30 ml of acid solution is netralized by 15 ml of a 0.2 N base. The srength of acid solution is

If 20 mL of 0.4 N NaOH solution completely neutralised 40 mL of a dibasic acid, the molarity of the acid solution is

If 20ml of 0.4 N NaOH solution completely neutralise 40ml of a dibasic acid, the molarity of the acid solution is:

If 20 mL of 0.4 N NaOH solution completely neutralises 40 mL of a dibasic acid, the molarity of the acid solution is :

0.63 g of diabasic acid was dissolved in water. The volume of the solution was made 100 mL . 20 mL of this acid solution required 10 mL of N//5 NaOH solution. The molecular mass of acid is:

0.9698 g of an acid are present in 300 mL of a solution. 10 mL of this solution requires exactly 20 mL of 0.05 N KOH solution. If the mol.wt. of acid is 98 , calculate the number of neutralizable protons.

100 mL of 0.3 N -Acetic acid solution is mixed with same volume of 0.2 N sodium hydroxide solution. Ionisation constant of acetic acid is 2 xx 10^(-5) the pH of the mixture is