What is the minimum volume of water required to dissolve 1g of calcium sulphate at 298 K? (For calcium sulphate, K_sp is 9.1 x 10^-6).

The ionization constant of acetic acid is 1.74 × 10^–5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.

An equilibrium mixture at 300K contains N₂ O₄ and NO₂ at .28 and 1.1 atm pressure respectively. If the volume of the container is doubled, calculate the new equilibrium pressure of two gases.

The ionization constant of dimethylamine is 5.4 × 10^–4. Calculate its degree of ionization in its 0.02M solution. What percentage of dimethylamine is ionized if the solution is also 0.1M in NaOH?

At 473K, equilibrium constant K_c for decomposition of phosphorus pentachloride Pcl₅ is \(8.3\times { 10 }^{ -3 }\) . If decomposition is depicted as, 
\({ PCl }_{ 5 }(g)\leftrightharpoons { PCl }_{ 3 }(g)+{ Cl }_{ 2 }(g);\)
\( \Delta H°=124.0 \ { kJmol }^{ -1 }\)
What would be the effect on \({ K }_{ c } \) if (a) more PCl₅   is added (b) pressure is increased (c) the temperatured in increased ?

4.9 g of sulphuric acid is present in 500 mL of the solution. Calculate the pH of the solution?

At 298 K, a 0.1M solution of acetic acid is 1.34% ionised. What is the ionisation constant K_a of acetic acid?

Find out the value of K_c for each of the following equilibria from the value of K_p:
(a) \(2 \mathrm{NOCl}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g}) ; K_{p}=1.8 \times 10^{-2} \text { at } 500 \mathrm{~K}\)
(b) \(CaCO_{ 3 }(s)\leftrightharpoons CaO(s)+CO_{ 2 }(g); { K }_{ p }=167at1073 \ K\)

The ionisation constant of HF,HCOOH and HCN at 298 are  6.8 x 10^-4 and 4.8 x 10 ^-9 respectively.Calculate the ionisation constant of the corresponding conjucate bases.
To find Kb of  a conjugate  base , use the formula K_a.K_b = K_w = 1 x 10^-14  Conjugate bases of HF,HCOOH and HCN are F^- HCOO^- and CN^- respectively.

The average concentration of SO₂ in atmosphere over a city on a certain a city on a certain  day is 10 ppm.when the average temperature is 298 k.Given that the solubility of SO₂ in water at 298 k is 1,3653 mol/L and the pKa of H₂SO₃ is 1.92. estimate the pH of acid rain on that day.

50.0 g of CaCO₃ are heated to 1073 K in a 5L vessel. What percent of the CaCO₃ would decompose at equilibrium? K_p for the reaction.
\({ CaCO }_{ 3 }(s)\rightleftharpoons CaO(s)+{ CO }_{ 2 }(g)\) is 1.15 a/m at 1073 K.

The degree of dissociation of PCl₅ at a certain temperature and atmospheric pressure is 0.2. Calculate the pressure at which it will be half (50%) dissociated at the same temperature.

At 450 K, K_p = 2.0 x 10¹⁰ bar^-1 for the equilibrium reaction:
2SO₂ (g) + O₂ (g) ⇄ 2SO₃ (g)
What is K_c at this temperature?

The ionization constant of HF, HCOOH and HCN at 298 K are is 6.8 x 10^-4 , 1.8 x 10^-4 and 4.8 x 10^-9 respectively, Calculate the ionization constant of the corresponding conjugate base.

Write the equilibrium constant (K) expression for the following reactions.
(i) Cu₂+(aq) + 2 Ag (s) ⇌ Cu(s) + 2Ag+ (aq)
(ii) 4HCl (g) + O₂(g) ⇌ 2Cl₂ (g) + 2H₂O(g)