Nitric acid can be neutralised by adding sodium hydroxide solution. The equation for the reaction is:
HNO3+NaOH→NaNO3+H2O \text{HNO}_3 + \text{NaOH} \rightarrow \text{NaNO}_3 + \text{H}_2\text{O} HNO3+NaOH→NaNO3+H2OA solution of nitric acid has a concentration of 0.125 mol/dm30.125\text{ mol/dm}^30.125 mol/dm3.
Calculate the amount, in moles, of HNO3\text{HNO}_3HNO3 in 60.0 cm360.0\text{ cm}^360.0 cm3 of the nitric acid solution.
Calculate the volume of 0.150 mol/dm30.150\text{ mol/dm}^30.150 mol/dm3 sodium hydroxide solution needed to exactly neutralise the nitric acid. Give the unit.
In another neutralisation reaction, a student uses 35.0 cm335.0\text{ cm}^335.0 cm3 of 0.800 mol/dm30.800\text{ mol/dm}^30.800 mol/dm3 aqueous sodium hydroxide solution.
Calculate the mass of sodium hydroxide contained in this solution. [Relative atomic masses, ArA_rAr: H=1\text{H} = 1H=1, O=16\text{O} = 16O=16, Na=23\text{Na} = 23Na=23]
