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You have a solution of the following acid: HOC 6 H 5 (aq) + H 2 O (l) H 3 O + (aq) + OC 6 H 5 - (aq) Given that the equilibrium concentrations are [HOC 6 H 5 ] = 0.062 M, [H 3 O + ] = 1.5 x 10 -4 M, and [OC 6 H 5 - ] = 3.1 x 10 -5 M, calculate the value of K a. ⇌

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Calculate the pH of a 0.036 M Nitric Acid (HNO 3 ) solution HNO 3 H + + NO 3 -

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Calculate the pH of a 0.036 M Sodium Hydroxide solution NaOH OH - + Na +

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Using the table below, which compound would you expect to be the strongest acid? A B C D

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CompoundKb Value A) Phosphate5.9 x 10 -3 B) Carbonate2.1 x 10 -4 C) Ammonia1.8 x 10 -5 D) Aniline9.5 x 10 -7

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Calculate the K a for the ammonium ion (K b = 1.8 x 10 -5 )

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Consider the following two acids and their ionization constants: HCOOHKa = 1.7 x 10 -4 HCNKa = 4.9 x 10 -10 Which conjugate base (HCOO- or CN-) is stronger?

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