Question

A solution of permanganate is standardized by titration with oxalic acid, . To react completely with mol of oxalic acid required 28.18 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is Determine the concentration of the permanganate solution in molarity. g

Answer 1

The question is incomplete, the complete question is:

A solution of permanganate is standardized by titration with oxalic acid. To react completely with 0.0018 mol of oxalic acid required 28.18 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is:

`\mathrm{MnO}_(4)^(-)(aq)+\mathrm{H}_(2)\mathrm{C}_(2)\mathrm{O}_(4)(aq)\stackrel{\mathrm{Acidic}}{\longrightarrow}\mathrm{Mn}^(2+)(aq)+\mathrm{CO}_(2)(\mathrm{g})`

Determine the concentration of the permanganate solution in molarity.

Answer: The molarity of permanganate solution is 0.026 M

Step-by-step explanation:

The balanced chemical equation follows:

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

Given values:

Moles of oxalic acid = 0.0018 moles

By the stoichiometry of the reaction:

If 5 moles of oxalic acid reacts with 2 moles of permanganate solution

So, 0.0018 moles of oxalic acid will react with =
`(2)/(5)* 0.0018mol=0.00072mol` of permanganate solution

Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:

`\text{Molarity of solution}=\frac{\text{Moles of solute}* 1000}{\text{Volume of solution (mL)}}` .....(1)

Given values:

Moles of permanganate solution = 0.00072 moles

Volume of solution = 28.18 mL

Putting values in equation 1, we get:

`\text{Molarity of permanganate solution}=(0.00072* 1000)/(28.18)\\\\\text{Molarity of permanganate solution}=0.026M`

Hence, the molarity of permanganate solution is 0.026 M