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Questions and Answers
Acids are substances that donate ______ in a solution.
Acids are substances that donate ______ in a solution.
protons
According to the Arrhenius theory, bases produce ______ ions in aqueous solutions.
According to the Arrhenius theory, bases produce ______ ions in aqueous solutions.
hydroxide
A Lewis acid is an electron pair ______.
A Lewis acid is an electron pair ______.
acceptor
Neutralization reactions produce a ______ and water when an acid reacts with a base.
Neutralization reactions produce a ______ and water when an acid reacts with a base.
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Strong acids completely ______ in water, releasing all available H+ ions.
Strong acids completely ______ in water, releasing all available H+ ions.
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Indicators change color depending on the ______ of the solution.
Indicators change color depending on the ______ of the solution.
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In a titration, a known concentration of a solution is called the ______.
In a titration, a known concentration of a solution is called the ______.
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Acid rain has a pH lower than ______.
Acid rain has a pH lower than ______.
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Buffers are important for maintaining a stable ______ in biological systems.
Buffers are important for maintaining a stable ______ in biological systems.
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The equivalence point in a titration is when the moles of acid equal the moles of ______.
The equivalence point in a titration is when the moles of acid equal the moles of ______.
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Study Notes
Definitions and Properties
- Acids are substances that donate protons (H+) in a solution. They have a sour taste and can react with certain metals to produce hydrogen gas. Common examples include hydrochloric acid (HCl) and sulfuric acid (H₂SO₄).
- Bases are substances that accept protons (H+) in a solution. They have a bitter taste and a soapy feel. Common examples include sodium hydroxide (NaOH) and ammonia (NH₃).
- pH is a measure of the concentration of hydrogen ions (H+) in a solution. A lower pH indicates a higher concentration of H+ ions, making the solution acidic. Conversely, a higher pH indicates a lower concentration of H+ ions, making the solution basic. pH ranges from 0 to 14, with 7 being neutral.
- Conjugate acid-base pairs are related by the gain or loss of a single proton. For example, HCl and Cl- are a conjugate acid-base pair.
Arrhenius Theory
- The Arrhenius theory defines acids and bases in terms of their ability to produce hydrogen ions (H+) and hydroxide ions (OH-) in aqueous solutions, respectively.
- Acids increase the concentration of H+ ions in water.
- Bases increase the concentration of OH- ions in water.
Brønsted-Lowry Theory
- The Brønsted-Lowry theory defines acids and bases in terms of proton donors and acceptors.
- An acid is a proton donor.
- A base is a proton acceptor.
- This theory is more general than the Arrhenius theory, as it applies to reactions in any solvent, not just water.
Lewis Theory
- The Lewis theory defines acids and bases in terms of electron pair donors and acceptors.
- A Lewis acid is an electron pair acceptor.
- A Lewis base is an electron pair donor.
- This theory is the most general, extending the definition to a wider range of species than the previous two theories.
Acid-Base Reactions
- Neutralization reactions are a type of double displacement reaction that happen between an acid and a base. The general reaction between an acid and a base produces a salt and water.
- Neutralization reactions are often used to determine the concentration of an unknown acid or base using titration techniques.
Strengths of Acids and Bases
- Strong acids completely ionize in water, releasing all available H+ ions.
- Weak acids only partially ionize in water, releasing a smaller quantity of H+ ions.
- Strong bases completely ionize in water, releasing all available OH- ions.
- Weak bases only partially ionize in water, releasing a smaller quantity of OH- ions.
Indicators
- Indicators are substances that change color depending on the pH of the solution. They are often used in titrations to determine the endpoint of the reaction. Common indicators include litmus paper (red in acidic solutions, blue in basic solutions), phenolphthalein (colorless in acid, pink in base), and bromothymol blue (yellow in acidic, blue in basic).
Acid-Base Titrations
- Titration is a technique used to determine the concentration of an unknown acid or base.
- A known volume and concentration of a solution (the titrant) are added to a solution of unknown concentration (the analyte) until the reaction is complete.
- The equivalence point of a titration is the point where the moles of acid equal the moles of base. This is often a crucial aspect observed in acid-base reactions.
- Indicators are used to visually signal the equivalence point, by observing the color change.
Acid Rain
- Acid rain is rain with a pH lower than 5.6, caused by the atmospheric reaction of sulfur dioxide and nitrogen oxides with water, oxygen, and other chemicals. This pollution can damage aquatic ecosystems, forests and infrastructure.
Buffers
- Buffers are solutions that resist changes in pH when small amounts of acid or base are added. They are composed of a weak acid and its conjugate base, or a weak base and its conjugate acid.
- Buffers are important in maintaining a stable pH in biological systems and industrial processes.
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Description
Test your understanding of acids and bases with this quiz focused on key definitions and properties. Learn about the pH scale, conjugate acid-base pairs, and the Arrhenius theory. This quiz will help reinforce your chemistry knowledge in these fundamental concepts.
