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;
26 Cards in this Set
- Front
- Back
Arrhennius Theory |
Based on what forms H+ (acid) and OH- (base) ions in water |
|
Limits of Arrhenius Theory |
Not all reactions happen in water, and some bases don't have OH- |
|
Brown-sted- Lowry Theory |
Based on what donate H+( acid) and what accepts H+ proton (base) |
|
Conjugate pairs |
base ->Conjugate acid acid->Conjugate base |
|
ionization of HCL |
Strong acid so it ionizes 100% which means it is not in equilibrium |
|
Ionization of Acetic Acid |
Weak acid so it does not ionize 100% which means it is in equilibrium will have electro negative ions |
|
Bronsted lowry Acid vs Base |
Acid- must have a removable proton base- must have a lone pair |
|
Amphiprotic |
Can act as an acid and a base ex. water |
|
Ka and Kb |
equilibrium constants for acid or base only for weak acid + base because they go to equilibrium A reaction can have ka and kb at the same time Pka+pkb=14 Kw= Ka*Kb (1.0*10^-14) |
|
PH scale |
Based on Concentration of [H3O+] pH= -log[H3O+] pOH= -log[OH-] [H3O+] =10^-pH [OH-]= 10^-pOH pKw= -logKw (14 at 25C) pKw(14)= pH+pOH
|
|
pH of 2 vs pH of 4 |
pH of 2 is 100x more acidic 10*10 |
|
How to measure pH? |
Use litmus paper -Red paper turns blue (above 8) -Blue paper turns reds (below 5) pH meter measures voltage i a solution -more accurate |
|
5% rule |
Percent ionization: [h3O] / [HA]initial |
|
Acid vs base reaction |
Acid produce H3O+ Base produce OH- |
|
Polyprotic Acids |
protic is based on the number of H's Ka1 is always greatest because that is when all the H3O+s are made |
|
Stronger the acid... |
Weaker the conjugate base |
|
Reactions always go from (based on strength of acid/base) |
Stronger member to weaker member |
|
lower pKa |
Stronger acid |
|
Strong Acids |
HI HBr HCl H2SO4 HNO3 H3O+ |
|
more polar (weaker H-X) the bond |
Stronger the acid |
|
Stronger the forward reaction |
Stronger the acid |
|
Larger Radius |
Stronger the acid |
|
Acid strength is inversely proportional to |
the strength of H-X bond dissociation energy |
|
More oxygen |
Stronger acid |
|
WHen OH bonds to atom, More electronegative... means |
Stronger acid |
|
Carboxylic acids |
Have -COOH group |