Ionic Equilibrium

The molar solubility (in ol L⁻¹) of a sparingly soluble salt MX₄ is "s". The corresponding solubility product is K_sp. 's' is given in term of K_sp by the relation :

Given below are two statements : Statement (I) : A Buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities Statement (II) : Blood is naturally occurring buffer solution whose $$\mathrm{pH}$$ is maintained by $$\mathrm{H}_2 \mathrm{CO}_3 / \mathrm{HCO}_3{ }^{\ominus}$$ concentrations. In the light of the above statements, choose the correct answer from the options given below :

The equilibrium $$\mathrm{Cr}_2 \mathrm{O}_7^{2-} \rightleftharpoons 2 \mathrm{CrO}_4^{2-}$$ is shifted to the right in :

An aqueous solution contains 0.10 M H₂S and 0.20 M HCl. If the equilibrium constants for the formation of HS^– from H₂S is 1.0 $$\times$$ 10^–7 and that of S²⁻ from HS^– ions is 1.2 $$\times$$ 10^–13 then the concentration of S²⁻ ions in aqueous solution is :

Which of the following salts is the most basic in aqueous solution?

The pH of a 0.02 M NH₄Cl solution will be : [given K_b (NH₄OH) = 10^–5 and log 2 = 0.301]

Given below are two statements : One is labelled as Assertion A and the other labelled as reason R Assertion A : During the boiling of water having temporary hardness, Mg(HCO₃)₂ is converted to MgCO₃. Reason R : The solubility product of Mg(OH)₂ is greater than that of MgCO₃. In the light of the above statements, choose the most appropriate answer from the options given below :

$$20 \mathrm{~mL}$$ of $$0.1\, \mathrm{M} \,\mathrm{NH}_{4} \mathrm{OH}$$ is mixed with $$40 \mathrm{~mL}$$ of $$0.05 \mathrm{M} \mathrm{HCl}$$. The $$\mathrm{pH}$$ of the mixture is nearest to : (Given : $$\mathrm{K}_{\mathrm{b}}\left(\mathrm{NH}_{4} \mathrm{OH}\right)=1 \times 10^{-5}, \log 2=0.30, \log 3=0.48, \log 5=0.69, \log 7=0.84, \log 11= 1.04)$$

Given below are two statements : Statement (I) : Aqueous solution of ammonium carbonate is basic. Statement (II) : Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on $$K_a$$ and $$K_b$$ value of acid and the base forming it. In the light of the above statements, choose the most appropriate answer from the options given below :

Let the solubility of an aqueous solution of Mg(OH)₂ be x then its K_sp is :