Ch. 4 Review – Reaction in Aqueous Solution
TEST NOTES:
1) Predicting Reactions: There will be a predicting reactions portion of the test. You will be asked to complete 3 net
ionic equations and answer a follow-up question. (8 reactions = 19 points)
a. Precipitate
b. Gas Formation
c. Acid/Base (Acids could be strong or weak; know how to write acid formulas given the name)
d. Redox
e. Combination
Note: Emphasis will be placed on the first
i. Metal oxide + water  base
four (a-d) reaction types. At least one
ii. Nonmetal oxide + water  acid
other reaction (e-f)will be assessed.
iii. Metal oxide + nonmetal oxide  salt
f. Decomposition (see pink Molecular reactions sheet)
Examples and points explained below.
2) Multiple Choice
a. Stoichiometry – there are a significant number of “hard” stoichiometry problems. Make sure you’ve
learned strategies involved in solving stoichiometry problems in a proficient way.
b. Redox balancing – there are a significant number of redox equations to balance. Be sure you feel
comfortable enough with them to balance them proficiently.
c. Predicting Reactions – there will be some predicting reactions and descriptive chemistry as well.
3) Free Response – The free response questions will emphasize the recent labs. Be sure to take time remembering
any descriptive chemistry involved: colors of ions, solids, solutions, or gases.
- Stoichiometry
o How do you use data to determine the correct mole ratio?
o How are graphs used in this determination?
o What can make your experimental set-up more reliable?
- % Cu in Brass
o How do you write the correct balanced equation for the reaction of brass in concentrated
nitric acid?
o How do you calculate the amount of concentrated acid to react with your sample?
o How do you make serial dilutions?
o How to you use spectrophotometric data to determine the concentration of copper (II)
ions in your solution?
o How do you use the visual method to determine the concentration of copper (II) ions in
solution?
o How do you determine the mass of copper in your brass sample?
- Redox Titration.
o What does standardization mean?
o How do you predict products when mixed with potassium permanganate?
o How do you do stoichiometric calculations involving redox titrations?
o How do you explain the use of the permanganate ion as an indicator?
o How do you predict the effect of lab errors on your calculated results?
Predicting Reactions:
You must very purposefully prepare for this section. Many students do splendidly, but many are caught totally off
guard and their anxiety shows in their performance on the rest of the test. Practice until you are confident!
 You must be able to identify the various reaction types with ease.
 Be adept at naming and writing formulas for any ionic compounds.
 You must have your first two solubility rules memorized.
o
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Know that all solid ionic compounds are NOT written as ions.
 An “insoluble” or “slightly soluble” ionic compound formed in solution
 An ionic reactant that starts as a solid
o Know that aqueous ionic compounds are written as ions.
 “Solutions” of means the compound is dissolved.
 An ionic compound that is soluble and is formed in solution is also dissolved.
You must have the six strong acids memorized (or 8 as shown on neon orange sheet)
o Be sure you know how to name and write the formulas for all acids (strong or weak).
o Know that strong acids are written as ions.
o Know that weak acids are written as molecules.
Know and recognize reactions that form gases in solution.
You must know your descriptive chemistry (colors of ions/solids/solutions/gases). Emphasis will be placed on
actual colors/evidence of reactions you have witnessed in lab, but others will be assessed as well.
Recognize common oxidizing and reducing agents.
Be able to predict products of redox reactions.
PRACTICE UNTIL YOU’RE CONFIDENT. If 4.1 equations or PS 4.4 did not go well and it took you a long time to
complete, then you need to practice more. Remember you have the thick packet of practice reactions with
all the answers. You can also use your previous assignment to practice again.
Naming/Formula Writing:
1. KMnO4
2. Na2CO3
3. KOH
4. HC2H3O2
5. HClO
6. HIO3
7. Li3PO4
8. SnCl2
9.
10.
11.
12.
13.
14.
15.
16.
Fe2O3
NH4OH
HNO2
H2S
Lithium chlorate
Manganese (II) oxide
Oxalic acid
Calcium perbromate
17.
18.
19.
20.
21.
22.
23.
24.
Copper (II) nitrate
Aluminum sulfate
Barium chloride
Potassium dichromate
Sodium nitrite
Nickel (II) hydroxide
Beryllium sulfide
Ammonium sulfite
Ch. 4 Review of Reactions
Precipitation – usually two solutions of ionic compounds mixed (you should be able to do all of these WITHOUT
solubility rules – the first two need to be memorized).
1) Solutions of barium nitrate and potassium sulfate are mixed forming a precipitate.
2) Solutions of magnesium chloride and ammonium carbonate are mixed forming a precipitate.
3) Solutions of silver nitrate and copper (II) chloride are mixed forming a precipitate.
4) Solutions of barium hydroxide and cobalt (II) nitrate are mixed forming a precipitate.
Acid-Base – An acid mixed with a base (for now the base must be a metal hydroxide or ammonia).
Note: Strong acids ionize completely and thus are written as ions in solution. Weak acids ionize only partial
thus most remain as molecules and thus should be written as molecules. Bases that are metal hydroxides are ionic
and thus dissociate in solution completely when dissolved. Thus they should be written as ions if in solution, but
should be written together if they are solids.
Practice naming acids:
a) Hypochlorous acid
b) Chloric acid
c) Hydrochloric acid
d) Acetic acid
e) Hydrosulfuric acid
1)
2)
3)
4)
f)
g)
h)
i)
j)
Sulfuric acid
Hydrofluoric acid
Phosphoric acid
Nitrous acid
Periodic acid
Solutions of hydroiodic acid and barium hydroxide are mixed.
100 mL of 0.100 M hypochlorous acid and 100 mL of 0.200 M calcium hydroxide are mixed.
Solid beryllium hydroxide is dropped into a solution of nitric acid.
Solutions of chlorous acid and lithium hydroxide are mixed.
Redox – These could be simple redox (synthesis, decomposition, single replacement) or could involve oxyanions such
as permanganate ions or dichromate ions.
Synthesis
1) Sodium metal is placed into liquid bromine.
2) A piece of magnesium ribbon is burned in air.
3) Chlorine gas is passed over iron metal.
Decomposition (see pink molecular reactions WS or yellow CRAPO sheet).
1) Molten lithium chloride is electrolyzed.
2) Potassium chlorate is heated strongly.
3) Magnesium carbonate is heated strongly.
4) Calcium hydroxide pellets are heated strongly.
Single-replacement:
1) Sodium metal is dropped into distilled water.
2) A piece of magnesium ribbon is dropped into a solution of hydrobromic acid.
3) A piece of copper wire is placed in a solution of silver nitrate.
4) A piece of aluminum foil is placed in a solution of copper (II) chloride.
5) Fluorine gas is bubbled through a solution of sodium bromide.
Oxyanions:
1) An acidified solution of potassium permanganate is mixed with a solution of tin (II) nitrate.
2) Chlorine gas is bubbled through a dilute solution of sodium hydroxide (forming chloride ions and
hypochlorite ions).
3) An acidified solution of sodium dichromate is mixed with a solution of copper (I) chloride.
4) An acidified solution of potassium permanganate is mixed with a solution of potassium nitrite.
Gas formation
1) Solutions of ammonium nitrate and calcium hydroxide are mixed.
2) A solution of lithium carbonate is mixed with hydrochloric acid.
3) A piece of limestone (calcium carbonate) is dropped into a solution of perchloric acid.
4) A solution of potassium sulfide is mixed with a solution of nitric acid.
5) A solution of rubidium sulfite is mixed with a solution of hydroiodic acid.
Combination Reactions (not redox); see pink molecular reactions WS
1) Solid barium oxide is placed in distilled water.
2) Carbon dioxide gas is bubbled through distilled water.
3) Sodium oxide powder is mixed with sulfur dioxide gas.
4) Dinitrogen pentoxide is bubbled through distilled water.
Mixed Review: Identify Reaction Type, then write the net ionic equation:
Reaction Type
Net Ionic Equation
1.
Solutions of sodium hydroxide and nickel (II) nitrate are mixed.
2. Calcium carbonate chips are dropped into a solution of perchloric acid.
3. Solid magnesium hydroxide is added to a solution of nitrous acid.
4. Solutions of potassium iodide and silver nitrate are mixed, making a precipitate.
5. A piece of magnesium ribbon is placed in a solution of hydrochloric acid.
6. A solution of magnesium carbonate is added to a solution of hydrobromic acid.
7. Lithium oxide powder is added to distilled water.
8. Dinitrogen trioxide gas is bubbled through water.
9. Lithium oxide powder is added to dinitrogen trioxide.
10. An acidified solution of potassium permanganate is added to a solution of tin (II) chloride.
11. Calcium shavings are added to an acidified solution of sodium dichromate.
12. A solution of potassium permanganate is mixed with a basic solution of iron (II) chloride.