The density of a concentrated Sulphuric acid () solution that is marked as by mass must be: — Mole Concept and Some Basic Concepts of Chemistry Chemistry Question

💡 Solution & Explanation

Step 1: Utilize the standard derivation connecting Molarity, mass percentage, and density: $\text{Molarity } (M) = \frac{(\text{Mass } \% \times \text{Density } \times 10)}{\text{Molar Mass of Solute}}$. Step 2: Isolate density ($d$) and substitute the parameters ($M_w$ of $H_2SO_4 = 98\text{ g/mol}$). $3.60 = \frac{29 \times d \times 10}{98}$ $d = \frac{3.60 \times 98}{290} = \frac{352.8}{290} = 1.2165\text{ g/mL}$. Rounding appropriately yields $1.22\text{ g/mL}$.