Textbook Question
The concentration of cholesterol (C27H46O) in blood is approximately 5.0 mM. How many grams of cholesterol are in 250 mL of blood?
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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 19
The typical concentration of Mg2+ in blood is 3 mEq/L. How many milligrams of Mg2+ are in 250 mL of blood?
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Step 1: Understand the given information. The concentration of Mg²⁺ is provided as 3 mEq/L (milliequivalents per liter), and the volume of blood is 250 mL. The goal is to determine the mass of Mg²⁺ in milligrams.
Step 2: Convert the volume of blood from milliliters to liters, since the concentration is given in mEq/L. Use the conversion factor: 1 L = 1000 mL. The formula is: \( \text{Volume in liters} = \frac{\text{Volume in mL}}{1000} \).
Step 3: Calculate the total milliequivalents of Mg²⁺ in the given volume of blood. Use the formula: \( \text{Total mEq} = \text{Concentration (mEq/L)} \times \text{Volume (L)} \).
Step 4: Convert milliequivalents (mEq) to millimoles (mmol). For Mg²⁺, 1 mEq corresponds to 0.5 mmol because the charge of Mg²⁺ is +2. Use the formula: \( \text{mmol} = \text{mEq} \times 0.5 \).
Step 5: Convert millimoles to milligrams. The molar mass of Mg²⁺ is approximately 24.31 g/mol. Use the formula: \( \text{Mass in mg} = \text{mmol} \times \text{Molar mass (mg/mmol)} \), where \( \text{Molar mass (mg/mmol)} = 24.31 \).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Milliequivalents (mEq)
Milliequivalents (mEq) is a unit of measurement used to express the concentration of ions in a solution. It accounts for the charge of the ion, allowing for a standardized way to compare different ions. For magnesium (Mg²⁺), 1 mEq corresponds to 1 millimole of the ion, considering its valence of +2. Understanding mEq is crucial for converting between different units of concentration.
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Concentration Calculation
Concentration calculation involves determining the amount of a substance in a given volume of solution. In this case, the concentration of Mg²⁺ is given as 3 mEq/L, which means there are 3 milliequivalents of magnesium in one liter of blood. To find the total amount in 250 mL, one must convert the volume from liters to milliliters and apply the concentration to find the total mEq present.
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Conversion from mEq to mg
To convert milliequivalents (mEq) of an ion to milligrams (mg), one must use the molecular weight of the ion. For magnesium, the atomic weight is approximately 24.3 g/mol. The conversion formula is: mg = mEq × (molecular weight / valence). This step is essential for translating the concentration of Mg²⁺ in mEq to its mass in mg, which is necessary for the final answer.
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Related Practice
Textbook Question
The Environmental Protection Agency has set the limit for arsenic in drinking water at 0.010 ppm. To what volume would you need to dilute 1.5 L of water containing 5.0 ppm arsenic to reach the acceptable limit?
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Textbook Question
The diagram to the right shows plots of vapor pressure versus temperature for a solvent and a solution.
b. What is the approximate boiling-point elevation for the solution?
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Textbook Question
The diagram to the right shows plots of vapor pressure versus temperature for a solvent and a solution.
c. What is the approximate concentration of the solution in mol/kg, if 1 mol of solute particles raises the boiling point of 1 kg of solvent by 3.63 °C?
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Textbook Question
The maximum amounts of lead and copper allowed in drinking water are 0.015 mg/kg for lead and 1.3 mg/kg for copper. Express these values in parts per million, and tell the maximum amount of each (in grams) allowed in 100 g of water.
Textbook Question
When 1.0 mol of HF is dissolved in 1.0 kg of water, the boiling point of the resulting solution is 100.5 °C. Is HF a strong or weak electrolyte? Explain.
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