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

Answer:

$M=0.120M$

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:

$1gH_2C_2O_4*\frac{1molH_2C_2O_4}{90.04gH_2C_2O_4} *\frac{2mol(MnO_4)^-}{5molH_2C_2O_4} =0.00444mol(MnO_4)^-$

Whereby the molality results:

$M=\frac{0.00444mol(MnO_4)^-}{0.03702L} =0.120M$

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

Best regards.