0.3 g of an acid is neutralized by `40 cm^(3)` of 0.125 N NaOH. Equivalent mass of the acid is

Exactly 20.0 cm^(3) of nitric acid neutralized 28.4 cm^(3) of 0.25 M NaOH. What is the molarity of the acid?

0.1092 g of a dibasic acid is exactly neutralized by 21cm^(3) of 0.1N NaOH. Calculate the molecular mass of the acid.

0.104 g of a monobasic acid was just neutralised y 10 ml (N)/(20) NaOH. Molar mass of the acid is

0.45 g of an acid ( mol. Mass = 90 ) is neutralised by 20 mol of 0.5 N NaOH solution. The basicity of the acid is :

0.45 g of acid (mol. Wt. =90 ) was exactly neutralized by 20 ml of 0.5(M) NaOH . The basicity of the given acid is

0.45 g of acid (mol. Wt. =90 ) was exactly neutralized by 20 ml of 0.5(M) NaOH . The basicity of the given acid is

0.45 g of acid (mol. Wt. =90 ) was exactly neutralized by 20 ml of 0.5(M) NaOH . The basicity of the given acid is

0.45 gm of an acid with molecular mass 90 g/mole is neutralized by 20 ml of 0.5 N caustic potash. The basicity of the acid is :

18.5 cm^(3) of oxalic acid was completely neutralised by 20.0 cm^(3), 0.125 N base. Calculate the (a) normality (b) molarity and ( c) mass of oxalic acid crystals in 1 dm^(3) of solution.