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WorksheetsAP Acid Base Review
Total questions: 20
Worksheet time: 53mins
KOH is ...
an acid
a base
a salt
an ionic compound
What is the [H+] if the pH is 4.0?
1.0 x 10-10 M
1.0 x 10-4 M
1.0 x 10-14 M
1.0 x 10-7 M
What is a titration?
when the moles of hydrogen ions is equal to the moles of hydroxide ions
adding a known amount of solution of known concentration to determine the concentration of an unknown
reaction in which an acid and a base react in an aqueous solution to produce a salt and water
the extent of ionization of an acid or base
What completely ionizes in solution?
Weak acids
Strong acids
Strong Salts
Neutral salts
A solution contains 0.04 M of a weak acid. Calculate the pH of the solution knowing that the Ka for the acid is 1.6 x 10-7
It is not possible to solve if the identity of the acid is not known
4.1
4.9
Because the Ka is very small, the pH is close to neutral (about 6)
When 200 mL of 2.0 M NaOH(aq) is added to 500 mL of 1.0 M HCl(aq), the pH of the resulting mixture is closest to
0.85
3.0
7.0
13.0
What is the pK a of hydrocyanic acid, if its Ka is 4.9 x 10 −10 ?
6.5
9.1
9.3
5.4
A student was testing the pH of two different acid solutions and found them both to have a pH of 3.25. Which of the following must be true?
Both solutions must be weak acids.
Both solutions must have the same molarity.
Both solutions must have the same percent dissociation.
Both solutions must have the same hydronium ion concentration.
Given 0.10 M solutions of the four weak acids below all with 0.10 M concentration, which will have the greatest percent ionization?
HF (Ka = 7.2 x 10-4)
HNO2 (Ka = 4.0 x 10-4)
HCO2H (Ka = 1.8 x 10-4)
HC3H5O3 (Ka = 1.4 x 10-4)
HF because its Ka is the largest.
HF because its molar mass is the smallest.
HC3H5O3 because its Ka is the smallest.
HC3H5O3 because its molar mass is the greatest.
What is the pH of a buffer mixture of 0.70 M KCH3COO and 0.50 M CH3COOH (Ka = 1.8x10-5)?
0.45
4.89
4.60
4.74
Which of the following best approximates the Ka value for this weak acid?
1 x 10–4
1 x 10–5
5x 10–6
5 x 10–7
Which point on the titration curve corresponds to the point at which the moles of the added strong base are equal to the moles of the weak acid initially present?
Q
R
S
T
50 mL of 0.10 M HCl is titrated by 0.20 M NaOH. What is the volume of NaOH at the equivalence point?
25 mL
50 mL
100 mL
75 mL
Which acid base pair produced this titration curve?
HCI + KOH
HCI + NH3
CH3COOH + KOH
CH3COOH + NH3
A student used a 0.125 M of sodium hydroxide solution in a titration experiment. The initial reading on the buret was 0.45 mL. After the titration, the buret reading was 14.98 mL. How many moles of sodium hydroxide was used?
1.82 moles
1.82 x 10-3 moles
8.34 x 10-3 moles
8.6 moles
How many mL of a 0.12 M NaOH solution are needed to neutralize 18 mL of 0.15 M H3PO4 solution?
3NaOH (aq) + H3PO4 (aq) ----> Na3PO4 (aq) + 3H2O (l)
7.5 mL
0.015 mL
68 mL
23 mL
