| 1020 - Buffer Solutions |
| 1010 - Recognize buffers are solutions that resist changes in pH. |
| 1020 - Use LeChateliers principle to rationalize buffer action. |
| 1030 - Explain why buffers solutions are made from a weak acid and its conjugate base. |
| 1040 - Use an ICE table to relate the pH of a buffer solution to the molarity solutes. |
| 1050 - Use the Henderson-Hasselbach equation to relate the pH of a buffer solution to the molarity solutes. |
| 1030 - Buffer Effectiveness |
| 1010 - Define the buffer properties effectiveness, range and capacity. |
| 1020 - Explain how the relative amount of acid and base relates to buffer effectiveness. |
| 1030 - Identify the ratio of acid and base at which buffers are most effective. |
| 1040 - Explain how the absolute amount of acid or base relates to buffer capacity. |
| 1050 - Identify the effective range of a buffer, given the pKa of its acid. |
| 1060 - Given quantities of acid and base in a buffer, calculate the capacity of the buffer for acid or base. |
| 1040 - Titration & pH Curves |
| 1010 - Determine the solute moles and concentration of a solution by titration and stoichiometry. |
| 1020 - Find the buffer region of pH curve from a weak acid or base and its strong conjugate. |
| 1030 - Describe and differentiate between end point, equivalence point and half equivalence point. |
| 1040 - Use a titration curve to determine the Ka of the component acid (where analyte is either a weak acid or base). |
| 1100 - Identify a polyprotic acid by the number of plateus in a pH curve. |
| 1110 - Define indicators as substances that change colors at specific pH values. |
| 1120 - State the pH range of phenothelein, bromothymol blue and litmus indicators. |