Multiple Choice
900 mL of water is added to 100 mL of a 0.1 M solution. What is the new concentration of the solution?
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6. Chemical Quantities & Aqueous Reactions
Dilutions
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
How many milliliters of 6.00 M H_2SO_4 are required to prepare 2.00 L of 0.300 M sulfuric acid solution?
A
100 mL
B
300 mL
C
200 mL
D
400 mL
Verified step by step guidance1
Identify the known values: the concentration of the stock solution \(C_1 = 6.00\, M\), the volume of the diluted solution \(V_2 = 2.00\, L\), and the concentration of the diluted solution \(C_2 = 0.300\, M\).
Recall the dilution equation which relates the concentrations and volumes before and after dilution: \(C_1 \times V_1 = C_2 \times V_2\), where \(V_1\) is the volume of the stock solution needed.
Rearrange the dilution equation to solve for \(V_1\): \(V_1 = \frac{C_2 \times V_2}{C_1}\).
Substitute the known values into the equation: \(V_1 = \frac{0.300\, M \times 2.00\, L}{6.00\, M}\).
Calculate \(V_1\) to find the volume in liters, then convert this volume to milliliters by multiplying by 1000 (since 1 L = 1000 mL).
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