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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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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Permanganate Solution
Permanganate solution typically refers to an aqueous solution containing permanganate ions extcolor{[MnO}_4-Jo

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Most popular questions from this chapter

A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess \(\mathrm{H}^{+}\) or \(\mathrm{OH}^{-}\) ions left in solution.

A stream flows at a rate of \(5.00 \times 10^{4}\) liters per second (L/s) upstream of a manufacturing plant. The plant discharges \(3.50 \times 10^{3} \mathrm{L} / \mathrm{s}\) of water that contains 65.0 \(\mathrm{ppm} \mathrm{HCl}\) into the stream. (See Exercise 135 for definitions.) a. Calculate the stream's total flow rate downstream from this plant. b. Calculate the concentration of \(\mathrm{HCl}\) in ppm downstream from this plant. c. Further downstream, another manufacturing plant diverts \(1.80 \times 10^{4} \mathrm{L} / \mathrm{s}\) of water from the stream for its own use. This plant must first neutralize the acid and does so by adding lime: $$\mathrm{CaO}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(i) $$ What mass of CaO is consumed in an 8.00-h work day by this plant? d. The original stream water contained 10.2 \(\mathrm{ppm} \mathrm{Ca}^{2+}\) . Although no calcium was in the waste water from the first plant, the waste water of the second plant contains \(\mathrm{Ca}^{2+}\) from the neutralization process. If 90.0% of the water used by the second plant is returned to the stream, calculate the concentration of \(\mathrm{Ca}^{2+}\) in ppm downstream of the second plant.

Assign the oxidation state for nitrogen in each of the following. a \(\mathrm{L}_{3} \mathrm{N} \quad\) d. NO \(\quad\) g. \(\mathrm{NO}_{2}^{-}\) b. \(\mathrm{NH}_{3} \quad\) e. \(\mathrm{N}_{2} \mathrm{O} \quad\) h. \(\mathrm{NO}_{3}^{-}\) c\(\mathrm{N}_{2} \mathrm{H}_{4} \quad\) f. \(\mathrm{NO}_{2} \quad\) i. \(\mathrm{N}_{2}\)

You are given a solid that is a mixture of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) A 0.205-g sample of the mixture is dissolved in water. An excess of an aqueous solution of \(\mathrm{BaCl}_{2}\) is added. The BaSO\(_{4}\) that is formed is filtered, dried, and weighed. Its mass is 0.298 g. What mass of \(\mathrm{SO}_{4}^{2-}\) ion is in the sample? What is the mass percent of \(\mathrm{SO}_{4}^{2-}\) ion in the sample? What are the percent compositions by mass of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the sample?

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