Equilibrium Tes...

Solubility of  a solute in a solvent (say water) is dependent on temperature as given by $$ S = A.e^{- \Delta HlRT} $$ , where $$ \Delta H$$ is heat of reaction : solute $$ + H_2O \leftrightharpoons $$ solution. For a given solution, a variation of log S with temperature is shown graphically the solute should be:

Calculate the formation constant for the reaction of a tripositive metal ion with thiocyanate ions to form the monocomplex if the total metal concentration in the solution is $$2 \times 10^{-3} M$$, the total $$SCN^{-}$$ concentration is $$1.51 \times 10^{-3} M$$ and the free $$SCN^{-}$$ concentration is $$1.0 \times 10^{-5} M$$.

A buffer solution is $$0.25 M - CH_{3}COOH + 0.15 M - CH_{3}COONa$$, saturated in $$H_{2}S (0.1 M)$$ and has $$[Mn^{2+}] = 0.04 M$$, $$K_{a}(CH_{3}COOH) = 2.0 \times 10^{-5}$$, $$ K_{a} (H_{2}S) = 1.0 \times 10^{-21}$$ and $$K_{sp}(MnS) = 2.5 \times 10^{-13}$$.

An amount of $$0.10$$ moles of $$AgCl(s)$$ is added to one litre of water. Next, the crystals of $$NaBr$$ are added until $$75$$% of the $$AgCl$$ is converted to $$AgBr(s)$$, the less soluble silver halide. What is $$Br^{-}$$ at this point? 

An amount of $$0.01$$ moles of solid $$AgCN$$ is rendered soluble in $$1 l$$ by adding just sufficient excess cyanide ion to form $$Ag(CN)^{2-}$$ and the concentration of free cyanide ion is $$2.5 \times 10^{-7} M$$. Determine $$[Ag^{+}]$$ in the solution neglecting hydrolysis of cyanide ion. $$K_{diss}$$ for $$Ag(CN)_{2}^{-} = 1.0 \times 10^{-20}$$.

Which of the following processes will increase $$[OH^{-}]$$ in $$NH_{4}OH$$ solution?

Which of the following statement(s) is/are incorrect?

The amino acid alanine has two isomers, $$ \alpha $$ alanine and $$ \beta $$ alanine when equal masses of these two compound are dissolved in equal mass of a solvent, the solution of $$ \alpha $$ alanine freeze at relatively l; lower temperature, which forms $$ \alpha $$ alanine and $$ \beta $$ alanine has the larger equilibrium constant for ionization?

The initial rate of hydrolysis of methyl acetate $$(1.0M)$$ by a weak acid $$(HA,1.0M)$$ is 1/100th of that of a strong acid $$(HX,1.0M)$$, at $${ 25 }^{ o }C$$. The $${K}_{a}$$ of $$HA$$ is

Solid ammonium carbamate dissociates as: $$ NH_2COONH_{4_{(s)}} \rightleftharpoons  2NH_{3_{(g)}} + CO_{2_{ (g)}} $$