Home
Class 11
CHEMISTRY
The concentration of an oxalic acid solu...

The concentration of an oxalic acid solution is x mol litre^-1. `40mL` of this solution reacts with `16mL` of `0.05M` acidified `KMnO_4`. What is the `pH` of 'x' M oxalic acid solution ? (Assume that oxalic acid dissociates completely).)

Text Solution

AI Generated Solution

Promotional Banner

Similar Questions

Explore conceptually related problems

The concentration of an oxalic acid solution is x mol litre^(-1) . 40mL of this solution reacts with 16 mL of 0.05 M acidified KMnO_(4) . What is the pH x M oxalic acid solution ? (Assume that oxalic acid dissociates completely.)

25 mL of N/10 NaOH solution exactly neutralise 20 mL of an acid solution. What is the normality of the acid solution ?

20 ml of 0.02 M KMnO_4 was required to completely oxidise 10 ml of oxalic acid solution. What is the molarity of the oxalic acid solution ?

500 ml of a solution contain 12.6 grams of oxalic acid [Mol. Mass = 126 g/mole]. 10 ml of this solution is diluted to 100 ml in a flask. What is the molarity of the resultant solution?

The dissociation constant of an acid, HA is 1 x 10^-5 The pH of 0.1 M solution of the acid will be

If 11g of oxalic acid are dissolved in 500 mL of solution (density= 1.1 g mL ^ (−1) ), what is the mass % of oxalic acid in solution?

40mL sample of 0.1M solution of nitric acid is added to 20mL of 0.3M aqueous ammonia. What is the pH of the resulting solution? (pK_b = 4.7447)

Density of a 2.05 M solution of acetic acid in water is 1.02 g/mL. The molality of the solution is:

When KMnO_(4) is reduced with oxalic acid in acidic solution, the oxidation number of Mn changes from

The amount of oxalic acid required to prepare 300 mL of 2.5 M solution is : (molar mass of oxalic acid = 90 g mol^(–1) ) :