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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Assuming that its density is 1.000 g/mL, what is the mass percent concentration of a 0.1432 M AgNO₃ solution?
A
1.43%
B
14.32%
C
2.43%
D
0.14%
Verified step by step guidance1
Calculate the molar mass of AgNO₃ by adding the atomic masses of Ag, N, and O₃. Use the periodic table to find these values.
Determine the mass of AgNO₃ in one liter of solution using the molarity (0.1432 M). Multiply the molarity by the molar mass of AgNO₃ to find the mass in grams.
Since the density of the solution is 1.000 g/mL, the mass of 1 liter (1000 mL) of the solution is 1000 grams.
Calculate the mass percent concentration by dividing the mass of AgNO₃ by the total mass of the solution and then multiplying by 100 to convert it to a percentage.
Express the mass percent concentration as a percentage to compare with the given options.
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