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 1.04g/mL, we can convert this to grams per liter:
1.04g/mL×1000mL/L=1040g/L
Step 2: Calculate the mass of solute in grams per liter
The solution contains 0.0720g of C2H3O2 per gram of solution. Therefore, the mass of the solute per liter of solution is:
0.0720g/g×1040g/L=74.88g/L
Step 3: Calculate the molar mass of C2H3O2
The molar mass of C2H3O2 is calculated as follows:
Molarity (M) is defined as the number of moles of solute per liter of solution. We can calculate the number of moles of C2H3O2 in one liter of solution: