Name: _____________________________
Date: ___________
Acid-Base Test Review
Period: ______
1. List 3 properties of just ACIDS:
2. List 3 properties of just BASES:
3. In a neutral solution the
a. pH = ____________,
b. pOH = ___________,
c. [OH-1] = ___________
d. [H+] = ___________
4. Write Acid/Base definitions and give one example
a. Arrhenius acid:
b. Arrhenius base:
c. Bronsted-Lowery acid:
d. Bronsted-Lowery base:
e. Lewis acid:
f. Lewis base:
5. Define and give an example for each of the following:
a. Monoprotic acids
b. Diprotic acids
c. Triprotic acids
6. Complete the table
Base
HSO4–1
Conjugate acid
Acid
HSO4–1
F-1
HC2H3O2
O2-
HNO2
NO3-1
H2CO3
SO4-2
H2S
HCO3–1
HCO3–1
Conjugate base
7. Label the acid, base, conjugate acid, and conjugate base in the reactions below:
a. HSO4-1 + NH4+1 → H2SO4 + NH3
b. H2O + NH3 → OH-1 + NH4+1
c. H2PO4-1 + H2O → OH-1 + H3PO4
8. Complete the following data table
pH
pOH
11.25
[H+1]
[OH-1]
Acid/Base/Neutral
1 x 10-7
2.53 x 10-13
9.14
9. Complete the following calculations
a. Find pH if [OH-1] = 2.8 x 10-8
b. Find [OH-1] if [H+1]= 8.64 x 10-3
c. Find pOH if [H+1]= 4.76 x 10-11
d. Find [H+1] if pOH = 6.48
10.
Acids
pH
Taste
Feel
Turn Litmus Paper
TWO Examples
(formula and Name)
Common Use
Two Properties that
BOTH have
Bases
11. Molarity
a. Define molarity
b. Find the molarity of a solution made with 425 mL and 68 g of HC2H3O2
c. What is the mass of H3PO4 used to make 75 mL of a 4.25 M solution?
d. What is the volume needed to make 2.50 M solution with 14.5 g of NaOH?
12. Define concentrated solution
13. Define dilute solutions.
14. How do concentrated and dilute solutions they differ from each other.
15. What are the units for solubility?
16. What are the factors that affect solubility of a solid in a liquid?
17. What are the three thing that you can do to dissolve a solid faster in a solvent?
18. Using the chart what are different types of
solutions (saturated, unsaturated or super
saturated) formed when the following
mass of potassium nitrate is dissolved at
400c
a. 65 Grams
b. 80 grams
c.
45 grams
19. How many grams of NaBr can dissolve at
80°C in the following amounts of water
a. 200 g H2O
b. 50 g H2O
c. 5.50 x 103 g H2O
FOLLOWING ITEMS ARE FOR HONORS ONLY
20. Write soluble or insoluble using solubility rules below
PbCO3
copper (II) sulfide
cadmium (II) sulfide
BaSO4
Mg3(PO4)2
zinc carbonate
Hg2SO4
PbI2
21. For following problems predict the products. Write the equation, balance it and circle the
compound that is insoluble.
a. Barium carbonate reacts with sodium sulfate
b. Ammonium chloride reacts with lead II chlorate
c. Magnesium iodide reacts with potassium phosphate
22. Find the volume of water necessary to make 250 mL of a 2.5 M solution from a 18 M solution?
23. What will the concentration (molarity) be if I add 560 mL of water to 340 mL of a 0.5 M NaBr
solution,
24. If I dilute 250 mL of 0.10 M lithium acetate solution to a volume of 750 mL, what will the
concentration (molarity) of this solution be?
NH4+1 and Group 1
NO3-1, C2H3O2-1, ClO3-1
Cl-1, Br-1, or I-1
F-1
CO3-2, PO4-3, CrO4-2,
OH-1
S-2
Solubility Rules for Ionic Compounds
Soluble Compounds
Ammonium and alkali metals all are soluble
Nitrate, acetate, and chlorate salts all are soluble
Chloride, Bromide, or Iodide Salts are soluble
[except Pb+2, Ag+1, Hg2+2 are insoluble]
Fluoride salts are soluble
[except group 2 (IIA), Pb+2, Fe+3 are insoluble]
Insoluble compounds
Carbonates, phosphate, and chromates are insoluble
[except: alkali metal and ammonium are soluble]
Hydroxide are insoluble
[except alkali metals, Sr+2, Ba+2, and ammonium are soluble]
Sulfides are insoluble
[except alkali metals, alkaline earth metals and ammonium are soluble]