/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 97 A solution of permanganate is st... [FREE SOLUTION] | 91影视

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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

Balance the following oxidation鈥搑eduction reactions that occur in acidic solution using the half-reaction method. a. \(\mathrm{Cu}(s)+\mathrm{NO}_{3}^{-}(a q) \rightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{NO}(g)\) b. \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{Cl}^{-}(a q) \rightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{Cl}_{2}(g)\) c. \(\mathrm{Pb}(s)+\mathrm{PbO}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{PbSO}_{4}(s)\) d. \(\mathrm{Mn}^{2+}(a q)+\mathrm{NaBiO}_{3}(s) \rightarrow \mathrm{Bi}^{3+}(a q)+\mathrm{MnO}_{4}-(a q)\) e. \(\mathrm{H}_{3} \mathrm{AsO}_{4}(a q)+\mathrm{Zn}(s) \rightarrow \mathrm{AsH}_{3}(g)+\mathrm{Zn}^{2+}(a q)\)

What mass of barium sulfate can be produced when 100.0 mL of a 0.100-M solution of barium chloride is mixed with 100.0 mL of a 0.100-M solution of iron(III) sulfate?

A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution after precipitation is complete.

Citric acid, which can be obtained from lemon juice, has the molecular formula \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\) . A 0.250 -g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?

The iron content of iron ore can be determined by titration with a standard \(\mathrm{KMnO}_{4}\) solution. The iron ore is dissolved in \(\mathrm{HCl},\) and all the iron is reduced to \(\mathrm{Fe}^{2+}\) ions. This solution is then titrated with \(\mathrm{KMnO}_{4}\), solution, producing \(\mathrm{Fe}^{3+}\) and \(\mathrm{Mn}^{2+}\) ions in acidic solution. If it required 38.37 \(\mathrm{mL}\) of 0.0198 \(\mathrm{M}\) \(\mathrm{KMnO}_{4}\) to titrate a solution made from 0.6128 \(\mathrm{g}\) of iron ore, what is the mass percent of iron in the iron ore?
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