Multiple Choice
Why is it necessary to dilute a bacterial culture when plating for a counting experiment?
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6. Chemical Quantities & Aqueous Reactions
Dilutions
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A laboratory has concentrated HNO3 solution with a molarity of 6.00 M. How many milliliters of this concentrated solution are required to prepare 1.15 L of 0.115 M HNO3 by dilution with water?
A
69.0 mL
B
22.1 mL
C
132 mL
D
0.115 mL
Verified step by step guidance1
Identify the known quantities: the concentration of the concentrated HNO3 solution (M₁ = 6.00 M), the desired concentration after dilution (M₂ = 0.115 M), and the final volume of the diluted solution (V₂ = 1.15 L).
Recall the dilution equation, which relates the concentrations and volumes before and after dilution: \(M_1 \times V_1 = M_2 \times V_2\), where \(V_1\) is the volume of the concentrated solution needed.
Rearrange the dilution equation to solve for \(V_1\): \(V_1 = \frac{M_2 \times V_2}{M_1}\).
Substitute the known values into the equation: \(V_1 = \frac{0.115\,\text{M} \times 1.15\,\text{L}}{6.00\,\text{M}}\).
Calculate \(V_1\) in liters, then convert this volume to milliliters by multiplying by 1000, since 1 L = 1000 mL.
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