Multiple Choice
The average human body contains about 5,000 grams of blood. What mass of arsenic is present in the body if the amount in blood is 0.86 ppb?
9. Solutions
Parts per Million (ppm)
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A 5.12 L sample of solution contains 0.230 g of potassium sulfate, K2SO4. Determine the concentration of K2SO4 in ppm if the density of the solution is 1.30 g/mL.
A
34.6 ppm
B
28.9 ppm
C
22.3 ppm
D
43.6 ppm
Verified step by step guidance1
First, calculate the mass of the solution using its volume and density. The volume is given as 5.12 L, which is equivalent to 5120 mL. Use the formula: \( \text{mass of solution} = \text{volume} \times \text{density} \).
Next, determine the mass of potassium sulfate (K2SO4) in the solution, which is already provided as 0.230 g.
To find the concentration in parts per million (ppm), use the formula: \( \text{ppm} = \left( \frac{\text{mass of solute}}{\text{mass of solution}} \right) \times 10^6 \).
Substitute the mass of K2SO4 and the mass of the solution into the ppm formula. Remember that ppm is a unit that expresses the ratio of the mass of the solute to the mass of the solution, multiplied by one million.
Finally, perform the calculation to determine the concentration of K2SO4 in ppm. Compare your result with the given options to identify the correct answer.
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