Textbook Question
Calculate the molarity of the following aqueous solutions: (a) 0.540 g of Mg(NO3)2 in 250.0 mL of solution, (b) 22.4 g of LiClO4 • 3 H2O in 125 mL of solution,
Ch.13 - Properties of Solutions
Chapter 13, Problem 44c
What is the molarity of each of the following solutions: (c) 35.0 mL of 9.00 M H2SO4 diluted to 0.500 L?
Verified step by step guidance1
Understand the concept of molarity, which is defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (M).
Recognize that when a solution is diluted, the number of moles of solute remains constant, but the volume of the solution changes. Use the formula for dilution: M1 * V1 = M2 * V2, where M1 and V1 are the initial molarity and volume, and M2 and V2 are the final molarity and volume.
Identify the given values: the initial molarity (M1) is 9.00 M, the initial volume (V1) is 35.0 mL, and the final volume (V2) is 0.500 L. Convert the initial volume from milliliters to liters by dividing by 1000, so V1 = 0.035 L.
Substitute the known values into the dilution equation: (9.00 M) * (0.035 L) = M2 * (0.500 L).
Solve for the final molarity (M2) by rearranging the equation: M2 = (9.00 M * 0.035 L) / 0.500 L.
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