What is the parts per million (ppm) concentration of a solution made with 0.0500 g of NaCl in 100 g of water (i.e. 150 g of total solution)? a. 333 ppm b. 500 ppm C. 550 ppm d. 50 ppm

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**Question:** What is the parts per million (ppm) concentration of a solution made with 0.0500 g of NaCl in 100 g of water (i.e., 150 g of total solution)?

a. 333 ppm  
b. 500 ppm  
c. 550 ppm (The correct answer is marked)  
d. 50 ppm  

**Explanation:** 

To calculate the parts per million (ppm) concentration, use the formula:
\[ \text{ppm} = \left(\frac{\text{mass of solute (g)}}{\text{mass of solution (g)}}\right) \times 10^6 \]

**Steps:**
1. **Mass of solute (NaCl):** 0.0500 g
2. **Mass of solution:** 150 g (100 g of water + 50 g, assumed as a typo - should be 0.0500 g solute assumed).

Plug in the values:
\[ \text{ppm} = \left(\frac{0.0500}{150}\right) \times 10^6 \approx 333 \]

Therefore, choice 'a' seems to be the calculated correct option, but 'c' is marked in the text. Either there is an oversight in the options provided, or additional context is affecting the choice.
Transcribed Image Text:**Question:** What is the parts per million (ppm) concentration of a solution made with 0.0500 g of NaCl in 100 g of water (i.e., 150 g of total solution)? a. 333 ppm b. 500 ppm c. 550 ppm (The correct answer is marked) d. 50 ppm **Explanation:** To calculate the parts per million (ppm) concentration, use the formula: \[ \text{ppm} = \left(\frac{\text{mass of solute (g)}}{\text{mass of solution (g)}}\right) \times 10^6 \] **Steps:** 1. **Mass of solute (NaCl):** 0.0500 g 2. **Mass of solution:** 150 g (100 g of water + 50 g, assumed as a typo - should be 0.0500 g solute assumed). Plug in the values: \[ \text{ppm} = \left(\frac{0.0500}{150}\right) \times 10^6 \approx 333 \] Therefore, choice 'a' seems to be the calculated correct option, but 'c' is marked in the text. Either there is an oversight in the options provided, or additional context is affecting the choice.
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