Neutralisation and buffers

Chemistry @ KZN

Exercises pH-calculations in acid-base-mixtures

Always first figure out whether the substances present are acid or base, weak or strong

Exercise 1

Exercise 2

Exercise 3

Exercise 4

Exercise 5

Exercise 6

Cacluate the resulting pH if 1 litre of hydrochloric acid with c(HCl) = 0.20 mol/L and 1 litre of ammonia with c(NH₃) = 0.10 mol/L are mixed.

pH of the solution:

Cacluate the pH of a solution containing 0.50 mol formic acid and 0.50 mol sodium formate.

pH of the solution:

Cacluate the pH of a solution containing 0.10 mol hydrogen cyanide (HCN) and 0.05 mol potassium cyanide (KCN).

pH of the solution:

Calculate the pH of 500 mL of a solution containing 1 g ammonia (NH₃) and 5 g ammonium chloride (NH₄Cl)

	NH₃	NH₄Cl
mass (g)
molar mass (g/mol)
amount of substance (mol)
concentration

pH of the solution:

Calculate the pH of 1 litre of a buffer solution containing 0.48 mol of acetic acid and 0.52 mol of sodium acetate before and after the addition of 0.01 mol NaOH

	before	after
amount of substance CH₃COOH (mol)
amount of substance NaCH₃COO (mol)
pH

Calculate the pH of 1 litre of a solution containing 0.48 mol of acetic acid and 0.52 mol of sodium acetate before and after the addition of 0.70 mol NaOH

	before	after
amount of substance CH₃COOH (mol)
amount of substance NaCH₃COO (mol)
amount of substance OH⁻ (mol)
pH