Textbook Question
Uric acid, the principal constituent of some kidney stones, has the formula C5H4N4O3. In aqueous solution, the solubility of uric acid is only 0.067 g/L. Express this concentration in (m/v)%, in parts per million, and in molarity.
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 86
Emergency treatment of cardiac arrest victims sometimes involves injection of a calcium chloride solution directly into the heart muscle. How many grams of CaCl2 are administered in an injection of 5.0 mL of a 5.0% (m/v) solution? How many milliequivalents of Ca2+?
Verified step by step guidance1
Determine the mass of CaCl₂ in the solution using the percent concentration formula: \( \text{mass of solute} = \text{percent concentration} \times \text{volume of solution} \). Here, the percent concentration is 5.0% (m/v), which means 5.0 g of CaCl₂ per 100 mL of solution. Use the given volume of 5.0 mL to calculate the mass of CaCl₂.
Convert the mass of CaCl₂ obtained in step 1 into moles using the molar mass of CaCl₂. The molar mass of CaCl₂ can be calculated as \( \text{molar mass of CaCl₂} = \text{atomic mass of Ca} + 2 \times \text{atomic mass of Cl} \).
Determine the moles of Ca²⁺ ions produced. Since each formula unit of CaCl₂ dissociates into one Ca²⁺ ion and two Cl⁻ ions, the moles of Ca²⁺ ions will be equal to the moles of CaCl₂.
Convert the moles of Ca²⁺ ions into milliequivalents (mEq). The milliequivalents are calculated using the formula \( \text{mEq} = \text{moles of ion} \times \text{valence} \times 1000 \). For Ca²⁺, the valence is 2.
Summarize the results: the mass of CaCl₂ administered and the milliequivalents of Ca²⁺ ions delivered. Ensure the units are consistent and clearly stated.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Mass/Volume Percentage (m/v)
Mass/volume percentage (m/v) is a concentration measurement that expresses the mass of solute in grams per 100 mL of solution. In this case, a 5.0% (m/v) solution means there are 5 grams of calcium chloride (CaCl₂) in every 100 mL of the solution. This concept is essential for calculating the total mass of solute in a given volume of solution.
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Mass Percent Concept
Calculating Grams from Volume
To find the grams of solute in a specific volume of a solution, you can use the formula: grams = (percentage/100) × volume (mL). For a 5.0% (m/v) solution, if you have 5.0 mL, you would calculate the grams of CaCl₂ by multiplying 5.0% by 5.0 mL, allowing you to determine the exact amount of solute administered in the injection.
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Milliequivalents of Calcium Ions (Ca²⁺)
Milliequivalents (mEq) measure the amount of a substance based on its chemical activity or reactivity, particularly in relation to ions. For calcium ions (Ca²⁺), 1 mole of Ca²⁺ is equivalent to 2 equivalents due to its +2 charge. To convert grams of CaCl₂ to milliequivalents of Ca²⁺, you need to calculate the number of moles of CaCl₂ and then multiply by 2, reflecting the number of Ca²⁺ ions produced.
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Related Practice
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Textbook Question
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