Term
| What are two physical features of acids? |
|
Definition
| They are sour and corrosive |
|
|
Term
| What are two physical features of bases? |
|
Definition
| They are bitter and slippery |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| Molecule that can act as either an acid or a base (ie. H2O) |
|
|
Term
|
Definition
| Will dissociate essentially completely; Ka is large. Yields relatively weak conjugate bases. EX: HCl, HNO3 |
|
|
Term
| Monoprotic acid versus diprotic acid |
|
Definition
| Monoprotic acids have one acidic proton while diprotic acids have two acidic protons |
|
|
Term
|
Definition
| Measure of acidity/basicity of a solution. pH=-log[H+] As [H+] increases, pH decreases. |
|
|
Term
|
Definition
| Will dissociate essentially completely; Kb is large. Yields a relatively weak conjugate acid. EX: NaOH, KOH |
|
|
Term
|
Definition
| Kw = [H+][OH-] = 1.000 x 10^(-14) |
|
|
Term
| In the presence of an acid, ignore the [H+] from water, except when: |
|
Definition
1. the acid concentration is extremely small
2. working with organic acids |
|
|
Term
| For a weak acid, the percent dissociation increases as the acid becomes more _______. |
|
Definition
|
|
Term
|
Definition
| Conjugate acid/base pairs that resist changes in pH. |
|
|
Term
| What is the Henderson-Hasselbalch equation? |
|
Definition
| pH = pKa + log([A-]/[HA]) |
|
|
Term
| What are the three conditions of the Henderson-Hasselbalch equation? |
|
Definition
1. Value of Ka for conjugate acid is between 10^(-11) and 10^(-4)
2. Ratio of [base]/[acid] is between 0.1 and 10
3. Values of [acid] and [base] are between 10^(-3) M and 1 M |
|
|
Term
| For the reaction quotient Q, what does it mean when Q=K? Q>K? Q |
|
Definition
Q=K ... the system is at equilibrium
Q>K ... the rxn shifts to the left, consuming products and forming reactants
Q |
|
|
Term
| What is the significance of the magnitude of K? |
|
Definition
| K describes the inherent tendency of a reaction to occur. |
|
|
Term
|
Definition
| (amount dissociated in M)/(initial concentration in M) X 100 |
|
|
Term
|
Definition
|
|
Term
| When a salt has a cation that's the conjugate acid of a weak base, what is the solution pH? |
|
Definition
|
|
Term
| What is the common ion effect? |
|
Definition
| The shift in equilibrium that occurs because of the addition of an ion already involved in a reaction. |
|
|
