Chapter 16 Review: Acids and Bases Name: Hr:
Terms:
Arrhenius acid Arrhenius base Bronsted-Lowry acid buffered solution
Bronsted-Lowry base strong acid weak acid equivalence point
amphoteric neutral solution acidic solution indicator
basic solution
Questions:
1) What is the pH of a 1 M solution of each of the following? NaOH, HF, HCl, H2O
2) What happens to the [H+]/[OH-] ratio as the pH of a solution increases / decreases? (Does it stay the same, get larger or smaller?)
3) Which pH values represent an acidic solution? neutral solution? basic solution?
4) Why can an acid be both strong and dilute?
5) What is the ion product constant for water?
6) What is pH? What does it measure?
7) What are conjugate acid/conjugate base pairs? How do you know if you are dealing with one? Give an example.
8) Calculate [H+] in a solution if [OH-] = 3.25 x 10-8 M at 25oC, and tell if the solution is acidic, basic, or neutral.
9) What is the pH of a solution if [OH-] is 1.0 x 10-6 M?
10) If the pOH of a solution is 4.27, what is [H+]?
11) What is the pH of a 0.15 M HCl solution?
12) Calculate the pH of a solution that has [H+] = 2.5 x 10-11 M, and tell if the solution is acidic, basic, or neutral.
13) What does a buffer solution contain? How does a buffer work?
14) What does a neutralization reaction produce?
15) Write a chemical equation that show how each of the following species behaves as an acid when dissolved in water. HCN, NH4+, H2PO4+
16) Calculate [H+] and pH for each of the following solutions, and tell whether the solution is acidic, basic, or neutral.
[OH-] = 8.16 x 10-3 M , [OH-] = 6.5 x 10-11 M , [OH-] = 1.00 x 10-5 M
17) Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH or pOH values, and tell whether the solution is acidic, basic, or neutral.
a) pH = 6.44
b) pH = 12.75
c) pOH = 10.50
18) If 50.0 mL of a HCl solution requires 20.0 mL of 0.20 M NaOH to titrate it to the equivalence point, what is the concentration, in moles per liter, of the HCl solution?