Calculate the number of moles of HCl added to the beaker when 100 cm^3 of 0.250 mol dm^-3 hydrochloric acid is used.
Complete Table 2.1 by entering the initial and final readings for titration 1, working out the volume of NaOH used in each titration, and placing a tick (✓) next to the best titration results.
Use the titration results with ✓ to find the mean volume of NaOH used.
Use your result from (b)(ii) to calculate the number of moles of 0.100\text{ mol dm}^{-3} NaOH that react with 25.0\text{ cm}^3 of B.
Calculate the amount in moles of NaOH that react with 100\text{ cm}^3 of B.
Use your answers to (a) and (d) to calculate the number of moles of HCl that react with the calcium carbonate in the sample of A.
The reaction equation is $\text{2HCl} + \text{CaCO}_3 \rightarrow \text{CaCl}_2 + \text{H}_2\text{O} + \text{CO}_2$. Calculate the number of moles of calcium carbonate in the sample of A.
Give a reason for stirring the reactants together.
Give a reason for waiting until the effervescence stops.
Explain why a measuring cylinder gives an inaccurate volume of HCl used. Suggest an improvement.
Explain why the burette is rinsed with sodium hydroxide after being rinsed with water.