Question

g A solution of permanganate is standardized by titration with oxalic acid, . To react completely with mol of oxalic acid required 22.69 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is

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 22.69 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is:

$MnO_4^-(aq)+H_2C_2O_4(aq)\stackrel{\mathrm{Acidic}}{\longrightarrow} Mn^{2+}(aq)+CO_2(g)$

Determine the concentration of the permanganate solution in molarity.

Answer: The molarity of permanganate solution is 0.0317 M

Explanation:

The balanced chemical equation follows:

$2MnO_4^-(aq)+6H^+(aq)+5H_2C_2O_4(aq)\stackrel{\mathrm{Acidic}}{\longrightarrow} 2Mn^{2+}(aq)+8H_2O(l)+10CO_2(g)$

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 = $\frac{2}{5}\times 0.0018=0.00072mol$ of permanganate solution

The formula used to calculate molarity:

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

Given values:

Moles of permanganate solution = 0.00072 moles

Volume of solution = 22.69 mL

Putting values in equation 1, we get:

$\text{Molarity of permanganate solution}=\frac{0.00072\times 1000}{22.69}\\\\\text{Molarity of permanganate solution}=0.0317M$

Hence, the molarity of permanganate solution is 0.0317 M

Answer 2

The concentration of the permanganate solution in molarity is 0.0317 M

We'll begin by calculating the number of mole of permanganate needed to react with 0.0018 mole of oxalic acid.

2MnO₄¯(aq) + 5H₂C₂O₄(aq) + 6H⁺(aq) —> 2Mn²⁺(s) + 10CO₂(g) + 8H₂O(l)

From the balanced equation above,

5 moles of H₂C₂O₄ reacted with 2 moles of MnO₄¯

Therefore,

0.0018 mole of H₂C₂O₄ will react with = (0.0018 × 2) / 5 = 0.00072 mole of MnO₄¯

• Finally, we shall determine the molarity of the permanganate solution.

Mole of MnO₄¯ = 0.00072 mole

Volume = 22.69 mL = 22.69 / 0.02269 L

Molarity of MnO₄¯ =

Molarity = mole / Volume

Molarity of MnO₄¯ = 0.00072 / 0.02269

Molarity of MnO₄¯ = 0.0317 M

Therefore, the molarity of the permanganate solution is 0.0317 M

Complete question:

A solution of permanganate is standardized by titration with oxalic acid. To react completely with 0.0018 mol of oxalic acid required 22.69 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is:

MnO₄¯(aq) + H₂C₂O₄(aq) —> Mn²⁺(s) + CO₂(g)

Determine the concentration of the permanganate solution in molarity.

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