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

In a saturated solution of the sparingly soluble strong electrolyte AgIO3(molecular mass = 283) the equilibrium which sets is AgIO₃(s) ⇌ Ag⁺(aq) + IO^–(aq). If the solubility product constant K_sp of AgIO₃ at a given temperature is 1.0 ×10^-8, what is the mass of AgIO₃ contained in 100 ml of its saturated solution?

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

The first and second dissociation constants of an acid H₂A are 1.0 × 10^-5 and 5.0 × 10^-10 respectively. The overall dissociation constant of the acid will be

Given the reaction between 2 gases represented by A₂ and B₂ to give the compound AB(g).
A₂(g) + B₂(g) ⇌ 2 AB(g).At equilibrium, the concentration
of A₂ = 3.0 × 10–3 M
of B₂= 4.2 × 10–3 M
of AB = 2.8 × 10–3 M
lf the reaction takes place in a sealed vessel at 527°C, then the value of K_c will be :

Given that the equilibrium constant for the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature ?
SO₃(g) ⇌ SO₂(g) + ¹/₂O₂(g)

Buffer solutions have constant acidity and alkalinity because

A buffer solution is prepared in which the concentration of NH₃ is 0.30 M and the concentration of NH₄⁺ is 0.20 M. If the equilibrium constant,Kb for NH₃ equals 1.8 × 10^–5, what is the pH of this solution ? (log 2.7= 0.433).