Equilibrium practice · Medium

Calculate the concentration of $\mathrm{OH}$ in the solution of base with $\mathrm{pH}=12.301$.

The equilibrium constant for the reaction ${Br}_2 \rightleftharpoons 2 {Br}$ at $500 {~K}$ and $700 {~K}$ are $1 \times 10^{-10}$ and $1 \times 10^{-5}$ respectively. The reaction is;

(A): Benzoic acid $\left(K_a=6.5 \times 10^{-5}\right)$ is stronger acid than acetic acid

$\left(K_a=1.74 \times 10^{-5}\right)$

(R): Larger the value of $K_a$, greater is the acidity.

Identify the correct order of acidic strength of $\mathrm{C}{\mathrm{O}_2},\mathrm{CuO},\mathrm{CaO},{\mathrm{H}_2}\mathrm{O}:$

$\mathrm{N}_2 \mathrm{O}_4$ is $50 \%$ dissociated into $\mathrm{NO}_2$ at equilibrium. The vapour density of the gaseous mixture at equilibrium is

Which of the following statements are correct?

(i) Ionic product of water $\left({K}_{{w}}\right)=\left[{H}^{+}\right]\left[{OH}^{-}\right]=10^{-14} {M}^2$

(ii) At $298 {~K}\left[{H}^{+}\right]=\left[{OH}^{-}\right]=10^{-7}$

(iii) ${K}_{{w}}$ does not depends upon temperature

(iv) Molarity of pure water $=55.55 \,{M}$

Statement-1: In acidic medium ${Zn}^{2+}$ is not precipitated by ${S}^{-2}$ ions. and

Statement-2: Common ion effect increases the concentration of ${S}^{-2}$ ions

For the reaction $2 \mathrm{~A}(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}_2(\mathrm{~g})$ the equilibrium constant $K_p$ at $300 \mathrm{~K}$ is 16.0 . The value of $\mathrm{K}_{\mathrm{p}}$ for $\mathrm{AB}_2(\mathrm{~g}) \rightleftharpoons \mathrm{A}(\mathrm{g})+\frac{1}{2} \mathrm{~B}_2(\mathrm{~g})$ is:

How will increase of pressure affect the equation?

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

$100 \mathrm{~mL}$ of a solution contains $2 \mathrm{~g}$ of acetic acid and $3 \mathrm{~g}$ of sodium acetate providing ${K}_{{a}}=1.8 \times 10^{-5}$ then choose the correct option

STATEMENT-1 : The gas phase reaction $\mathrm{PCl}_3(g)+\mathrm{Cl}_2(g) \rightleftharpoons \mathrm{PCl}_5(g)$ shifts to the right on increasing pressure.

STATEMENT-2 : When pressure increases, equilibrium shifts towards more number of moles.

$\mathrm{Ca}\left(\mathrm{HCO}_3\right)_2(s)$ decomposes as $\mathrm{Ca}\left(\mathrm{HCO}_3\right)_2(s) \longrightarrow \mathrm{CaCO}_3(s)+\mathrm{H}_2 \mathrm{O}(g)+\mathrm{CO}_2(g)$
Total pressure at equilibrium is found to be 0.12 bar. Thus $K_p$ is

$\mathrm{H}_2 \mathrm{~S}$ is passed into $1 \mathrm{~dm}^3$ of a solution containing 0.1 mole of $\mathrm{Zn}^{2+}$ and 0.01 mole of the $\mathrm{Cu}^{2+}$ till the sulphide ion concentration reaches $8.1 \times 10^{-19}$ mole. Which one of the following statements is true? [ $K_{\mathrm{sp}}$ of Zns and CuS are $3 \times 10^{-22}$ and $8 \times 10^{-36}$, respectively].

Which of the following statement is correct?

$A\left( \mathrm{g} \right) + B\left( \mathrm{g} \right)\;\leftrightharpoons\;AB\left( \mathrm{g} \right)$ is a reversible reaction. At equilibrium 0.4 mole of $AB$ is formed when each $A$ and $B$ are taken one mole. How much of $A$ changes into $AB$?

Which among the following is an electron deficient compound?

Given below are two statements one is labelled as Assertion A and the other is labelled as Reason R:
Assertion A: The amphoteric nature of water is explained by using Lewis acid/base concept
Reason R: Water acts as an acid with $N{H_3}$ and as a base with ${H_2}S.$
In the light of the above statements choose the correct answer from the options given below:

The equilibrium constants for the reaction,

$\begin{aligned} & \mathrm{Zn}(s)+\mathrm{Cu}^{2+}(a q) \rightleftharpoons \mathrm{Zn}^{2+}(a q)+\mathrm{Cu}(s) \text { and } \\ & \mathrm{Cu}(s)+2 \mathrm{Ag}^{+}(a q) \rightleftharpoons \mathrm{Cu}^{2+}(a q)+2 \mathrm{Ag}(s) \end{aligned}$

are $K_1$ and $K_2$ respectively. The equilibrium constant for the combined reaction is

One litre of an aqueous solution contain 0.15 moles of $C{H_3}COOH\left( {pka = 4.8} \right)$ and 1.5 mole of $C{H_3}COONa$ . The pH of solution is:

The $\mathrm{pH}$ of $10^{-11} \mathrm{~M} {~HCl}$ at $25^{\circ} \mathrm{C}$ is

Solution of $0.1 \mathrm{~M} \mathrm{~NH}_4 \mathrm{OH}$ and $0.1 \mathrm{~M} \mathrm{~NH}_4 \mathrm{Cl}$ has $\mathrm{pH} ~9.25$, The $\mathrm{pK}_{\mathrm{b}}$ of $\mathrm{NH}_4 \mathrm{OH}$ is;

Assertion(A) ${CaO}$ donates oxide, hence it is a base and ${CO}_2$ accepts an oxide, hence it is an acid. This is in accordance with Lux-Flood concept.

Reason(R) ${Cu}^{+}, {Ag}^{+}, {Au}^{+}$, etc., are soft acids while ${Li}^{+}, {Na}^{+}, {Ca}^{+}$, etc., are hard acids.

$\Delta G^{\circ}$ for the reaction $\mathrm{X}+\mathrm{Y} \rightleftharpoons \mathrm{C}$ is $-4.606 \mathrm{~kcal}$ at $1000 \mathrm{~K}.$ The equilibrium constant for the reverse mode of the reaction is

(A): In presence of dilute ${HCl}, {Zn}^{2+}$ is not precipitated by $S^{2-}$ ions

(R): The dissociation of ${H_2}S$ is suppressed by addition of dilute $HCl$.

The following reactions are known to occur in the body,

$\mathrm{C}{\mathrm{O}_2} + {\mathrm{H}_2}\mathrm{O}\leftrightharpoons{\mathrm{H}_2}\mathrm{C}{\mathrm{O}_3}\leftrightharpoons{\mathrm{H}^ + } + \mathrm{HCO}_3^ -$

If $\mathrm{C}{\mathrm{O}_2}$ escapes from the system, then:

The hydrolysis constant for $\mathrm{ZnCl}_2$ will be

Where, ${K}_{\mathrm{b}}$ is effective dissociation constant of base $\mathrm{Zn}^{++}$

Statement (S): Hydrolysis of salt is an exothermic phenomenon.

Explanation (E): It involves breaking up of water molecule of produce acid and base respectively.

Calculate the concentration of hydrogen ion in the acidic solution with $\mathrm{pH}=$ 4.3

At $1000 \mathrm{~K}$, pressure of $\mathrm{CO}_2$ in equilibrium with $\mathrm{CaCO}_3$ and $\mathrm{CaO}$ is equal to $2.105 \mathrm{~atm}$. The equilibrium constant for the reaction,
$\mathrm{C}(s)+\mathrm{CO}_2(g) \rightleftharpoons 2 \mathrm{CO}(g)$
is 1.9 at the same temperature when pressure are in atm. Solid $\mathrm{C}, \mathrm{CaO}$, and $\mathrm{CaCO}_3$ are mixed and allowed to come to equilibrium at $1000 \mathrm{~K}$ in a closed vessel. What is the pressure of $\mathrm{CO}(\mathrm{g})$ at equilibrium (in $\mathrm{atm}$ )?

Solution of $0.1 \mathrm{~N} {~NH}_4 {OH}$ and $0.1 \mathrm{~N} {~NH}_4 {Cl}$ has pH $9.25.$ Then find out ${pK}_{{b}}$ of ${NH}_4 {OH}$