Open Question
An aqueous solution that contains 285 ppm of potassium nitrate (KNO₃) is being used to feed plants in a garden. What volume of this solution is needed to prepare 2.0 L of a solution that is 75 ppm in KNO₃?
9. Solutions
Dilutions
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To what final volume would 100 mL of 5.0 M KCl have to be diluted in order to make a solution that is 0.54 M KCl?
A
72 mL
B
289 mL
C
330 mL
D
930 mL
E
1400 mL
Verified step by step guidance1
Start by identifying the key components of the dilution problem: the initial concentration (C1 = 5.0 M), the initial volume (V1 = 100 mL), and the final concentration (C2 = 0.54 M). We need to find the final volume (V2).
Use the dilution equation, which is C1 * V1 = C2 * V2. This equation states that the product of the initial concentration and volume is equal to the product of the final concentration and volume.
Substitute the known values into the equation: (5.0 M) * (100 mL) = (0.54 M) * V2.
Rearrange the equation to solve for V2: V2 = (5.0 M * 100 mL) / (0.54 M).
Calculate the result to find the final volume V2. This will give you the volume to which the solution must be diluted to achieve the desired concentration.
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