20 mL of 0.02 M K2Cr2O7 solution is used for the titration of 10 mL of Fe2+ solution in the acidic medium. The molarity of Fe2+ solution is ______×10–2 M. (Nearest integer)
Correct Answer: 24
Approach Solution - 1
The titration equation for the reaction between dichromate ions (Cr2O72–) and iron ions (Fe2+) in an acidic medium is:
Cr2O72– + 6Fe2+ + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O
The stoichiometry indicates that 1 mole of Cr2O72– oxidizes 6 moles of Fe2+.
Calculate moles of K2Cr2O7:
moles = Molarity × Volume (L) = 0.02 M × 0.020 L = 0.0004 mol
Since 1 mole of Cr2O72– reacts with 6 moles of Fe2+, moles of Fe2+ are:
6 × 0.0004 mol = 0.0024 mol
The molarity of Fe2+ solution is calculated using its volume:
Molarity = (moles/Volume in L) = 0.0024 mol / 0.010 L = 0.24 M
Express it as: 24 × 10–2 M.
The solution value is 24, which lies within the expected range (24,24). Thus, the molarity of the Fe2+ solution is 24×10–2 M.
Approach Solution -2
Applying the law of equivalence,
milliequivalents of Fe2+ = milliequivalents of K2Cr2O7
10 × 1 × M = 20 × 6 × .02
M = 24 × 10–2 M
∴ Answer will be 24.
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Ordinary Differential Equations is an equation that indicates the relation of having one independent variable x, and one dependent variable y, along with some of its other derivatives.
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