10 ml of `NaHC_2O_4` solution is neutralized by 10 ml of 0.1 M NaOH solution. 10 ml of same `NaHC_2O_4` solution is oxidised by 10 ml of `KMnO_4` solution in acidic medium. Calculate the molarity of `KMnO_4` solution.

10ml 0.05 N H_2SO_4 solution is mixed with 10 ml 0.1 N NaOH solution. The pH of the final mixture is

Density of 3 molal NaOH solution is 1.110 g*mL^(-1) . Calculate the molarity of the solution.

The pH of solution obtained by mixing 10 ml of 10^-1 N HCl and 10 ml of 10^-1 N NaOH is

100 mL of 0.05 (M) NaOH solution is added to a 100 mL of 0.1 (M) NaH_2PO_4 solution. Will the mixed solution act as a buffer ?

100 mL of 30% (m/v) NaOH solution is mixed with 100 mL of 90% (m/v) NaOH solution then the molarity of final solution will be-

On adding 20 ml. of N/10 NaOH solution to 10 ml. of N/10 HCl, the resulting solution will

Ratio of moles of Fe (II) oxidised by equal volumes of equimolar KMnO_4 and K_2Cr_2O_7 solutions in acidic medium will be :

The molarity of a solution obtained by mixing 750 ml of 0.5 M HCl with 250 ml of 2M HCl will be

V ml solution of Fe^(2+) can be oxidised by 60 ml of KMnO_4 in acidic medium. What will be the volume of K_2Cr_2O_7 required to oxidise V ml of the same Fe^(2+) solution in an acidic medium ? Consider the molarity of KMnO_4 and K_2Cr_2O_7 to be the same.