Textbook Question
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
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 45
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?
Verified step by step guidance1
Step 1: Understand the concept of % (m/v). The percentage mass/volume (% m/v) is defined as the mass of solute (in grams) per 100 mL of solution. For a 0.50% (m/v) solution, this means 0.50 g of boric acid is dissolved in 100 mL of solution.
Step 2: Determine the total mass of boric acid needed for 500.0 mL of solution. Since the solution is 0.50% (m/v), scale up the mass proportionally: (0.50 g / 100 mL) × 500.0 mL.
Step 3: Weigh the calculated mass of boric acid using a balance. Ensure the balance is properly calibrated for accurate measurement.
Step 4: Dissolve the measured boric acid in a volume of distilled water that is less than 500.0 mL. Stir the solution until the boric acid is completely dissolved.
Step 5: Transfer the solution to a 500.0 mL volumetric flask and add distilled water until the total volume reaches exactly 500.0 mL. Mix thoroughly to ensure a uniform solution.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Concentration (m/v)
Mass/volume (m/v) concentration expresses the mass of solute per 100 mL of solution. A 0.50% (m/v) solution means there are 0.50 grams of solute (boric acid) in every 100 mL of solution. This concept is crucial for understanding how to prepare solutions with specific concentrations.
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Dilution
Dilution is the process of reducing the concentration of a solute in a solution, typically by adding more solvent. In this case, to prepare a 0.50% (m/v) solution from a more concentrated stock solution, one must calculate the appropriate volume of stock solution and the amount of water needed to achieve the desired concentration.
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Measurement and Units
Accurate measurement is essential in preparing solutions. Understanding units such as grams for mass and milliliters for volume is necessary to ensure the correct proportions are used. This knowledge helps in converting between different units and ensuring the final solution meets the specified concentration.
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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
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)
Textbook Question
The solubility of NH3 gas in water at an NH3 pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.
b. How many moles of NH3 would be released from 1.0 L of a saturated NH3 solution if the temperature was increased from 25 to 50 °C?