Strong Acids/Bases
Weak Acids/Bases
Buffer Solutions
Titrations
Chance
100
[H3O+] of a solution with a pH of 4.56
2.75 x 10-5 M
100
Rank the following from weakest to strongest acid
HCl, NH3, HI
What is
NH3< HCl< HI
100
Write the Henderson Hasselbalch Equation
pH = pka + log([A-]/[HA])
100
Draw the curve of a strong acid being titrated with a strong base
see board
100
If an acid has a pKa of 4.6, what is its pKb?
What is 9.4
200
pOH of a 0.3M HCl Solution
What is 13.47
200
Rank the following from highest to lowest pH:
HI, NaOH, HCN, Ca(OH)2
Ca(OH)2>NaOH>NH3>HCN>HI
200
List three common buffer solutions
Acetic Acid, Benzoate, phosphate buffer, bicarb buffer, etc
200
do you expect this compound to be acidic, basic or neutral - (CH3NH3)(ClO4)?
Acidic (CH3NH3+ strong enough to protonate water)
300
[OH] = 4.7 x 10-4. What is the pH and is this solution acidic or basic?
What is 10.67 and Basic.
300
Draw the weak acid of the imidazole ion.
Lone pair on nitrogen with original positive charge
300
What is the equivalence point?
equivalence point: moles of acid = moles of base added
300
What is the pH of a solution containing 60mg of NaOH in 300mL?
The molar mass of KOH is 56 g/mol
pH=11.55
400
The [¯OH] in a solution containing a pH of 3.45
What is 2.818 x 10-11 M
400
What is the [HA] initially of a weak monoprotic acid if the resulting pH is 3.6 and the ka=1.5x10-6?
[HA]=0.0421
400
What is the pH of a 0.17M solution of KCN at 25°C? The Ka of HCN is 4.9 x 10-10
pH = 11.28
500
The pH of a 0.4 M solution of Ba(OH)2
What is 13.9
500
What is the pKb of a weak monoprotic base if the pOH of a 0.35 M solution is 1.95 at 25°C?
What is a pkb of 3.45
500
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid and 0.220 M sodium benzoate.
How many milliliters of each solution should be mixed to prepare this buffer?
22 mL benzoate
78 mL benzoic acid