Chemistry Videos

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  1. Define acids and bases according to the Bronsted-Lowry and Lewis theories.

  2. What are the factors that affect the strength of an acid?

  3. Rank the following in terms of acidity: HClO, IOH, and HBrO. Explain the trend.

  4. Rank the following in terms of acidity: HClO, HClO\(_2\), HClO\(_3\), HClO\(_4\). Explain the trend.

  5. Rank the following in terms of basicity:

    HCN K\(_a\) = 4.8 x 10\(^{-10}\)

    HSO\(_4^-\) K\(_a\) = 1.2 x 10\(^{-2}\)

    HS\(^-\) K\(_a\) = 7.1 x 10\(^{-15}\)

    H\(_2\)CO\(_3\) K\(_a\) = 4.3 x 10\(^{-7}\)

  6. In the below reactions, identify which reactant is the lewis acid and which is the lewis base.

    NH\(_3\) + BF\(_3\) \(\leftrightharpoons\) NH\(_3\)BF\(_3\)

    KOH + CH\(_3\)Br \(\leftrightharpoons\) KBr + CH\(_3\)OH

  7. Hydrogen bromide is a gas at room temperature. It is soluble in water, forming hydrobromic acid. Identify the conjugate acid-base pairs.
    HBr (aq) + H\(_2\)O (l) \(\longrightarrow\)

  8. Ammonia is a pungent gas at room temperature. Its main use is in the production of fertilizers and explosives. It is very soluble in water. It forms a basic solution that is used in common products, such as glass cleans. Identify the conjugate acid-base pairs in the reaction between aqueous ammonia and water.

    NH\(_3\) (aq) + H\(_2\)O (l) \(\longrightarrow\)

  9. Predict the products for the following reaction

    KHSO\(_3\) + NH\(_3\) \(\leftrightharpoons\) ?

    KHSO\(_3\) has K\(a\) = 6.2 x 10\(^{-8}\) K\(b\) = 1.0 x 10\(^{-4}\)

    NH\(_3\) has K\(a\) = 7.8 x 10\(^{-13}\) K\(b\) = 1.8 x 10\(^{-5}\)

  10. The percent ionization of NH\(_3\) is found to be 4.2% in a solution, find the concentration of NH\(_3\).

    NH\(_3\) (aq) + H\(_2\)O \(\leftrightharpoons\) NH\(_4^+\) + OH\(^-\) , K\(_b\) = 1.8 x 10\(^{-5}\)

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