100 , mL of a sample containing calcium oxala | vedclass

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(A) The balanced redox reaction in acidic medium is: $5C_2O_4^{2-} + 2MnO_4^- + 16H^+ \rightarrow 10CO_2 + 2Mn^{2+} + 8H_2O$. Number of millimoles of

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$2$

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(A) The balanced redox reaction in acidic medium is: $5C_2O_4^{2-} + 2MnO_4^- + 16H^+ ightarrow 10CO_2 + 2Mn^{2+} + 8H_2O$. Number of millimoles of $KMnO_4 = 	ext{Molarity} 	imes 	ext{Volume (in mL)} = 1 \, M 	imes 20 \, mL = 20 \, mmol$. From the stoichiometry,$2 \, mol$ of $MnO_4^-$ reacts with $5 \, mol$ of $C_2O_4^{2-}$. Therefore,$mmol$ of $C_2O_4^{2-} = \frac{5}{2} 	imes 20 = 50 \, mmol$. Since $1 \, mol$ of $CaC_2O_4$ contains $1 \, mol$ of $Ca^{2+}$,$mmol$ of $Ca^{2+} = 50 \, mmol$. Mass of $Ca^{2+} = \frac{50}{1000} 	imes 40 \, g = 2 \, g$.

$100 \, mL$ of a sample containing calcium oxalate $[CaC_2O_4]$ is dissolved in an acidic solution. It required $20 \, mL$ of $1 \, M \, KMnO_4$ for complete oxidation. Find the mass of $Ca^{2+}$ ions (in grams) present in the sample. [Atomic mass of $Ca = 40$]

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