JEE Main Ionic Equilibrium Practice Questions With Solutions

Given below are two statements : One is labelled as Assertion A and the other is labelled as Reason R

Assertion A : Permanganate titrations are not performed in presence of hydrochloric acid.

Reason R : Chlorine is formed as a consequence of oxidation of hydrochloric acid.

In the light of the above statements, choose the correct answer from the options given below

The plot of $\mathrm{pH}$pH-metric titration of weak base ${\mathrm{NH}}_4\mathrm{OH}$NH_{4} OH vs strong acid HCl looks like :

Class XII students were asked to prepare one litre of buffer solution of $\mathrm{pH}8.26$pH 8.26 by their Chemistry teacher: The amount of ammonium chloride to be dissolved by the student in $0.2\mathrm{M}$0.2 M ammonia solution to make one litre of the buffer is :

(Given: ${\mathrm{pK}}_{\mathrm{b}}\left({\mathrm{NH}}_3\right)=4.74$pK_{b} \left(\right. NH_{3} \left.\right) = 4.74

Molar mass of ${\mathrm{NH}}_3=17\mathrm{g}{\mathrm{mol}}^{-1}$NH_{3} = 17 \textrm{ } g \left(\textrm{ } mol\right)^{- 1}

Molar mass of ${\mathrm{NH}}_4\mathrm{Cl}=53.5\mathrm{g}{\mathrm{mol}}^{-1}$NH_{4} Cl = 53.5 \textrm{ } g \left(\textrm{ } mol\right)^{- 1} )

$K_{a_1}$K_{a_{1}}, $K_{a_2}$K_{a_{2}} and $K_{a_3}$K_{a_{3}} are the respective ionization constants for the following reactions (a), (b) and (c).

(a) $H_2{C}_2{O}_4\overrightarrow{\leftarrow \phantom{{}_{\text{vbox}to.5ex\text{vss}}}}{H}^{+}+H{C}_2{O}_4^{-}$H_{2} C_{2} O_{4} \overset{\rightarrow}{\leftarrow } H^{+} + H C_{2} O_{4}^{-}

(b) $H{C}_2{O}_4^{-}\overrightarrow{\leftarrow \phantom{{}_{\text{vbox}to.5ex\text{vss}}}}{H}^{+}+C_2{O}_4^{2-}$H C_{2} O_{4}^{-} \overset{\rightarrow}{\leftarrow } H^{+} + C_{2} O_{4}^{2 -}

(c) $H_2{C}_2{O}_4^{}\overrightarrow{\leftarrow \phantom{{}_{\text{vbox}to.5ex\text{vss}}}}2H^{+}+C_2{O}_4^{2-}$H_{2} C_{2} O_{4}^{} \overset{\rightarrow}{\leftarrow } 2 H^{+} + C_{2} O_{4}^{2 -}

The relationship between $K_{a_1}$K_{a_{1}}, $K_{a_2}$K_{a_{2}} and $K_{a_3}$K_{a_{3}} is given as :

$20\mathrm{mL}$20 \textrm{ } mL of $0.1\mathrm{M}{\mathrm{NH}}_4\mathrm{OH}$0.1 M NH_{4} OH is mixed with $40\mathrm{mL}$40 \textrm{ } mL of $0.05\mathrm{M}\mathrm{HCl}$0.05 M HCl. The $\mathrm{pH}$pH of the mixture is nearest to :

(Given : ${\mathrm{K}}_{\mathrm{b}}\left({\mathrm{NH}}_4\mathrm{OH}\right)=1\times {10}^{-5},\log 2=0.30,\log 3=0.48,\log 5=0.69,\log 7=0.84,\log 11=1.04)$K_{b} \left(\right. NH_{4} OH \left.\right) = 1 \times 10^{- 5} , log ⁡ 2 = 0.30 , log ⁡ 3 = 0.48 , log ⁡ 5 = 0.69 , log ⁡ 7 = 0.84 , log ⁡ 11 = 1.04 \left.\right)

The solubility of AgCl will be maximum in which of the following?

A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio of $\frac{[C{H}_{3}C{H}_{2}CO{O}^{-}]}{[C{H}_{3}C{H}_{2}COOH]}$\frac{\left[\right. C H_{3} C H_{2} C O O^{-} \left]\right.}{\left[\right. C H_{3} C H_{2} C O O H \left]\right.} required to make buffer is ___________.

Given : $K_a(C{H}_{3}C{H}_{2}COOH)=1.3\times {10}^{-5}$K_{a} \left(\right. C H_{3} C H_{2} C O O H \left.\right) = 1.3 \times 10^{- 5}

The K_sp for bismuth sulphide (Bi₂S₃) is 1.08 $\times$\times 10^$-$-73. The solubility of Bi₂S₃ in mol L^$-$-1 at 298 K is :

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 NH₃ and as a base with H₂S.

In the light of the above statements choose the correct answer from the options given below :