Textbook Question
Research information related to dialysis and answer the following questions:
a. What is the difference between hemodialysis and peritoneal dialysis?
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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 100b
Many carbonate minerals are insoluble in water and appear in water pipes as 'scale.'
b. Why is scale formation typically only a problem in hot water pipes?
Verified step by step guidance1
Understand the solubility of carbonate minerals: Carbonate minerals, such as calcium carbonate (CaCO₃), are generally sparingly soluble in water. Their solubility is influenced by temperature and the concentration of ions in the water.
Recall the effect of temperature on solubility: For many solids, solubility increases with temperature. However, for carbonate minerals like CaCO₃, solubility decreases as temperature increases. This is because the dissolution of CaCO₃ is an exothermic process, and higher temperatures shift the equilibrium toward the solid form (precipitation).
Consider the role of hot water pipes: In hot water pipes, the water temperature is elevated, which reduces the solubility of carbonate minerals. As a result, dissolved carbonate ions (CO₃²⁻) and calcium ions (Ca²⁺) in the water are more likely to combine and precipitate as solid CaCO₃, forming scale.
Account for the concentration of ions: Hard water, which contains high concentrations of calcium (Ca²⁺) and bicarbonate (HCO₃⁻) ions, is more prone to scale formation. When heated, bicarbonate ions decompose into carbonate ions (CO₃²⁻), further promoting the precipitation of CaCO₃.
Conclude why scale forms in hot water pipes: The combination of reduced solubility of carbonate minerals at higher temperatures and the increased availability of carbonate ions in hot water leads to the precipitation of scale, making it a common issue in hot water pipes.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Solubility of Carbonate Minerals
Carbonate minerals, such as calcium carbonate, have varying solubility in water depending on temperature and pressure. Generally, these minerals are more soluble in cold water than in hot water. As water temperature increases, the solubility of these minerals decreases, leading to precipitation and the formation of scale in hot water pipes.
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Temperature Effects on Scale Formation
In hot water systems, the elevated temperatures promote the precipitation of dissolved minerals as they exceed their solubility limits. This process is exacerbated in hot water pipes, where the constant heat encourages the formation of scale, which can accumulate and restrict water flow, leading to maintenance issues.
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Water Chemistry and pH Levels
The chemistry of water, including its pH level, significantly influences the solubility of carbonate minerals. Higher temperatures can alter the pH, making the water more alkaline, which further reduces the solubility of calcium carbonate. This change in water chemistry is a key factor in the increased likelihood of scale formation in hot water pipes.
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Related Practice
Textbook Question
Look up the composition of Ringer's solution used in the treatment of burns and wounds.
b. What is the osmolarity of the solution? Is it hypertonic, isotonic, or hypotonic with blood plasma (0.30 osmol)? Discuss possible medicinal reasons for the osmolarity of the solution.
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Textbook Question
Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the solubility of O2, N2, CO, and CO2 in water at standard temperature and pressure (1 atm, 25 °C).
b. Explain how elevated pressures in a hyperbaric chamber be used to treat decompression sickness (excess N2 in blood) and carbon monoxide poisoning.
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Textbook Question
To prevent accumulation of ice on roads and sidewalks, many municipalities (and home-owners) will apply de-icing compounds to 'melt' the ice by lowering the freezing point.
b. Some de-icing compositions include dyes or colored compounds called indicators. Why?
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