he mass of solute (glucose) and the mass of solvent (water). alve Mass % of glucose omment The mass percentage of water in this solution is (100 11.9) % = 88.1%. b) Analyze In this case we are given the number of micrograms of solute. Because 1 µg is 1 x 10g, 5.4 µg = 5.4 x 10 g. Plan We calculate the parts per million using Equation 13.6. 5.4 X 106g 2.5 g Solve ppm = mass glucose mass soln mass of solute mass of soln ge by using Equation 13.5. The mass of the solutie age of sol X 106 - X 100 = 13.5 g 13.5 g + 100 g 0/ X 106 = 2.2 ppm Practice Exercise 1 Calculate the mass percentage of NaCl in a solution containing 1.50 g of NaCl in 50.0 g of water. (a) 0.0291%, (b) 0.0300%, (c) 0.0513%, (d) 2.91%, (e) 3.00%. X 100 = 11.9% Practice Exercise 2 A commercial bleaching solution contains 3.62% by mass of sodium hypochlorite, NaOCI. What is the mass of NaOCl in a bottle containing 2.50 kg of bleaching solution? Mole Fraction, Molarity, and Molality Concentration expressions are often based on the number of moles of one or more components of the solution. Recall from Section 10.6 that the mole fraction of a compo- nent of a solution is given by MacBook Pro & #
he mass of solute (glucose) and the mass of solvent (water). alve Mass % of glucose omment The mass percentage of water in this solution is (100 11.9) % = 88.1%. b) Analyze In this case we are given the number of micrograms of solute. Because 1 µg is 1 x 10g, 5.4 µg = 5.4 x 10 g. Plan We calculate the parts per million using Equation 13.6. 5.4 X 106g 2.5 g Solve ppm = mass glucose mass soln mass of solute mass of soln ge by using Equation 13.5. The mass of the solutie age of sol X 106 - X 100 = 13.5 g 13.5 g + 100 g 0/ X 106 = 2.2 ppm Practice Exercise 1 Calculate the mass percentage of NaCl in a solution containing 1.50 g of NaCl in 50.0 g of water. (a) 0.0291%, (b) 0.0300%, (c) 0.0513%, (d) 2.91%, (e) 3.00%. X 100 = 11.9% Practice Exercise 2 A commercial bleaching solution contains 3.62% by mass of sodium hypochlorite, NaOCI. What is the mass of NaOCl in a bottle containing 2.50 kg of bleaching solution? Mole Fraction, Molarity, and Molality Concentration expressions are often based on the number of moles of one or more components of the solution. Recall from Section 10.6 that the mole fraction of a compo- nent of a solution is given by MacBook Pro & #
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Mass Percentage Calculation
#### Example
Calculate the mass percentage of glucose using Equation 13.5. The mass of the solute (glucose) and the mass of the solvent (water) are given.
**Formula:**
\[ \text{Mass \% of glucose} = \frac{\text{mass glucose}}{\text{mass solution}} \times 100 \]
Using the given data:
\[ \text{Mass \% of glucose} = \frac{13.5 \, \text{g}}{13.5 \, \text{g} + 100 \, \text{g}} \times 100 = 11.9\% \]
#### Comment
The mass percentage of water in this solution is calculated as:
\[ 100\% - 11.9\% = 88.1\% \]
#### Example Calculation
**b) Analyze:**
Given the number of micrograms of solute. Because \(1 \, \mu\text{g} = 1 \times 10^{-6} \, \text{g}\):
\[ 5.4 \, \mu\text{g} = 5.4 \times 10^{-6} \, \text{g} \]
**Plan:**
Calculate the parts per million (ppm) using Equation 13.6.
**Solve:**
\[ \text{ppm} = \frac{\text{mass of solute}}{\text{mass of solution}} \times 10^6 = \frac{5.4 \, \times 10^{-6} \, \text{g}}{2.5 \, \text{g}} \times 10^6 = 2.2 \, \text{ppm} \]
---
#### Practice Exercise 1
Calculate the mass percentage of NaCl in a solution containing 1.50 g of NaCl in 50.0 g of water.
(a) 0.0291%
(b) 0.0300%
(c) 0.0513%
(d) 2.91%
(e) 3.00%
#### Practice Exercise 2
A commercial bleaching solution contains 3.62% by mass of sodium hypochlorite, NaOCl.
What is the mass of NaOCl in a bottle containing 2.50 kg of bleaching solution?
---
### Mole Fraction, Molar](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F97d95e45-995f-411a-a6fb-c34e70a82379%2Fb5918bf0-9c3e-4fba-80bf-dc36ece40f3c%2Fjkjpaum_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Mass Percentage Calculation
#### Example
Calculate the mass percentage of glucose using Equation 13.5. The mass of the solute (glucose) and the mass of the solvent (water) are given.
**Formula:**
\[ \text{Mass \% of glucose} = \frac{\text{mass glucose}}{\text{mass solution}} \times 100 \]
Using the given data:
\[ \text{Mass \% of glucose} = \frac{13.5 \, \text{g}}{13.5 \, \text{g} + 100 \, \text{g}} \times 100 = 11.9\% \]
#### Comment
The mass percentage of water in this solution is calculated as:
\[ 100\% - 11.9\% = 88.1\% \]
#### Example Calculation
**b) Analyze:**
Given the number of micrograms of solute. Because \(1 \, \mu\text{g} = 1 \times 10^{-6} \, \text{g}\):
\[ 5.4 \, \mu\text{g} = 5.4 \times 10^{-6} \, \text{g} \]
**Plan:**
Calculate the parts per million (ppm) using Equation 13.6.
**Solve:**
\[ \text{ppm} = \frac{\text{mass of solute}}{\text{mass of solution}} \times 10^6 = \frac{5.4 \, \times 10^{-6} \, \text{g}}{2.5 \, \text{g}} \times 10^6 = 2.2 \, \text{ppm} \]
---
#### Practice Exercise 1
Calculate the mass percentage of NaCl in a solution containing 1.50 g of NaCl in 50.0 g of water.
(a) 0.0291%
(b) 0.0300%
(c) 0.0513%
(d) 2.91%
(e) 3.00%
#### Practice Exercise 2
A commercial bleaching solution contains 3.62% by mass of sodium hypochlorite, NaOCl.
What is the mass of NaOCl in a bottle containing 2.50 kg of bleaching solution?
---
### Mole Fraction, Molar
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