Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
19 Cards in this Set
- Front
- Back
What is an Arrhenius acid or base?
|
acid: dissociates to form an excess of H in solution;
base: dissociate to form excess of OH in solution; |
|
What is a Bronsted-Lowry acid or base?
|
acid: species that donates H ions;
base: a species that accepts them ---> not limited to solutions |
|
What is a Lewis acid or base? What's the mnemonic?
|
acid: electron pair acceptor
base: electron pair donor; Lewis Acid is an Acceptor of electron pairs; |
|
what is an amphoteric species? amphiprotic? |
one that reacts like an acid in a basic environment and like a base in an acidic environment; amphiprotic: can either gain or lose a proton |
|
Upon what factors is Kw dependent? |
only temperature |
|
When is pH = 7 --> neutral valid? |
only at 25 degrees C |
|
What is a trick for calculating log values when it isn't 1 x 10^-m? |
long(n x 10^-m) = -log(n) - log(10^-m) = m - log(n) -----? p = m - 0.n |
|
What is the equation for the acid dissociation constant? |
Ka = [H3O+][A-]/[HA]; the smaller the Ka, the weaker the acid; generally, weak acid if Ka is less than 1.0, same for weak base |
|
What is induction? |
electronegative elements positioned near an acidic proton increase acid strength by pulling electron density out of the bond holding the acidic proton |
|
What happens when you react a strong acid with a weak base? or opposite? |
(strong a) + (weak b) --> (very weak b) + (okay a); (okay a) + (water) --> (weak b) + (H3O+); final pH below 7 |
|
what happens if you react a weak acid and a weak base? |
must compare the strengths of the reactants; if one has a stronger Kb than the other has a Ka, then it will be more basic, etc. |
|
what is an acid equivalent? |
1 mole of H |
|
What is normality? |
quantity of acidic or basic capacity; so each mole of H3PO4 yields three moles of H3O. so 3N |
|
What is gram equivalent weight? |
mass of a compound that produces one equivalent (one mole of H or OH) |
|
what is a titrant? |
the solution of known concentration |
|
what is the equivalence point? what is the equation that represents this? |
when number of acid equivalents present in the original solution equals number of base equivalents, vice-versa; NaVa = NbVb |
|
What are the three most population buffer systems? |
acetic acid (CH3COOH) and sodium acetate (CH3COO-Na+); ammonia (NH3) and ammonium chloride (NH4+Cl-); Bicarbonate CO2 (g) + H2O (l) <--> H2CO3 <--> H+ +HCO3- |
|
What is the range of optimal activity for buffers? |
pKa +/- 1 |
|
What is the Henderson-Hasselbalch equation? both pKa and pKb forms |
pH = pKa + log [A-]/[HA]; pOH = pKb + log [B+]/[BOH] |