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BCE

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Answer all of the questions below. If you do not know an answer enter CNA. However, it will help me the most if you answer each question with your best intuition/idea about what would be a reasonable answer.

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A second definition of acids and bases is the Bronsted-Lowry definition. According to this definition an acid is a proton, H+, donor and a base is a proton acceptor.

1. In the following equation, label the Bronsted-Lowry acid and base (on the reactants side) and the Bronsted-Lowry acid and base on the product side;

 

NH3(aq)

+

HNO3(aq)

NH4+(aq)

+

NO3-(aq)

Your Response:

 

 

conjugate

 

conjugate

2. A Bronsted-Lowry conjugate acid/base pair differe by ONLY a proton, H+. In Q1 there are two Bronsted-Lowry conjugate acid/base pairs? Write the pair using the following format....acid/base.

conjugate acid/base pair #1

conjugate acid/base pair #2

3. For the reaction in Q1, the equilibrium constant, K, is VERY large. Using the chemical equation in Q1, and knowing that K is very large, identify the strongest acid and the strongest base in the equation.

formula of the strongest acid

formula of the strongest base

You are given a solution with the label 0.500 M formic acid (HCOOH). Formic acid is know to be a weak acid. Answer the following questions.

5. Is the concentration of HCOOH in the solution actually 0.500 M? Explain.

6. Write an Arrhenius or a Bronsted-Lowry chemical equation which describes how formic acid behaves as an acid.

7a. The pH of the 0.500 M HCOOH solution is 2.02, calculate the [H+] in this solution.

[H+] = M

If formic acid were a strong acid, what would be the pH of the solution? (Hint: You may want to set up an ICE table.)

pH =

9. Is there anything about the questions that you feel you do not understand? List your concerns/questions.

10. If there is one question you would like to have answered in lecture, what would that question be?