A acidic aqueous mixture contains exactly and . This entire mixture is titrated against a standard s — Mole Concept and Some Basic Concepts of Chemistry Chemistry Question
Question
A $100\text{ mL}$ acidic aqueous mixture contains exactly $0.1\text{ N } HCl$ and $0.2\text{ N } H_2SO_4$. This entire mixture is titrated against a standard $0.1\text{ M } NaOH$ solution. Which of the following analytical statements accurately reflect this process?
💡 Solution & Explanation
Step 1: Calculate total acid milliequivalents. Meq of $HCl = 100\text{ mL} \times 0.1\text{ N} = 10\text{ meq}$. Meq of $H_2SO_4 = 100\text{ mL} \times 0.2\text{ N} = 20\text{ meq}$. Total acid meq = $10 + 20 = 30\text{ meq}$ (Option A is true). Step 2: Evaluate the base. For $NaOH$, the n-factor is 1, so Molarity = Normality = $0.1\text{ N}$ (Option C is true). Step 3: Apply the Law of Equivalence. Meq of Base = Meq of Acid. $0.1 \times V_{\text{base}} = 30 \Rightarrow V_{\text{base}} = 300\text{ mL}$ (Option B is true). Option D is false because $150\text{ mL}$ of $0.1\text{ N } NaOH$ provides only $15\text{ meq}$, leaving the solution acidic.