of a metal was dissolved in of . The excess acid required of for neutralization. The equivalent weig — Mole Concept and Some Basic Concepts of Chemistry Chemistry Question
Question
$1.6 \text{ g}$ of a metal was dissolved in $100 \text{ mL}$ of $1\text{N } H_2SO_4$. The excess acid required $20 \text{ mL}$ of $1\text{N } NaOH$ for neutralization. The equivalent weight of the metal is:
Answer: A
💡 Solution & Explanation
Total $\text{mEq acid} = 100 \times 1 = 100$. <br>$\text{mEq excess acid} = 20 \times 1 = 20$. <br>$\text{mEq used by metal} = 100 - 20 = 80$. <br>$\text{Equivalent weight} = \frac{\text{Mass in grams}}{\text{mEq} / 1000} = \frac{1.6}{0.08} = 20$.
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