The strength of a mixture of HCl & H2SO4 is 0.1 N. On treatment with an excess of AgNO3 solution, 20 ml of this acid mixture gives 0.1435 gm of AgCl. The strength of the H2SO4 is:

Explanation

To find the strength of H2SO4, first calculate the moles of AgCl formed: the molar mass of AgCl is approximately 143.35 g/mol, so 0.1435 g corresponds to 0.001 moles of AgCl. Since AgCl is formed from Cl- ions from HCl, calculate the moles of HCl in the solution: 0.001 moles of Cl- correspond to 0.001 moles of HCl. Given that the total normality of the acid mixture is 0.1 N, and assuming all of this is due to H+ ions from HCl and H2SO4, we can set up an equation based on the stoichiometry of the reactions:2HCl + 2AgNO3 → 2AgCl + 2HNO3H2SO4 + 2AgNO3 → Ag2SO4 + 2HNO3Given the 0.001 moles of HCl, the rest of the 0.1 N is contributed by H2SO4. Therefore, calculate the concentration of H2SO4 using the formula: Concentration (g/litre) = Normality × Equivalent weight = 0.049 x 49 = 2.45 g/litre. Thus, the correct answer is 2.45 g/litre.