1.35g of an unknown solid with the chemical formula (X_{3}*C*O_{3}) was dissolved in water to make 500c * m ^ 1 of solution. 50c * m ^ 3 of the solution was poured into a conical flask and titrated against 0.1mol / d m3 hydrochloric acid. The amount of acid that was required to neutralise the solution was 19.5c * m ^ 3 The balanced symbol equation for the reaction is shown below. X_{2}*C*O_{3} + 2HCl -> 2XCl + C*O_{2} + H_{2}*O Determine the identity of metal X.
