Ionic Equilibrium

Species acting as both Bronsted acid and base is :

The conjugate base of H₂PO₄⁻ is :

What is the conjugate base of OH⁻?

The first and second dissociation constants of an acid H₂A are 1.0 $$\times$$ 10^−5 and 5.0 $$\times$$ 10^−10 respectively. The overall dissociation constant of the acid will be :

Four species are listed below i. $$HCO_3^−$$ ii. $$H_3O^+$$ iii. $$HSO_4^−$$ iv. $$HSO_3F$$ Which one of the following is the correct sequence of their acid strength?

Three reactions involving $$H_2PO_4^−$$ are given below : (i) H₃PO₄ + H₂O $$\to$$ H₃O⁺ + $$H_2PO_4^−$$ (ii) $$H_2PO_4^−$$ + H₂O $$\to$$ $$HPO_4^{2−}$$ + H₃O⁺ (iii) $$H_2PO_4^−$$ + OH⁻ $$\to$$H₃PO₄ + O²⁻ In which of the above does $$H_2PO_4^−$$ act as an acid?

How many litres of water must be added to 1 litre of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2?

pK_a of a weak acid (HA) and pK_b of a weak base (BOH) are 3.2 and 3.4, respectively. The pH of their salt (AB) solution is :

Which of the following are Lewis acids?

Which of the following is a Lewis acid?

The decreasing order of electrical conductivity of the following aqueous solutions is : 0.1 M Formic acid (A), 0.1 M Acetic acid (B), 0.1 M Benzoic acid (C)

Which of the following compound CANNOT act as a Lewis base?

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 :

$${K_{{a_1}}}$$, $${K_{{a_2}}}$$ and $${K_{{a_3}}}$$ are the respective ionization constants for the following reactions (a), (b) and (c). (a) $${H_2}{C_2}{O_4} \mathbin{\lower.3ex\hbox{$\buildrel\textstyle\rightarrow\over {\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}$}} {H^ + } + H{C_2}O_4^ -$$ (b) $$H{C_2}O_4^ - \mathbin{\lower.3ex\hbox{$\buildrel\textstyle\rightarrow\over {\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}$}} {H^ + } + {C_2}O_4^{2 - }$$ (c) $${H_2}{C_2}O_4^{} \mathbin{\lower.3ex\hbox{$\buildrel\textstyle\rightarrow\over {\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}$}} 2{H^ + } + {C_2}O_4^{2 - }$$ The relationship between $${K_{{a_1}}}$$, $${K_{{a_2}}}$$ and $${K_{{a_3}}}$$ is given as :

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

1 M NaCL and 1 M HCL are present in an aqueous solution. The solution is

When rain is accompanied by a thunderstorm, the collected rain water will have a pH value :

Hydrogen ion concentration in mol / L in a solution of pH = 5.4 will be :

The pK_a of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid is ionized is :