Acids/Bases
In a salt solution, with a strong acid and a weak base, will the solution be basic or acidic
Acidic
What is the definition of a Lewis acid?
What is the equation for Kb?
Kb = [BH⁺] [OH⁻] / [B]
Salts from what will hydrolyze?
All group ____ compounds are soluble.
Group 1
When an acid is named with -ic suffix (ex: sulfuric acid), it comes from the compound ending in what suffix?
-ate
Sulfate --> Sulfuric acid
When an acid is named with -ous suffix (ex: nitrous acid), it comes from the compound ending in what suffix?
-ite
nitrite --> nitrous acid
Ka x Kb = ?
Kw = 1x10-14
Buffers are made from what kind of pairing?
Weak acid/base and its salt
How do you find the dissociation constand Kd?
1 / Kf
Inverse of the formation constant
In an acid base reaction, it proceeds from the ____ acid/base to the ____ acid/base
From strong to weak
In a salt solution, if we have a strong acid and a strong base, will the solution be acidic or basic?
Compare Ka & Kb
Higher Ka = Acidic
Higher Kb = Basic
How do you calculate percent ionization?
[H+ formed] / [HA initial] x 100 = % ionized
Where is the equivalence point in a titration curve?
Where it goes vertical
Where the two are equal (equivalence)
When Qc is greater than Ksp does a precipitate form?
Yes, a precipitate will form
With sequential acid/base polyprotic reactions, you can generally assume the pH will be based on?
The first Ka / first equilibrium
In reference to acid strength, is HClO or HClO2 stronger and why?
HClO2 is stronger
More O atoms pull electron density away, weakening the O-H bond
When can we assume in a RICE table that x is negligible or so small it doesn't count?
When it doesn't affect the significant figures of the initial concentration.
When Ka is very small. (1x10^-6 to -12)
When x makes up less than 5% of the initial concentration.
If you have a strong acid and a weak base, will the equivalence point in the titration be acidic or basic?
Acidic
When we have soluble solutions in buffers, (ex. Mg(OH)2 ) how do we find the OH concentration?
Use HH equation to find pH / pOH, then find [OH] and use that in the solubility equation.
If you move down a group (column) on a periodic table, what happens to acidity?
Acidity increases.
Larger atoms = longer, weaker H-X bonds = easier to break
If you move left across a period (row) on the periodic table, what happens to acidity?
It decreases
Right is increasing electronegativity, more electrons pulled to that side, easier to let H go.
What is the Henderson Hasselbach equation?
pH = pKa - log( [A-]/[HA] )
What is the common ion effect?
The suppression of ionization of a weak acid/base by adding a common ion (like H+ or OH-)
When we have a formation problem looking for the concentration of an ion, what step do we do before finding equilibrium?
Limiting reactant, assume it all forms first and then dissociates backwards.