Ch.3 - WaterSee all chapters
All Chapters
Ch.1 - Introduction to Biology
Ch.2 - Chemistry
Ch.3 - Water
Ch.4 - Carbon
Ch.5 - Biological Molecules
Ch.6 - Cells
Ch.7 - The Membrane
Ch.8 - Energy and Metabolism
Ch.9 - Respiration
Ch.10 - Photosynthesis
Ch.11 - Cell Signaling
Ch.12 - Cell Division
Ch.13 - Meiosis
Ch.14 - Mendelian Genetics
Ch.15 - Chromosomal Theory of Inheritance
Ch.16 - DNA Synthesis
Ch.17 - Gene Expression
Ch.18 - Regulation of Expression
Ch.19 - Viruses
Ch.20 - Biotechnology
Ch.21 - Genomics
Ch.22 - Development
Ch.23 - Evolution by Natural Selection
Ch.24 - Evolution of Populations
Ch.25 - Speciation
Ch.26 - History of Life on Earth
Ch.27 - Phylogeny
Ch.28 - Prokaryotes
Ch.29 - Protists
Ch.30 - Plants
Ch.31 - Fungi
Ch.32 - Overview of Animals
Ch.33 - Invertebrates
Ch.34 - Vertebrates
Ch.35 - Plant Anatomy
Ch.36 - Vascular Plant Transport
Ch.37 - Soil
Ch.38 - Plant Reproduction
Ch.39 - Plant Sensation and Response
Ch.40 - Animal Form and Function
Ch.41 - Digestive System
Ch.42 - Circulatory System
Ch.43 - Immune System
Ch.44 - Osmoregulation and Excretion
Ch.45 - Endocrine System
Ch.46 - Animal Reproduction
Ch.47 - Nervous System
Ch.48 - Sensory Systems
Ch.49 - Muscle Systems
Ch.50 - Ecology
Ch.51 - Animal Behavior
Ch.52 - Population Ecology
Ch.53 - Community Ecology
Ch.54 - Ecosystems
Ch.55 - Conservation Biology

Acids and Bases

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Sections
Properties of Water
Acids and Bases
Additional Practice
Calculating pH

Practice: Acids ________________________ H+ concentration, and have a pH of _________ to __________.

Practice: Why are buffers important for biological systems?

Additional Problems
Homeostasis means:  a.  That a population changes over time b.  That conditions are held constant and do not change c.  That cells have enough water d.  That all organisms require an energy source e.  That conditions remain within a constant range
An acid:  a. Has a value above seven on the pH scale b. Is a chemical that takes hydrogen ions from a solution c. Has a value of seven on the pH scale d. Is a chemical that adds hydrogen ions to a solution e. All are correct
A base:  a. Has a value of 7 on the pH scale b. Is a chemical that adds hydrogen ions to a solution c. Is a chemical that absorbs hydrogen ions from a solution d. Has a value below 7 on the pH scale
A substance having a pH of 2 would best be described as:  a. Neutral b. A weak acid c. A weak base d. A strong base e. A strong acid
A substance having a pH of 6 would best be described as:  a. A weak acid b. Neutral c. A weak base d. A strong acid e. A strong base
A substance having a pH of 7 would best be described as:  a. A weak acid b. A weak base c. Neutral d. A strong acid e. A strong base
A substance having a pH of 8 would best be described as:  a. Neutral b. A weak base c. A weak acid d. A strong acid e. A strong base
A substance having a pH of 13 would best be described as:  a. A weak acid b. A weak base c. Neutral d. A strong acid e. A strong base
What is the pH of 40.0mL of a solution that is 0.13 M CN- and 0.21 M in HCN? For HCN, use Ka = 4.9 x 10-9.
What are the concentrations of acetic acid (pKa = 4.76) and acetate in a buffer solution of 0.20M at pH 4.5? Enter your answer to two significant figures.
The molar ratio of HPO42- to H2PO4- in a solution is 1.4. What is the pH of the solution? Phosphoric acid (H3PO4) is a triprotic acid, with 3 pKa values: 2.14, 6.86, and 12.4.A. 2.3B. 12.5C. 7.0D. 6.2
In our discussion of the acid-base properties of individual amino acids, we indicated that most amino acids will be electrically neutral over a very broad range of pH values, so that the pI of an individual amino acid is a nearly meaningless quantity. By contrast, a full-length protein will be electrically neutral over a relatively narrow pH range — typically less than one pH unit. Thus the pI of a protein is a well-defined quantity. Why is this?
Formic acid has a pKa of 3.75; acetic acid has a pKa of 4.76. Which is the stronger acid? Does the stronger acid have a greater or lesser tendency to lose its proton than the weaker acid?