Textbook Question
Obtain a bottle of aspirin and identify the amount of active ingredient (acetylsalicylic acid, C9H8O4) per tablet.
a. How many moles of aspirin are in one tablet?
3
views
Ch.6 Chemical Reactions: Mole and Mass Relationships
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187
Not the one you use?Change textbookSelect a different textbook
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 6, Problem 70b
Calcium citrate, Ca(C6H5O7)2(MW = 498.5 amu), is a common dietary supplement to provide calcium needed for strong teeth and bones.
b. What mass of calcium citrate would be needed to provide the recommended daily intake of calcium?
Verified step by step guidance1
Determine the molar mass of calcium citrate, which is given as 498.5 amu. This represents the mass of one mole of calcium citrate.
Identify the number of calcium atoms in one formula unit of calcium citrate. The formula Ca(C6H5O7)2 indicates there is 1 calcium atom per formula unit.
Calculate the molar mass of calcium (Ca) using the periodic table. The atomic mass of calcium is approximately 40.08 g/mol.
Determine the mass fraction of calcium in calcium citrate by dividing the molar mass of calcium by the molar mass of calcium citrate: \( \text{Mass fraction of calcium} = \frac{40.08}{498.5} \).
To find the mass of calcium citrate needed to provide the recommended daily intake of calcium, divide the recommended daily intake of calcium (in grams) by the mass fraction of calcium calculated in the previous step: \( \text{Mass of calcium citrate} = \frac{\text{Recommended daily intake of calcium}}{\text{Mass fraction of calcium}} \).
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
3mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Mass Calculation
Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). For calcium citrate, the molar mass is calculated by summing the atomic masses of all atoms in its formula, Ca(C6H5O7)2. This value is essential for converting between grams of the compound and moles, which is necessary for determining how much calcium citrate is needed to meet dietary requirements.
Recommended video:
Guided course
01:10
Calculating Molar Mass
Calcium Daily Intake
The recommended daily intake of calcium varies by age and gender, but for most adults, it is around 1000 mg (1 g) per day. Understanding this requirement is crucial for calculating how much calcium citrate must be consumed to meet this intake, as the amount of elemental calcium in calcium citrate must be determined to ensure adequate supplementation.
Recommended video:
Guided course
01:38The Scientific Method Concept 2
Elemental Calcium Content
Calcium citrate contains a specific percentage of elemental calcium, which is the actual calcium available for absorption in the body. To find out how much calcium citrate is needed to meet the daily intake, one must first determine the amount of elemental calcium in a given mass of calcium citrate. This involves using the molar mass of calcium and the molar mass of calcium citrate to calculate the proportion of calcium in the compound.
Recommended video:
Guided course
01:14Valence Electrons of Elements (Simplified) Example 1
Related Practice
Textbook Question
Pyrite, also known as fool's gold, is used commercially to produce SO2 used in the production of paper products.
b. How many moles of SO2 can be produced from 1.0 kg of pyrite?
2
views
Textbook Question
Elemental phosphorus exists as molecules of P4. It reacts with Cl2(g) to produce phosphorus pentachloride.
a. Write the balanced chemical equation for this reaction.
3
views
Textbook Question
Calcium citrate, Ca(C6H5O7)2(MW = 498.5 amu), is a common dietary supplement to provide calcium needed for strong teeth and bones.
a. Look up the recommended daily dietary intake of calcium for adult men and premenopausal women.
1
views
Textbook Question
Lovastatin, a drug used to lower serum cholesterol.
a. Look up the molecular formula for Lovastatin and calculate the molar mass.
1
views
Textbook Question
Acetylsalicylic acid, the active ingredient in aspirin, is prepared from salicylic acid by reaction with acetic anhydride.
C7H6O3 (salicylic acid) + C4H6O3 (acetic anhydride) → C9H8O4 (acetylsalicylic acid) + C2H4O2 (acetic acid)
a. Calculate the theoretical yield if 47 g of salicylic acid is reacted with 25 g of acetic anhydride.
1
views