AP Reactions WS 5
Name ______________________________________________
For the following reactions write a net ionic equation. Box your final answer.
Example: A strip of magnesium is added to a solution of silver nitrate
Mg + 2 Ag+ → Mg2+ + 2 Ag
1.
Sodium Sulfite is added to water.
a.
2.
Potassium dichromate is added to lead(II) nitrate in an acidic solution.
a.
3.
What are the two Bronsted-Lowry bases in this reaction?
Solid lithium oxide is added to water.
a.
9.
What are the spectator ions in this reaction?
Solutions of carbon dioxide and ammonia are mixed.
a.
8.
What would you expect the pH of the products to be, less than 7, near 7, or greater than 7? Explain.
Hydrogen chloride gas is bubbled through water.
a.
7.
Is this a redox reaction? Explain.
Solutions of acetic acid and sodium carbonate are mixed.
a.
6.
What indication of a chemical reaction would you see as this reaction proceeds?
Hydrogen sulfide gas is bubbled through a solution of cadmium nitrate.
a.
5.
How does chromium’s oxidation number change in this reaction?
Calcium carbonate chips are added to excess nitric acid.
a.
4.
Which reactant is the Bronsted-Lowry acid and which is the Bronsted-Lowry base?
What would be the color if phenolphthalein is added to the products?
Powdered iron is added to a solution of iron(III) sulfate.
a.
How does iron change oxidation number in this reaction?
10. A mixture of solid calcium oxide and solid tetraphosphorous decaoxide is heated.
a.
What is the oxidation number of phosphorus before and after this reaction?
11. Molten magnesium chloride is electrolyzed between platinum electrodes.
a.
Why is it important that the electrodes are platinum?
12. Solid sodium cyanide is added to water.
a.
What are the spectator ions?
13. Gaseous boron hydride is mixed with ammonia gas.
a.
Identify the Lewis acid and base?
14. Gaseous silane (SiH4) is burned in excess oxygen.
a.
Which elements undergo a change in oxidation numbers? What is that change?
15. Magnesium ribbon is burned in pure nitrogen.
a.
How many liters of nitrogen at STP would be needed to make one mole of the product?
16. Hydrogen peroxide is added to an acidified solution of potassium iodide.
a.
Is the iodine oxidized or reduced? Explain.
17. Potassium permanganate is added to an acidified solution of oxalic acid.
a.
What would be one observation that would indicate this chemical reaction occurs?
18. Tin(II) acetate is added to an acidified solution of Potassium dichromate.
a.
Explain how both metals can end up oxidized in this reaction.
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SO32- + H2O  HSO3- + OHH+ + Pb2+ + Cr2O72-  Cr3+ + Pb4+ + H2O
CaCO3 + H+  Ca2+ + CO2 + H2O
H2S + Cd2+  CdS + H+
CH3COOH + CO32-  CH3COO- + CO2 + H2O
HCl + H2O  H3O+ + ClH2CO3 + NH3  NH4+ + HCO3- (CO32-)
Li2O + H2O  Li+ + OHFe + Fe3+  Fe2+
CaO + P4O10  Ca3(PO4)2 or Ca3(PO3)2
Mg2+ + Cl-  Mg + Cl2
NaCN + H2O  HCN + OH- + Na+
BH3 + NH3  BH3NH3
SiH4 + O2  SiO2 + H2O
Mg + N2  Mg3N2
H+ + H2O2 + I-  H2O + I2
H+ + MnO4- + H2C2O4  Mn2+ + CO2 + H2O
H+ + Sn2+ + Cr2O72-  Sn4+ + Cr3+ + H2O