Intermediate 2 Chemistry - Unit 3(A)

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    In water and aqueous solutions there is an _______________ between hydrogen and hydroxide ions and water molecules.

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About This Quiz


A quiz which assesses the content statements from the SQA Intermediate 2 Chemistry course, Unit 3(a): acids and bases.

Intermediate 2 Chemistry - Unit 3(A) - Quiz

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  • 2. 

    An alkaline solution has a pH of above 7 and contains a higher concentration of hydroxide ions than hydrogen ions.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    An alkaline solution is characterized by having a pH value above 7, indicating that it is basic rather than acidic. This means that the concentration of hydroxide ions (OH-) in the solution is higher than the concentration of hydrogen ions (H+). In other words, there are more hydroxide ions available to accept protons than there are protons available to donate. Therefore, the statement that an alkaline solution has a higher concentration of hydroxide ions than hydrogen ions is true.

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  • 3. 

    The concentration (in mol l-1) of a solution made by dissolving 0.25mol of sodium chloride in 500cm3 of water is...

    Correct Answer
    0.5
    Explanation
    The concentration of a solution is calculated by dividing the amount of solute (in moles) by the volume of the solution (in liters). In this case, 0.25 mol of sodium chloride is dissolved in 500 cm3 of water. To convert the volume from cm3 to liters, we divide by 1000. So, the volume of the solution is 500/1000 = 0.5 L. Therefore, the concentration is 0.25 mol / 0.5 L = 0.5 mol L-1.

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  • 4. 

    In pure water, there are no hydrogen or hydroxide ions, only water molecules.

    • True

    • False

    Correct Answer
    A. False
    Explanation
    In pure water, there are actually very small amounts of hydrogen and hydroxide ions present due to the process of self-ionization. This is when water molecules can break apart into hydrogen ions (H+) and hydroxide ions (OH-). Therefore, the statement that there are no hydrogen or hydroxide ions in pure water is false.

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  • 5. 

    When a reversible reaction is in equilibrium...

    • ...the concentrations of reactants and products are equal

    • ...the concentrations of reactants and products are constant

    Correct Answer
    A. ...the concentrations of reactants and products are constant
    Explanation
    In a reversible reaction at equilibrium, the concentrations of reactants and products remain constant. This means that the rate of the forward reaction is equal to the rate of the reverse reaction, resulting in a stable concentration of both reactants and products. This state of equilibrium is achieved when there is no net change in the concentrations of reactants and products over time.

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  • 6. 

    Diluting an acid or an alkali brings the pH closer towards 7 because this lowers the concentration of hydrogen and hydroxide ions.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Diluting an acid or an alkali reduces the concentration of hydrogen and hydroxide ions in the solution. Since the pH scale measures the concentration of these ions, dilution will result in a decrease in the pH value. As a result, the pH of the solution will move closer towards 7, which is considered neutral on the pH scale. Therefore, the given statement is true.

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  • 7. 

    How many grams of sodium hydrxide are required to make up 500cm3 of a 0.1 mol l-1 solution?

    Correct Answer
    2g
    2 g
    Explanation
    To calculate the grams of sodium hydroxide required, we need to use the formula:

    grams = moles x molar mass

    Given that the solution is 0.1 mol/l and the volume is 500 cm3, we can calculate the number of moles:

    moles = concentration x volume
    moles = 0.1 mol/l x 0.5 l
    moles = 0.05 mol

    The molar mass of sodium hydroxide (NaOH) is 40 g/mol. Plugging in the values, we can calculate the grams:

    grams = 0.05 mol x 40 g/mol
    grams = 2 g

    Therefore, 2 grams of sodium hydroxide are required to make up 500 cm3 of a 0.1 mol/l solution.

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  • 8. 

    Which of the following substances produce an acid(s) when added to water?

    • Sodium chloride

    • Hydrogen chloride

    • Copper(II) oxide

    • Sodium oxide

    • Carbon dioxide

    • Silicon oxide

    • Sodium carbonate

    • Sodium sulphate

    • Sodium hydroxide

    • Ammonia

    Correct Answer(s)
    A. Hydrogen chloride
    A. Carbon dioxide
    Explanation
    Hydrogen chloride (HCl) is a substance that produces an acid when added to water. When HCl dissolves in water, it dissociates into H+ ions and Cl- ions, resulting in the formation of hydrochloric acid (HCl). This acid increases the concentration of H+ ions in the solution, making it acidic. Similarly, carbon dioxide (CO2) also produces an acid when added to water. When CO2 dissolves in water, it reacts with water to form carbonic acid (H2CO3), which increases the concentration of H+ ions, making the solution acidic.

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  • 9. 

    Which of the following substances produce an alkali(s) when added to water?

    • Sodium chloride

    • Hydrogen chloride

    • Copper(II) oxide

    • Sodium oxide

    • Carbon dioxide

    • Silicon oxide

    • Sodium carbonate

    • Sodium sulphate

    • Sodium hydroxide

    • Ammonia

    Correct Answer(s)
    A. Sodium oxide
    A. Sodium carbonate
    A. Sodium hydroxide
    A. Ammonia
    Explanation
    Sodium oxide, sodium carbonate, sodium hydroxide, and ammonia produce an alkali when added to water. These substances have the ability to react with water to form hydroxide ions (OH-) which give the solution an alkaline pH. Sodium oxide (Na2O) reacts with water to form sodium hydroxide (NaOH). Sodium carbonate (Na2CO3) also reacts with water to form sodium hydroxide. Sodium hydroxide (NaOH) itself is a strong alkali. Ammonia (NH3) dissolves in water to form ammonium hydroxide (NH4OH), which is also an alkali.

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  • 10. 

    Which of the following statements relating to strong and weak acids and bases is/are true?

    • Hydrochloric acid and nitric acid are both strong acids

    • Ammonia is a strong base

    • A strong acid is fully dissociated into ions in aqueous solution

    • A strong acid will always have a lower pH than a weak acid

    • 0.1 mol/l HCl and 0.1 mol/l HNO3 have the same pH

    • 0.1 mol/l HCl and 0.1 mol/l H2SO4 have the same pH

    • Equimolar solutions (equal concentrations) of ethanoic acid and hydrochloric acid will conduct electricity equally well

    • Equimolar solutions of ethanoic acid and hydrochloric acid will react at the same rate with magnesium ribbon

    • Equimolar solutions of ammonia and sodium hydroxide will have the same pH

    • A solution of ammonia has more ions present in it than a solution of sodium hydroxide

    Correct Answer(s)
    A. Hydrochloric acid and nitric acid are both strong acids
    A. A strong acid is fully dissociated into ions in aqueous solution
    Explanation
    Hydrochloric acid and nitric acid are both strong acids because they completely dissociate into ions in aqueous solution. This means that they break apart into their component ions, H+ and Cl- for hydrochloric acid, and H+ and NO3- for nitric acid. This complete dissociation results in a high concentration of H+ ions in the solution, leading to a low pH. Therefore, a strong acid will always have a lower pH than a weak acid, which only partially dissociates in solution.

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  • Current Version
  • Aug 22, 2023
    Quiz Edited by
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  • Apr 05, 2011
    Quiz Created by
    Brobertson13
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