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

F is a solution, O a dibasic acid H\(_2\)X. G is a solution containing 1.00g of sodium hydroxide in 250cm\(^3\) of solution.

(a) Put F in the burette and titrate with 20cm\(^3\) or 25cm\(^3\) portion of G using methyl orange as indicator. Record the volume of your pipette. Tabulate your burette readings and calculate the average volume of F used 

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

(i) concentration of G in mol. dm\(^3\)

(ii) concentration of F in mol. dm\(^{-3}\)

(iii) molar mass of the acid H\(_2\)X, given that 100cm\(^3\) of solution F contained 0.4850 the acid.

The equation for the reaction is H\(_2\)X\(_{(aq)}\) + 2NaOH\(_{(aq)}\) \(\to\) Na\(_2\)X\(_{(aq)}\) + 2H\(_2\)O [H = 1; O = 16; Na = 23]