If x g is the mass of `NaHC_(2)O_(4)` required to neutralize 100 ml of 0.2 M NaOH and y g that required to reduce 100 ml of 0.02 M `KMnO_(4)` in acidic medium then

The weight of oxalic acid required to reduce 80 ml of 0.4 M KMnO_(4) in acidic medium is

Moles of KHC_(2)O_(4) (potassium acid oxalate) required to reduce 100 mL of 0.02M KMnO_(4) in acidic medium (to Mn^(2+) ) is

The weight of KMnO_4 that can oxidise 100 ml of. 0.2M oxalic acid in acidic medium is

Number of moles of KMnO_(4) required to oxidize one mole of Fe(C_(2)O_(4)) in acidic medium is

The volume of 0.1 M NaOH will be required to neutralise 100 ml of 0.1 ml H_(3)PO_(4) using methyl red indicator to change the colour from pink (acidic medium) to yellow (basic medium) is 10^(x) . What is x?

X gm of KHC_(2)O_(4) requires 100 ml of 0.02 M KMnO_(4) in acidic medium. In another experiment, y gm of KHC_(2)O_(4) requires 100 mkl of 0.05 M Ca(OH)_(2) . The ratio of x and y is

From the given reaction 2KMnO_(4) + 3H_(2)SO_(4) + 5H_(2)O_(2) rarr K_(2)SO_(4) + 2MnSO_(4) + 8H_(2)O + 5O_(2) Find the normality of H_(2)O_(2) solution, if 20 mL of it is required to react completely with 16 mL of 0.02M KMnO_(4) solution (Molar mass of KMnO_(4) = 158 g mol^(-1) )

What is the approximate volume (in mL) of 10 vol H_(2)O_(2) solution that will react completely with 1 L of 0.02 M KMnO_(4) solution in acidic medium?