Questions: What is the molarity of an aqueous solution that contains 0.0720 g C2H3O2 per gram of solution? The density of the solution is 1.04 g / mL
Transcript text: What is the molarity of an aqueous solution that contains 0.0720
$\mathrm{g} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$ per gram of solution ? The density of the solution is $1.04 \mathrm{~g} / \mathrm{mL}$
Solution
Solution Steps
Step 1: Calculate the mass of the solution in grams per liter
Given the density of the solution is \(1.04 \, \text{g/mL}\), we can convert this to grams per liter:
Step 2: Calculate the mass of solute in grams per liter
The solution contains \(0.0720 \, \text{g}\) of \(\mathrm{C}_2\mathrm{H}_3\mathrm{O}_2\) per gram of solution. Therefore, the mass of the solute per liter of solution is:
Molarity (M) is defined as the number of moles of solute per liter of solution. We can calculate the number of moles of \(\mathrm{C}_2\mathrm{H}_3\mathrm{O}_2\) in one liter of solution: