Topic 9 ReactionsofAcids. Titrations Burette with acid solution e.g. dilute hydrochloric acid HCl(aq) Alkali solution e.g. sodium hydroxide NaOH(aq) +

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Topic 9 ReactionsofAcids

Titrations Burette with acid solution e.g. dilute hydrochloric acid HCl(aq) Alkali solution e.g. sodium hydroxide NaOH(aq) + indicator White tile

We use the following formula: P acid x V acid x C acid = P alkali x V alkali x C alkali Where P= power V= volume (l) C=Concentration

Power of the acid is the number of H + ions in the formula HCl has a power of 1 HNO 3 has a power of 1 H 2 SO 4 has a power of 2 Power of the alkali is the number of OH - ions in the formula NaOH has a power of 1 Mg(OH) 2 has a power of 2

Example 1 Q. In a titration, 25cm 3 of 0.1 mol/l NaOH was exactly neutralised by 22.2cm 3 of hydrochloric acid. Calculate the concentration of the hydrochloric acid. A. P acid x V acid x C acid = P alkali x V alkali x C alkali C acid = P alkali x V alkali x C alkali P acid x V acid

C acid = P alkali x V alkali x C alkali P acid x V acid C acid = 1 x x x C acid = 0.11mol/l Therefore the concentration of acid is 0.11mol/l.

Example 2 Q. What volume of 0.2mol/l sulphuric acid will exactly neutralise 25.0cm 3 of 0.5 mol/l potassium hydroxide? A. P acid x V acid x C acid = P alkali x V alkali x C alkali V acid = P alkali x V alkali x C alkali P acid x C acid

V acid = P alkali x V alkali x C alkali P acid x C acid V acid = 1 x x x 0.2 V acid = l Therefore 31.25cm 3 will neutralise the alkali.