Reading...
Play button
Play button
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;
18 Cards in this Set
- Front
- Back
|
Give the definition for an Arrhenius acid/base
|
acid - produces H+ in water
base - produces OH- in water |
|
|
Give the Bronstead definition for acids and bases.
|
acid - donates proton
base - accepts proton |
|
|
Give the Lewis definition for acids and bases
|
acid - accepts e- pair
base - donates e- pair |
|
|
Strong acids
|
HCl, HBr, HI, H2SO4, HNO3, HClO4
|
|
|
What is the value for Kw?
|
Kw=[H30+]{OH-] = 1.00 x 10 -14
|
|
|
How do you find pH?
|
pH= - log [H30+]
|
|
|
What is the relationship between pH and pOH?
|
pH + pOH = 14
|
|
|
What is the relationship between Ka and Kb?
|
Ka x Kb = Kw
|
|
|
What is pKa?
|
pKa= - log Ka
|
|
|
What are the two factors that determine acidic strength?
|
Bond polarity and bond strength
|
|
|
How does polarity affect acidic strength?
|
The more polar the bond, the stronger the acid.
|
|
|
How does bond strength affect acidic strength?
|
The stronger the bond, the weaker the acid.
|
|
|
How do periodic trends affect acidic strength?
|
Acidic strength increases across a period
|
|
|
How do group trends affect acidic strength?
|
Acidic strength increases going down a group
|
|
|
Two oxyacids with different central atoms - how is the stronger acid determined?
|
Acidity increase as electronegativity of the central atom increases
|
|
|
Two oxyacids with the same central atom - how is the stronger acid determined?
|
Acidity increases as the oxidation number of the central atom increases
|
|
|
Henderson-Hasselbalch Equation and purpose
|
pH = pKa + log (Conjugate base/Acid)
Used to determine the pH of a solution of acid after a certain amount of titrant is added. |
|
|
Kw =
|
Ka * Kb = 10^-14
|
