Chemistry Chapter 2: Acids, Bases, and pH
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Questions and Answers

What is the pH level of a neutral solution?

  • 0
  • 14
  • 7 (correct)
  • 3

    • Which of the following statements about acids is true?

  • They decrease the concentration of free H+ in a solution.
  • They have a pH greater than 7.
  • They act as proton acceptors.
  • Stronger acids dissociate more H+ than weaker acids. (correct)

    • Which of these describes a basic solution?

  • pH greater than 7 (correct)
  • pH of 3
  • Greater concentration of H+ than OH−
  • pH of 7

    • What role do buffers play in the body?

    <p>They prevent drastic pH changes when acids or bases are added. (B)</p> Signup and view all the answers

    What happens to the pH when H+ concentration increases?

    <p>The pH decreases. (D)</p> Signup and view all the answers

    How do stronger bases differ from weaker bases?

    <p>Stronger bases absorb more H+. (A)</p> Signup and view all the answers

    What is the function of the kidneys in relation to the carbonic acid-bicarbonate buffer system?

    <p>They regulate bicarbonate levels. (A)</p> Signup and view all the answers

    Which of the following conditions is indicated by a low blood pH?

    <p>Acidosis (C)</p> Signup and view all the answers

    Flashcards

    pH

    A measure of hydrogen ion concentration in a solution, ranging from 0 to 14.

    Acidic Solutions

    Solutions with a pH less than 7, having higher concentrations of H+ than OH−.

    Basic Solutions

    Solutions with a pH greater than 7, containing higher concentrations of OH− than H+.

    Neutral Solution

    A solution with a pH of 7, where H+ and OH− concentrations are equal.

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    Acid

    A substance that donates protons (H+) and increases their concentration in a solution.

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    Base

    A substance that accepts protons (H+) and decreases their concentration in a solution.

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    Neutralization

    The reaction process where an acidic and basic solution combine to return to a neutral state (pH 7).

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    Buffers

    Solutions that resist changes in pH by accepting or donating H+ as needed.

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    Study Notes

    Chapter 2: Atoms, Ions, and Molecules - Acids, Bases, and pH

    • Learning Objectives: Define pH, differentiate acidity and basicity, compare and contrast acids and bases, and describe how buffers maintain blood pH in the carbonic acid-bicarbonate buffer system.

    pH

    • pH is a measure of the relative amount of H+ in a solution.
    • The pH scale ranges from 0 to 14.
    • pH and H+ concentration are inversely related. As H+ concentration increases, pH decreases. Conversely, as H+ concentration decreases, pH increases.
    • A pH of 7 is neutral. pH values below 7 are acidic, and above 7 are basic.
    • Each step on the pH scale represents a tenfold difference in H+ concentration.

    pH and Solutions

    • Neutral solutions have equal concentrations of H+ and OH-.
    • Acidic solutions have a greater concentration of H+ than OH-.
    • Basic solutions have a greater concentration of OH- than H+.

    Acids

    • Acids are proton donors, increasing the concentration of free H+.
    • Stronger acids have a greater dissociation of H+ than weaker acids.
    • Examples include hydrochloric acid (stomach acid) and carbonic acid (in the blood).

    Bases

    • Bases are proton acceptors, decreasing the concentration of free H+.
    • Stronger bases absorb more H+ than weaker bases.
    • Examples include ammonia and bleach. Bicarbonate is a weak base that buffers blood pH.

    Neutralization

    • Neutralization occurs when an acidic or basic solution is returned to a neutral pH (7)
    • Acids are neutralized by adding a base.
    • Bases are neutralized by adding acid. Example: Medications to neutralize stomach acid often contain a base.

    Buffers

    • Buffers help prevent major pH changes.
    • The carbonic acid-bicarbonate buffer system is critical in maintaining blood pH within a narrow range.
    • Carbonic acid (weak acid) and bicarbonate (weak base) act together to resist changes in pH.
    • Blood pH is maintained at a critical range of 7.35-7.45.
    • Low blood pH is acidosis, while high blood pH is alkalosis.
    • Lungs regulate CO2, while kidneys regulate bicarbonate levels for proper pH balance.

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    Related Documents

    Chapter 2 Student Lab Notes - Acids, Bases, and pH PDF

    Description

    Explore the fundamental concepts of acids, bases, and pH in this quiz focused on Chapter 2 of the chemistry curriculum. Test your understanding of the pH scale, the properties of acids and bases, and the role of buffers in maintaining blood pH. Dive into the details of how these chemical processes affect solutions.

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