Acid-Base Reactions and Properties
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Questions and Answers

What is the primary purpose of a universal indicator?

  • To neutralize acids and bases
  • To indicate the presence of salts
  • To measure the pH of a solution (correct)
  • To create a color chart for base solutions
  • A universal indicator is made of a single type of indicator.

    False

    What is the method used to determine the pH of a solution with a universal indicator?

    A drop of the indicator is added to the solution and the color is matched with a color chart.

    The process of combining an acid with a base to form a salt and water is called __________.

    <p>neutralization</p> Signup and view all the answers

    Match the following terms with their correct descriptions:

    <p>Universal Indicator = A mixture used to measure pH pH = A scale to measure acidity or alkalinity Neutralization = Reaction between an acid and a base Color Chart = Guide for matching colors to pH values</p> Signup and view all the answers

    Which of the following indicators is most commonly extracted from lichens?

    <p>Litmus</p> Signup and view all the answers

    Synthetic indicators change color sharply when an acid is neutralized by an alkali.

    <p>True</p> Signup and view all the answers

    What is the pH value range for strong acids?

    <p>0-2</p> Signup and view all the answers

    The pH scale ranges from ______ to ______.

    <p>1, 14</p> Signup and view all the answers

    Match each pH range to its corresponding strength:

    <p>pH 0-2 = Strong acid pH 3-6 = Weak acid pH 8-11 = Weak alkali pH 12-14 = Strong alkali</p> Signup and view all the answers

    Which indicator is not suitable for titrations due to its gradual color change?

    <p>Litmus</p> Signup and view all the answers

    What relationship exists between the concentration of hydrogen ions and pH?

    <p>Inverse relationship</p> Signup and view all the answers

    PH 7 indicates a strong alkaline solution.

    <p>False</p> Signup and view all the answers

    What characterizes a strong acid?

    <p>It completely dissociates in water.</p> Signup and view all the answers

    Hydrochloric acid is an example of a weak acid.

    <p>False</p> Signup and view all the answers

    What is the chemical equation for the reaction between ethanoic acid and sodium hydroxide?

    <p>CH3COOH + NaOH → CH3COONa + H2O</p> Signup and view all the answers

    An acid is a proton (H+) __________.

    <p>donor</p> Signup and view all the answers

    Match the acids to their associated products when reacting with magnesium:

    <p>Hydrochloric acid = Magnesium chloride and hydrogen Sulfuric acid = Magnesium sulfate and hydrogen Nitric acid = Magnesium nitrate and hydrogen Ethanoic acid = Sodium ethanoate and water</p> Signup and view all the answers

    Which of the following statements is true about weak acids?

    <p>They produce pH values close to 7.</p> Signup and view all the answers

    The concentration of an acid determines whether it is strong or weak.

    <p>False</p> Signup and view all the answers

    What is a base in terms of proton transfer?

    <p>Proton acceptor</p> Signup and view all the answers

    A concentrated solution of an acid contains a higher number of acid molecules per __________ of solution.

    <p>dm3</p> Signup and view all the answers

    What product is formed when hydrochloric acid reacts with magnesium carbonate?

    <p>Magnesium chloride, carbon dioxide, and water</p> Signup and view all the answers

    Study Notes

    Proton Transfer

    • Acids are proton donors, releasing H+ ions in solutions, making the solution acidic.
    • Bases are proton acceptors, taking H+ ions from acids.

    Strong and Weak Acids

    • Strong acids fully ionize in water, creating solutions with a low pH.
    • Examples of strong acids are HCl and H2SO4.
    • Weak acids partially ionize in water, resulting in solutions with pH closer to 7.
    • Weak acids establish an equilibrium between the molecules and ions in water.
    • Examples of weak acids include propanoic acid and ethanoic acid.

    Acid-Base Reactions

    • Reaction with Metals: Acid + Metal → Salt + Hydrogen
      • Example: Magnesium + Hydrochloric acid → Magnesium chloride + Hydrogen
    • Reaction with Bases: Acid + Base → Salt + Water
      • Example: Magnesium hydroxide + Hydrochloric acid → Magnesium chloride + Water
    • Reaction with Carbonates: Acid + Carbonate → Salt + Carbon dioxide + Water
      • Example: Magnesium carbonate + Hydrochloric acid → Magnesium chloride + Carbon dioxide + Water

    Indicators

    • Indicators show the pH of substances.
    • Litmus is a natural indicator extracted from lichens, turning red in acid and blue in alkali.
    • Synthetic indicators, like thymolphthalein and methyl orange, are organic compounds showing distinct color changes in different pH ranges.

    pH Scale

    • The pH scale ranges from 0-14.
    • Acids have a pH below 7, alkalis above 7.
    • A neutral solution has a pH of 7.
    • Strong acids have a low pH (0-2), while strong alkalis have a high pH (12-14).
    • Universal indicators are mixtures of indicators used to determine the pH of a solution by matching the resulting colour to a chart.
    • Lower pH indicates higher H+ ion concentration, and higher pH indicates higher OH- ion concentration.

    Neutralization

    • Neutralization is a reaction between an acid and a base, producing salt and water.
    • The pH of the resulting solution is closer to neutral (pH 7).
    • The neutralization reaction is a commonly used process in chemistry.

    Titration

    • Titration is a technique used to determine the concentration of an unknown solution using a solution of known concentration.
    • A burette is used to deliver a known volume of the solution with known concentration (the titrant) into a flask containing the unknown solution (the analyte).
    • The endpoint of the titration is the point at which the reaction is complete, indicated by a clear color change in the indicator.
    • Titration is used in many chemical applications, including determining the concentration of acids and bases, measuring the amount of a substance in a sample, and monitoring chemical reactions.

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    Description

    This quiz explores the concepts of proton transfer, the characteristics of strong and weak acids, and the different types of acid-base reactions. Test your knowledge on how acids and bases interact and the nature of solutions they form.

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