Question

A solution of permanganate is standardized by titration with oxalic acid, . To react completely with mol of oxalic acid required 37.02 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is

Answer 1

`M=0.120M`

Step-by-step explanation:

Hello,

In this case, the undergone chemical reaction is:

`MnO_4^-(aq)+H_2C_2O_4(aq)\rightarrow Mn^(+2)+CO_2`

In such a way, the acidic redox balance turns out:

`(Mn^(+7)O_4)^-+5e^-+8H^+\rightarrow Mn^(+2)+4H_2O\\H_2C_2O_4\rightarrow2CO_2+2H^++2e^-`

Which leads to the total balanced equation as follows:

`2(MnO_4)^-(aq)+6H^+(aq)+5H_2C_2O_4(aq)\rightarrow2Mn^(+2)(aq)+8H_2O(l)+10CO_2(g)`

Thus, as the mass of oxalic acid is not given, one could suppose a value of 1 g (which you can modify based on the actual statement) in order to compute the oxalic acid moles as shwon below:

`1gH_2C_2O_4*(1molH_2C_2O_4)/(90.04gH_2C_2O_4) *(2mol(MnO_4)^-)/(5molH_2C_2O_4) =0.00444mol(MnO_4)^-`

Whereby the molality results:

`M=(0.00444mol(MnO_4)^-)/(0.03702L) =0.120M`

Remember you can modify the oxalic acid mass as you desire.

Best regards.