Multiple Choice
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. What is the molarity of Cl⁻ ions in this solution?
6. Chemical Quantities & Aqueous Reactions
Molarity
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An aqueous solution of fructose (MM = 180.2 g/mol) has a molality of 4.87 m and a density of 1.30 g/mL. What is the molarity of fructose in the solution?
A
5.20 M
B
3.75 M
C
6.33 M
D
4.87 M
Verified step by step guidance1
Understand the relationship between molality and molarity. Molality (m) is defined as moles of solute per kilogram of solvent, while molarity (M) is moles of solute per liter of solution.
Calculate the mass of the solvent using the molality formula: \( m = \frac{\text{moles of solute}}{\text{mass of solvent in kg}} \). Rearrange to find the mass of the solvent: \( \text{mass of solvent} = \frac{\text{moles of solute}}{m} \).
Determine the moles of fructose using its molar mass. Given the molality and the mass of the solvent, calculate the moles of fructose: \( \text{moles of fructose} = \text{molality} \times \text{mass of solvent in kg} \).
Calculate the total mass of the solution using the density. Use the formula: \( \text{mass of solution} = \text{density} \times \text{volume of solution} \). Rearrange to find the volume of the solution: \( \text{volume of solution} = \frac{\text{mass of solution}}{\text{density}} \).
Finally, calculate the molarity using the formula: \( M = \frac{\text{moles of solute}}{\text{volume of solution in liters}} \). Convert the volume from mL to L if necessary.
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