All your burette readings (initial and final) as well as the size size of your pipette, must be recorded but no account of experimental procedure is require...

All your burette readings (initial and final) as well as the size size of your pipette, must be recorded but no account of experimental procedure is required. All calculations must be done in your answer book.

A is a solution containing \(1.04\text{ g HCl}\) per \(500\text{ cm}^3\) of solution. B was prepared by diluting \(50.0\text{ cm}^3\) of a saturated solution of \(\mathrm{Na}_2\mathrm{CO}_3\) at room temperature to \(1000\text{ cm}^3\)

(a) Put A into the burette and titrate it against \(20.0\text{ cm}^3\) or \(25.0\text{ cm}^3\) portions of B using methyl orange as indicator. Repeat the titration to obtain consistent titres. Tabulate your results and calculate the average volume of acid used.

9b) From your results and information provided above, calculate the;

(i) concentration of A in \(\mathrm{mol\,dm}^{-3}\)

(ii) concentration of B in \(\mathrm{mol\,dm}^{-3}\)

(iii) solubility of \(\mathrm{Na}_2\mathrm{CO}_3\) in \(\mathrm{mol\,dm}^{-3}\)

(iv) volume of \(\mathrm{CO}_2\) that would be liberated from \(1\text{ dm}^3\) of B if the titration were carried out at s.t.p.

The equation for the reaction is \(\mathrm{Na}_2\mathrm{CO}_{3(aq)} + 2\mathrm{HCl}_{(aq)} \to 2\mathrm{NaCl}_{(aq)} + \mathrm{H}_2\mathrm{O}_{(l)} + \mathrm{CO}_{2(g)}\)

[H = 1; C = 12; O = 16; Na = 23; Cl = 35.5; Molar volume of gas at s.t.p = \(22.4\text{ dm}^3\)]