Textbook Question
Nalorphine, a relative of morphine, is used to combat withdrawal symptoms in heroin users. How many milliliters of a 0.40% (m/v) solution of nalorphine must be injected to obtain a dose of 1.5 mg?
Ch.9 Solutions
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187
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Table of contents
- Ch.1 Matter and Measurements27
- Ch.2 Atoms and the Periodic Table20
- Ch.3 Ionic Compounds8
- Ch.4 Molecular Compounds23
- Ch.5 Classification & Balancing of Chemical Reactions12
- Ch.6 Chemical Reactions: Mole and Mass Relationships28
- Ch.7 Chemical Reactions: Energy, Rate and Equilibrium64
- Ch.8 Gases, Liquids and Solids24
- Ch.9 Solutions52
- Ch.10 Acids and Bases25
- Ch.11 Nuclear Chemistry22
- Ch.12 Introduction to Organic Chemistry: Alkanes57
- Ch.13 Alkenes, Alkynes, and Aromatic Compounds47
- Ch.14 Some Compounds with Oxygen, Sulfur, or a Halogen50
- Ch.15 Aldehydes and Ketones45
- Ch.16 Amines42
- Ch.17 Carboxylic Acids and Their Derivatives57
- Ch.18 Amino Acids and Proteins82
- Ch.19 Enzymes and Vitamins63
- Ch.20 Carbohydrates44
- Ch.21 The Generation of Biochemical Energy65
- Ch.22 Carbohydrate Metabolism45
- Ch.23 Lipids42
- Ch.24 Lipid Metabolism33
- Ch.25 Protein and Amino Acid Metabolism24
- Ch.26 Nucleic Acids and Protein Synthesis45
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187Not the one you use?Change textbook
Chapter 9, Problem 48
What is the mass/volume percent concentration of the following solutions?
a. 0.078 mol KCl in 75 mL of solution
b. 0.044 mol sucrose (C12H22O11) in 380 mL of solution
Verified step by step guidance1
Step 1: Recall the formula for mass/volume percent concentration: \( \text{Mass/Volume Percent} = \frac{\text{Mass of solute (g)}}{\text{Volume of solution (mL)}} \times 100 \).
Step 2: For part (a), calculate the mass of KCl. Use the molar mass of KCl (\( 39.10 \ \text{g/mol} \) for K and \( 35.45 \ \text{g/mol} \) for Cl) to find the mass of 0.078 mol of KCl: \( \text{Mass of KCl} = \text{Moles of KCl} \times \text{Molar Mass of KCl} \).
Step 3: Substitute the calculated mass of KCl and the given volume of solution (75 mL) into the mass/volume percent formula: \( \text{Mass/Volume Percent} = \frac{\text{Mass of KCl (g)}}{75 \ \text{mL}} \times 100 \).
Step 4: For part (b), calculate the mass of sucrose (C₁₂H₂₂O₁₁). Use the molar mass of sucrose (\( 12 \times 12.01 \ \text{g/mol} + 22 \times 1.008 \ \text{g/mol} + 11 \times 16.00 \ \text{g/mol} \)) to find the mass of 0.044 mol of sucrose: \( \text{Mass of sucrose} = \text{Moles of sucrose} \times \text{Molar Mass of sucrose} \).
Step 5: Substitute the calculated mass of sucrose and the given volume of solution (380 mL) into the mass/volume percent formula: \( \text{Mass/Volume Percent} = \frac{\text{Mass of sucrose (g)}}{380 \ \text{mL}} \times 100 \).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Mass/Volume Percent Concentration
Mass/volume percent concentration is a way to express the concentration of a solution, defined as the mass of solute (in grams) per 100 mL of solution. It is calculated using the formula: (mass of solute in grams / volume of solution in mL) × 100. This measurement is particularly useful in chemistry for understanding how concentrated a solution is.
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Percent Concentrations Concept 1
Molarity and Moles
Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. To find the mass of a solute from its moles, one can use the molar mass, which is the mass of one mole of that substance. Understanding how to convert between moles and grams is essential for calculating mass/volume percent concentration.
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Dilution and Solution Preparation
Dilution refers to the process of reducing the concentration of a solute in a solution, typically by adding more solvent. When preparing solutions, it is important to know the final volume and the amount of solute needed to achieve the desired concentration. This concept is crucial for accurately calculating mass/volume percent concentrations in various scenarios.
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Related Practice
Textbook Question
How is volume/volume percent concentration defined and for what types of solutions is it typically used?
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Textbook Question
If you had only 23 g of KOH remaining in a bottle, how many milliliters of 10.0% (m/v) solution could you prepare? How many milliliters of 0.25 M solution?
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Textbook Question
The solubility of CO2 gas in water is 0.15 g/100 mL at a CO2 pressure of 760 mmHg.
b. An atmospheric concentration of 380 ppm, CO2 corresponds to a partial pressure of 0.00038 atm. What percentage of the CO2 originally dissolved in the solution in part (a) remains in solution after the soft drink reaches equilibrium with the ambient atmosphere?
Textbook Question
A dilute aqueous solution of boric acid, H3BO3 is often used as an eyewash. How would you prepare 500.0 mL of a 0.50% (m/v) boric acid solution?
Textbook Question
How many moles of each substance are needed to prepare the following solutions?
a. 50.0 mL of 8.0% (m/v) KCl (MW = 74.55 g/mol)
b. 200.0 mL of 7.5% (m/v) acetic acid (MW = 60.05 g/mol)