A standard solution of potassium permanganate (KMnO4) has a concentration of 0.0240 M. It is titrated against a solution of iron (II) sulfate (FeSO4). The equation for the reaction is 5Fe^{2+}(aq) + MnO_{4}^-(aq) + 8H^{+}(aq) → 5Fe^{3+}(aq) + Mn^{2+}(aq) + 4H_{2}O(l) 15.60 mL of the KMnO4 solution reacts exactly with 20.00 mL of the FeSO4 solution. The concentration of the FeSO4 solution, in M, is A. 0.0187 B. 0.0307 C. 0.0936 D. 0.1540

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A standard solution of potassium permanganate (KMnO4) has a concentration of 0.0240 M - VCE - SSCE Chemistry - Question 9 - 2004 - Paper 1

Question 9

A standard solution of potassium permanganate (KMnO4) has a concentration of 0.0240 M. It is titrated against a solution of iron (II) sulfate (FeSO4). The equation ... show full transcript

Worked Solution & Example Answer:A standard solution of potassium permanganate (KMnO4) has a concentration of 0.0240 M - VCE - SSCE Chemistry - Question 9 - 2004 - Paper 1

Step 1

Calculate the moles of KMnO4 used

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Answer

To determine the moles of KMnO4 used, we can use the formula:

$n = C imes V$

Where:

$C$ is the concentration of KMnO4 = 0.0240 M
$V$ is the volume of KMnO4 = 15.60 mL = 0.01560 L

Calculating the moles:

$n_{KMnO4} = 0.0240 ext{ M} imes 0.01560 ext{ L} = 0.0003744 ext{ moles}$

Step 2

Determine the moles of Fe^{2+} from the reaction

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Answer

From the balanced equation, 1 mole of MnO4^- reacts with 5 moles of Fe^{2+}. Therefore, the moles of Fe^{2+} are:

$n_{Fe^{2+}} = 5 imes n_{KMnO4} = 5 imes 0.0003744 = 0.001872 ext{ moles}$

Step 3

Calculate the concentration of FeSO4

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Answer

The concentration ( $C$ ) of FeSO4 can be calculated using the number of moles and the volume of the FeSO4 solution:

$C = rac{n}{V}$

Where:

$n_{Fe^{2+}} = 0.001872$ moles
$V_{FeSO4} = 20.00$ mL = 0.02000 L

Calculating:

$C_{FeSO4} = rac{0.001872}{0.02000} = 0.0936 ext{ M}$

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