A stock solution of substance A has a concentration of 8.42% by mass. You make three solutions from this stock using the amounts shown in the table. Calculate the total volume and the molarity for each solution. (Assume a density of 1.00 g/mL for the stock solution and a molecular weight of 68.6 g/mol for A). mL of stock A added to mL of water Total volume [A] (molarity) 70 mL A 0 mL of water 15 mL A 50 mL of water 10 mL A 65 mL of water
A stock solution of substance A has a concentration of 8.42% by mass. You make three solutions from this stock using the amounts shown in the table. Calculate the total volume and the molarity for each solution. (Assume a density of 1.00 g/mL for the stock solution and a molecular weight of 68.6 g/mol for A). mL of stock A added to mL of water Total volume [A] (molarity) 70 mL A 0 mL of water 15 mL A 50 mL of water 10 mL A 65 mL of water
Chemistry
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ISBN:9781305957404
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![### Preparation of Solutions from a Stock Solution of Substance A
#### Introduction:
A stock solution of substance A has a concentration of 8.42% by mass. You are required to prepare three different solutions using this stock solution and water, as outlined in the table below. Calculate the total volume and the molarity for each solution. Assume a density of 1.00 g/mL for the stock solution and a molecular weight of 68.6 g/mol for substance A.
#### Table of Prepared Solutions:
| mL of stock A added to mL of water | Total volume | [A] (molarity) |
|-------------------------------------|--------------|----------------|
| 70 mL A | 0 mL of water| |
| 15 mL A | 50 mL of water| |
| 10 mL A | 65 mL of water| |
#### Explanation:
1. **70 mL A with 0 mL of water:**
- **Total Volume:** Since no water is added, the total volume is 70 mL.
- **Calculation of Molarity:**
- From the density of 1.00 g/mL, the mass of the stock solution is \( 70 \text{ mL} \times 1.00 \text{ g/mL} = 70 \text{ g} \).
- The mass of substance A in 70 g of the stock solution: \( 70 \text{ g} \times 0.0842 = 5.894 \text{ g} \).
- Moles of A: \( \frac{5.894 \text{ g}}{68.6 \text{ g/mol}} = 0.086 \text{ moles} \).
- Molarity \( (M) \) = \( \frac{0.086 \text{ moles}}{0.070 \text{ L}} = 1.23 \text{ M} \).
2. **15 mL A with 50 mL of water:**
- **Total Volume:** \( 15 \text{ mL} + 50 \text{ mL} = 65 \text{ mL} \).
- **Calculation of Molarity:**
- Mass of 15 mL of the stock solution: \( 15 \text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd1cf2ec1-831d-43ac-84b4-19fe406513bb%2F3e8d949d-7f1d-4812-89b2-25dad6288aef%2Fywxbc5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Preparation of Solutions from a Stock Solution of Substance A
#### Introduction:
A stock solution of substance A has a concentration of 8.42% by mass. You are required to prepare three different solutions using this stock solution and water, as outlined in the table below. Calculate the total volume and the molarity for each solution. Assume a density of 1.00 g/mL for the stock solution and a molecular weight of 68.6 g/mol for substance A.
#### Table of Prepared Solutions:
| mL of stock A added to mL of water | Total volume | [A] (molarity) |
|-------------------------------------|--------------|----------------|
| 70 mL A | 0 mL of water| |
| 15 mL A | 50 mL of water| |
| 10 mL A | 65 mL of water| |
#### Explanation:
1. **70 mL A with 0 mL of water:**
- **Total Volume:** Since no water is added, the total volume is 70 mL.
- **Calculation of Molarity:**
- From the density of 1.00 g/mL, the mass of the stock solution is \( 70 \text{ mL} \times 1.00 \text{ g/mL} = 70 \text{ g} \).
- The mass of substance A in 70 g of the stock solution: \( 70 \text{ g} \times 0.0842 = 5.894 \text{ g} \).
- Moles of A: \( \frac{5.894 \text{ g}}{68.6 \text{ g/mol}} = 0.086 \text{ moles} \).
- Molarity \( (M) \) = \( \frac{0.086 \text{ moles}}{0.070 \text{ L}} = 1.23 \text{ M} \).
2. **15 mL A with 50 mL of water:**
- **Total Volume:** \( 15 \text{ mL} + 50 \text{ mL} = 65 \text{ mL} \).
- **Calculation of Molarity:**
- Mass of 15 mL of the stock solution: \( 15 \text
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