Multiple Choice
Assuming that its density is 1.000 g/mL, what is the mass percent concentration of a 0.1432 M AgNO₃ solution?
6. Chemical Quantities & Aqueous Reactions
Molarity
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Calculate the molarity of calcium chloride (CaCl2) if 31.9 g of solid calcium chloride is dissolved in enough water to make 692 mL of solution. (Molar mass of CaCl2 = 110.98 g/mol)
A
0.420 M
B
0.520 M
C
0.610 M
D
0.290 M
Verified step by step guidance1
First, calculate the number of moles of calcium chloride (CaCl2) using the formula: \( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \). Substitute the given values: mass = 31.9 g and molar mass = 110.98 g/mol.
Next, convert the volume of the solution from milliliters to liters, since molarity is expressed in moles per liter. Use the conversion: \( 1 \text{ L} = 1000 \text{ mL} \). Therefore, \( 692 \text{ mL} = 0.692 \text{ L} \).
Now, calculate the molarity of the solution using the formula: \( \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{volume of solution in liters}} \).
Substitute the number of moles of CaCl2 calculated in step 1 and the volume in liters from step 2 into the molarity formula.
Finally, compare the calculated molarity with the given options to determine the correct answer.
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