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Chapter 4: Problem 97

A solution of permanganate is standardized by titration with oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right) .\) It required 28.97 \(\mathrm{mL}\) of the permanganate solution to react completely with 0.1058 g of oxalic acid. The unbalanced equation for the reaction is $$\mathrm{MnO}_{4}^{-}(a q)+\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q) \stackrel{\mathrm{Acidic}}{\longrightarrow} \mathrm{Mn}^{2+}(a q)+\mathrm{CO}_{2}(g)$$ What is the molarity of the permanganate solution?

Short Answer

Expert verified
The molarity of the permanganate solution is \(0.00811\:M\).

Step by step solution

01

Balance the equation

First, we must balance the given chemical equation: \[ \mathrm{MnO}_{4}^{-}(aq) + 8 \mathrm{H}^{+}(aq) + 5 \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(aq) \rightarrow 2 \mathrm{Mn}^{2+}(aq) + 10 \mathrm{CO}_{2}(g) + 18 \mathrm{H}_{2}\mathrm{O}(l) \]
02

Convert the mass of oxalic acid into moles

Next, we will convert the given mass of oxalic acid (0.1058 g) into moles, using its molar mass (90.03 g/mol): \[ moles\:of\:oxalic\:acid = \frac{0.1058\:g}{90.03\:g/mol} = 1.175 \times 10^{-3}\:moles \]
03

Determine the moles of permanganate ions reacted

Now, we will use stoichiometry to determine the moles of permanganate ions reacted with oxalic acid. From the balanced equation, we can see that 5 moles of oxalic acid react with 1 mole of permanganate ions: \[ moles\:of\:permanganate\:ions = \frac{1.175 \times 10^{-3}\:moles\:oxalic\hdash acid}{5\:moles\:oxalic\hdash acid} \times 1\: mole\:permanganate\hdash ion = 2.350 \times 10^{-4}\:moles\:permanganate\:ions \]
04

Calculate the molarity of the permanganate solution

Finally, we will find the molarity of the permanganate solution by dividing the moles of permanganate ions by the volume of the solution used in the titration, which is given as 28.97 mL. Make sure to convert the volume to liters: \[ molarity\:of\:permanganate\:solution = \frac{2.350 \times 10^{-4}\:moles}{28.97 \times 10^{-3}\:L} = 0.00811\:M\] The molarity of the permanganate solution is 0.00811 M.

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Most popular questions from this chapter

Balance the following oxidation–reduction reactions that occur in basic solution. a. $\mathrm{Al}(s)+\mathrm{MnO}_{4}^{-}(a q) \rightarrow \mathrm{MnO}_{2}(s)+\mathrm{Al}(\mathrm{OH})_{4}-(a q)$ b. \(\mathrm{Cl}_{2}(g) \rightarrow \mathrm{Cl}^{-}(a q)+\mathrm{OCl}^{-}(a q)\) c. $\mathrm{NO}_{2}^{-}(a q)+\mathrm{Al}(s) \rightarrow \mathrm{NH}_{3}(g)+\mathrm{AlO}_{2}^{-}(a q)$

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