What is concentration of hydronium (H3O+) * concentration of hydroxide (OH-) always equal to (equilibrium constant)
10^-14

What side of the reaction is heat on (use with le chatelier principle)
left

Is pH negative log of hydronium (H3O+/H+) or hydroxide (OH-)
hydronium

What is pH + pOH equal to
14

pH of solution with strong acid, what happens to the acid when it enters water
fully disassociates

For strong acid kA is `a`, for weak acid is `b`
a: much greater than 1
b: much less than 1

For this acid what is numerator of kA equal to, assuming concentration of H3O is x
x^2

In a salt where the anion is from a weak acid (e.g. acetate) is the solution acidic or basic
basic

In a salt where the cation is from a weak acid (e.g. ammonium) is the solution acidic or basic
acidic

For an acid base pair (e.g. ammonium acetate) what is true about the Ka (ammonium) and Kb (acetate)
KaKb = Kw

pH of weak acid + conjugate base (HA/A-), e.g. acetic acid and sodium acetate (which dissasociates)
pKa + log([A-]/[HA])

At what point in buffer is it not effective (ratio between A- and HA or HA and A-)
10

What pH range relative to pKa is buffer effective
+/- 1

When you add acid to a buffer what goes down, HA or A-
A-

When you titrate a weak acid (e.g. acetic acid) with a strong base is pH above or below 7
above

At half equivalence point with weak acid titrated by strong base what is formed (you can use equations for this)
buffer

What do you look at when choosing an indicator (this value should be close to the equivalence point)
pKa