Here is a generic statement of the problem to solve:

Determine the pH of a _____ M solution of _____ acid, K_{a} = _____.

Notice that the molarity, acid name and K_{a} are not there. That is because the solution technique is the same for almost all weak acids.

The following list gives sets of names and values that can be inserted into the above problem. The **boldface** first letter of the acid name and Number will be used in the assignment given below the table.

Name of Acid | K_{a}
| Number | Molarity |

Anisic
| 3.38 x 10¯^{5}
| 1 | 0.150 |

Cyanoacetic
| 3.65 x 10¯^{3}
| 2 | 0.200 |

Ethylbenzoic
| 4.47 x 10¯^{5}
| 3 | 0.325 |

Hexanoic
| 1.31 x 10¯^{5}
| 4 | 0.475 |

Methylmalonic
| 1.17 x 10¯^{4}
| 5 | 0.550 |

Trimethylacetic
| 9.40 x 10¯^{6}
| 6 | 0.700 |

1) Choose an acid from the above list. Please use the K_{a} listed just to the right of the acid name.

2) Now pick a molarity. It DOES NOT have to be in the same row as your acid.

3) Rewrite the generic statement of the problem, filling in the blanks with the specific acid name, K_{a} and molarity.

4) Solve the problem in this manner:

a) write the dissociation equation for the acid dissolving in water solution. Use the boldfaced letter to represent the anion (the part remaining after the acid donates its proton).

b) write the K_{a}expression for the specific acid.

c) calculate the pH of the acid solution, showing sufficient steps to justify your answer.

5) Pick a different acid and a different molarity and follow steps 3 and 4. Do this twice for a total of three problems completed.

Here is a generic statement of the problem to solve:

Determine the pH of a _____ M solution of _____ , K_{b} = _____.

Notice that the molarity, base name and K_{b} are not there. That is because the solution technique is the same for almost all weak bases.

The following list gives sets of names and values that can be inserted into the above problem. The **boldface** first letter of the base name and Number will be used in the assignment given below the table.

Name of Base | K_{b}
| Number | Molarity |

Aniline
| 4.62 x 10¯^{10}
| 1 | 0.150 |

Codeine
| 1.62 x 10¯^{6}
| 2 | 0.200 |

Ephedrine
| 9.08 x 10¯^{5}
| 3 | 0.325 |

Nicotine
| 1.05 x 10¯^{6}
| 4 | 0.475 |

Pyridine
| 1.78 x 10¯^{9}
| 5 | 0.550 |

Strychnine
| 1.82 x 10¯^{6}
| 6 | 0.700 |

1) Choose a base from the above list. Please use the K_{b} listed just to the right of the base name.

2) Now pick a molarity. It DOES NOT have to be in the same row as your base.

3) Rewrite the generic statement of the problem, filling in the blanks with the specific base name, K_{b} and molarity.

4) Solve the problem in this manner:

a) write the ionization equation for the base dissolving in water solution. Use the boldfaced letter to represent the base (which accepts a proton).

b) write the K_{b}expression for the specific base.

c) calculate the pH of the base solution, showing sufficient steps to justify your answer. Remember the additional step you must use at the very end of the problem.

5) Pick a different base and a different molarity and follow steps 3 and 4. Do this twice for a total of three problems completed.