An analytical chemist performs a titration to determine the volume of nitric acid required to completely neutralise a sample of calcium hydroxide solution.
The chemist begins with 30.0 cm330.0\text{ cm}^330.0 cm3 of calcium hydroxide solution with a concentration of 0.0800 mol/dm30.0800\text{ mol/dm}^30.0800 mol/dm3.
Nitric acid with a concentration of 0.150 mol/dm30.150\text{ mol/dm}^30.150 mol/dm3 is added from a burette until the neutralisation endpoint is reached.
The equation for this reaction is:
Ca(OH)2+2HNO3→Ca(NO)3)2+2H2O \text{Ca(OH)}_2 + 2\text{HNO}_3 \rightarrow \text{Ca(NO)}_3)_2 + 2\text{H}_2\text{O} Ca(OH)2+2HNO3→Ca(NO)3)2+2H2OCalculate the amount, in moles, of calcium hydroxide used.
Calculate the amount, in moles, of nitric acid needed to neutralise this amount of calcium hydroxide.
Calculate the volume, in cm3cm^3cm3, of nitric acid needed to neutralise this solution of calcium hydroxide.
