| Question |
Answer |
| What is the relation of K(sp), solubility constant to soulubility? |
K(sp) is directly related to solubility; therefore the larger the K(sp) the more soluble the product |
| What is the common ion effect? |
Another form of Le Chatelier's Principle, the the decrease in the solubility of a salt occurs because another salt is added that contains one of its ions. |
| What is the relatonship bw autoionization of water K(w) and temp |
it increases when temp increases |
| polyprotic |
can accept or donate more than one H+ |
| high [H] means... |
low pH and the solution is acidic |
| pH + pOH = |
14 |
| pH = |
-log[H] or -log[H3O+] |
| pOH = |
-log[OH] |
| What is the relation bw K(a) and pKa? |
The larger the K(a) value the smaller the pKa value and therefore the stronger the acid |
| What is the Henderson-Hasselbalch equation? |
pH = pKa + log {[conjugate base]/[weak acid]} |
| what happens at a half-equivalence point? |
the pKa equals the pH |
| K(w) |
= [H3O+][OH-] |
| Titration equation |
pH = [vol acid]/ [vol base] |
| pKa + pKb = |
14 |
Ch.18 LTI-MA 509
