows: $A\left( s \right)\,\leftrightharpoons\,B\left( g \right) + C\left( g \right);\,\,{K_{{P_1}}} = x\,\,\,\mathrm{at}{\mathrm{m}^2}$
$D\left( s \right)\,\leftrightharpoons\,C\left( g \right) + E\left( g \right);\,\,{K_{{P_2}}} = y\,\,\,\mathrm{at}{\mathrm{m}^2}$ The total pressure when both the solids dissociate simultaneously is

$K_1, K_2$ and $K_3$ are the equilibrium constants of the following reactions (I), (II) and (III) respectively:

(I) ${N}_2+2 {O}_2 \rightleftharpoons 2 {NO}_2$

(II) $2 {NO}_2 \rightleftharpoons {N}_2+2 {O}_2$

(III) ${NO}_2 \rightleftharpoons \frac{1}{2} {~N}_2+{O}_2$

The correct relation from the following is

What will be the resultant $\mathrm{pH}$ when $200 \mathrm{~ml}$ of an aqueous solution of ${HCl}(\mathrm{pH}=2.0)$ is mixed with $300 \mathrm{~ml}$ of an aqueous solution of ${NaOH}$ $(\mathrm{pH}=12.0)?$

Calculate the pH and degree of hydrolysis of $0.01 \mathrm{~M}$ solution of $\mathrm{NaCN}, \mathrm{K}_{\mathrm{a}}$ for $\mathrm{HCN}$ is $6.2 \times 10^{-12}.$

Assertion (A): pH of $x \mathrm{~M~HCl}$ is less than pH of $x \mathrm{~M} \mathrm{~CH}_3 \mathrm{COOH}.$

Reason (R): The degree of ionization of HCl and $\mathrm{CH}_3 \mathrm{COOH}$ are equal at infinite dilution.

At $90^\circ C$, pure water has $\left[ {{\mathrm{H}^ + }} \right] = {10^{ - 6}}$ M, if $100\;mL$ of $0.2\;M\;\;HCl$ is added to 200 mL of $0.1\;M\mathrm{ }\;KOH$ at $90^\circ C$ then pH of the resulting solution will be

The correct order of increasing $\left[ {{\mathrm{H}_3}{\mathrm{O}^ + }} \right]$ in the following aqueous solutions is:

For the following gaseous equilibria $\mathrm{X}, \mathrm{Y}$ and $\mathrm{Z}$ at $300 \mathrm{~K}$

$\mathrm{X}: 2{SO}_2+{O}_2 \rightleftharpoons {SO}_3$

$\begin{aligned} & \text {Y}: {PCl}_5 \rightleftharpoons {PCl}_3+{Cl}_2 \\ & \mathrm{Z}: 2 {HI} \rightleftharpoons {H}_2+{I}_2 \end{aligned}$

ratio of $K_p$ and $K_C$ in the increasing order is

Assertion (A): Higher order ionisation constant $\left(K_{a_2}, K_{a_3}\right)$ are smaller than the lower order ionisation constant $\left(K_{a_1}\right)$ of a polyprotic acid.

Reason (R): It is more difficult to remove a positively charged proton from a negative ion due to Coulombic forces.

(A): Water acts as leveling solvent for various acids.

(R): Levelling effect of water is due to its high dielectric constant and strong proton accepting tendency.

Nucleophiles are:

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

In the problem 13, the dissociation constant of acid is :

$\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightleftharpoons \mathrm{CuSO}_4 \cdot 3 \mathrm{H}_2 \mathrm{O}(\mathrm{s})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{g}), K_{\mathrm{P}}$ for this equilibrium is $1.0 \times 10^{-4} \mathrm{~atm}^2$ at $25^{\circ} \mathrm{C}$. What is the maximum pressure of water vapour (moisture) in the atmosphere, below which the pentahydrate is efflorescent?

Assuming 100% ionisation which will have maximum pH

When heated ammonium carbamate decomposes as follows

${NH}_4 {COONH}_2\text{(s)} \Leftrightarrow 2 {NH}_3(\mathrm{g})+{CO}_2(\mathrm{g})$

At a certain temperature, the equilibrium pressure of the system is $0.318 \mathrm{~atm}, {K}_{{p}}$ for the reaction is

Statement I: The solubility of gases always increases with inctease in pressure

Statement II : High prespure favours the change where volume decreases

Assertion :- The pH of an aqueous solution of acetic acid remains unchanged on the addition of sodium acetate.

Reason :- The ionization of acetic acid is suppressed by the addition of sodium acetate.

If $\mathrm{pK}_{\mathrm{b}}$ for fluoride ion at $25^{\circ} \mathrm{C}$ is 10.83 , the ionisation constant of hydrofluoric acid in water at this temperature is:

$100 \mathrm{ml}$ solution (I) of buffer containing $0.1(\mathrm{M}) \mathrm{HA}$ and 0.2 (M) $\mathrm{A}^{-}$, is mixed with another solution (II) of $100 \mathrm{ml}$ containing 0.2(M) HA and 0.3(M) $\mathrm{A^{-}}$ .
After mixing what is the $\mathrm{pH}$ of resulting solution?
Given $\mathrm{pK}_{\mathrm{a}}$ of $\mathrm{HA}=5$

The change in $\mathrm{pH}$ of water when 0.01 mole of $\mathrm{NaOH}$ are added in 10 litre water is :

What minimum concentration of ${SO}_4^{2-}$ is required to precipitate ${BaSO}_4$ from the solution containing $1.0 \times 10^{-4}$ moles of ${Ba}^{2+}$ ? (Given $K_{S P}$ for ${BaSO}_4$ is $4 \times 10^{-10}$ )

The normal vapor density of ${PCl}_5$ is 104.25. At $250^{\circ} \mathrm{C},$ its vapor density is 57.9. The degree of dissociation of ${PCl}_5$ at this temperature will be

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?

${NH}_2-{COONH}_4({s}) \rightleftharpoons 2 {NH}_3({g})+{CO}_2({g})$. Total pressure at equilibrium is equal to $\left({K}_{{p}}=4 \mathrm{~atm}^3\right)$.