The hydrogen ion concentration of a fruit juice is 3.3 x 10^-2 M. What is the pH of the juice? Is it acidic or basic?

Calculate the pH of a buffer containing 0.08 mole of acetic acid and 0.12 mole of sodium acetate per dm, of the solution. The ionisation constant of acetic acid is 1.8 x 10^-5.

Calculate the pH of 0.1 M acetic acid if its ionisation constant Ka = 1.8 x 10^-5.

pH of a solution is 5.5 at 25°C. Calculate its [OH^-].

Calculate the pH of solution with HO⁺ concentrations in mol dm^-3.
(i) 10^-4
(ii) 10^-7
(iii) 6.8 x 10^-3
(iv) 3.2 x 10^-5
(v) 0.035
(vi) 0.25
(vii) 5.4 x 10^-9
(viii) 7.1 x 10^-7

Calculate the pH of 0.02 m Ba(OH)₂ aqueous solution assuming Ba(OH)₂ as a strong electrolyte.

The ionisation constant of 0.2 M formic acid is 1.8 x 10^-4. Calculate its percentage ionisation.

Calculate the pH of 0.001 M HCI solution.

Calculate the pH of a buffer mixture which contains 7.5 gms if acetic acid and 10.25 gms of sodium acetate in 1 litre of the solution. K_a for acetic acid is 1.8 x 10^-5.

If a solution has a pH of 7.41, determine its H⁺ concentration.

Calculate the pH of 0.02 MHCl.

The degree of dissociation of acetic acid in 0.1 Msolution is 0.04. Calculate K_a for acetic acid. Where a is the degree of dissociation, C is the concentration of the acid in moles/ lit.

Calculate the K_b for ammonium hydroxide given its degree of dissociation to be 0.042 in 0.01 N solution.

A 0.02 M solution of a weak mono basic acid is 5% ionised. Calculate the ionisation constant of the acid.

Calculate the hydrogen ion concentration from the following pH value:
(i) 5.5
(ii) 8.6 and
(iii) 3.2