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

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

A is \(0.125\ \text{mol dm}^{-3}\) H\(_2\)SO\(_4\). B is a solution containing X \(\text{g dm}^{-3}\) of NaOH.

(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. Record the volume of your pipette. Tabulate your burette readings and calculate the average volume of A used. The equation for the reaction involved in the titration is H\(_2\)SO\(_4\) + 2NaOH\(_{(aq)}\) \(\to\) Na\(_2\)SO\(_4\) + 2H\(_2\)O\(_{(l)}\)

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

(i) amount of H\(_2\)SO\(_4\) in the average volume of A used

(ii) Concentration of B in \(\text{mol dm}^{-3}\)

(iii) value of X.

[H = 1: O = 16; Na = 23]

(c) Describe briefly a suitable laboratory procedure for obtaining pure water from the titration mixture. (No diagram is required)