Ionic Equilibrium

What is the conjugate base of OH⁻?

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

Species acting as both Bronsted acid and base is :

The conjugate base of H₂PO₄⁻ is :

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?

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

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 :

The pK_a of a weak acid, HA, is 4.80. The pK_b of a weak base, BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be

At 25°C, the solubility product of Mg(OH)₂ is 1.0 $\times$ 10^–11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001 M Mg²⁺ ions?

The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, K_a of this acid is :