1. The name of the acid HBrO is a. Bromite acid b. Hypobromous Acid c. Bromic Acid d. Hydrobromic Acid 2. The reaction between an alkali metal and

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1 1. The name of the acid HBrO is a. Bromite acid b. Hypobromous Acid c. Bromic Acid d. Hydrobromic Acid 2. The reaction between an alkali metal and water generally results in the formation of a. A metal hydroxide b. Hydrogen gas c. A and B d. Neither A nor B 3. A 6.00 mol sample of AgNO3 is mixd with 5.00 mol of Na3PO4 in water and solid Ag3PO4 forms as a precipitate. What is the maximum number of moles of silver phosphate that can form in this reaction? a mol b mol c mol d mol 4. Which of the following is a weak acid? a. HCl b. H2SO4 c. HNO3 d. None of the above 5. In which of the following species is the oxidation state of bromine +5? a. BrO4 - b. Br - c. BrO3 - d. BrCl 6. Which of the following elements is capable of having more than one oxidations state? a. O b. Sr c. F d. Na 7. In aqueous solution, acetic acid behaves as a. a strong electrolyte b. a weak electrolyte c. a nonelectrolyte d. a gas 8. Which of the following species is expected to be insoluble in water? a. KNO3 b. PbI2 c. LiBr d. NH4SO4 9. How many ml of a 4.00 M CaCl2 solution must be diluted with enough water to produce 1.00 L of a M CaCl2 solution? a ml b ml

2 c ml d ml 10. Provide the name or formula, as appropriate, for each of the following. a. HNO3 b. HF c. Chlorous acid d. Carbonic acid 11. In aqueous solutions do the following compounds behave as an electrolyte or nonelectrolyte? a. Mg(NO3)2 b. CH3CH2OH c. HCl 12. In redox reactions, why must at least one species be oxidized and at least one other species be reduced? In other words, why cannot a redox reaction include only one species that are oxidized or only species that are reduced?

3 13. If ml of a M solution of ammonium phosphate (NH4)3PO4, is added to 50.0 ml of a M solution or NiCL2, a precipitate forms. a. Determine which reactant is limiting and calculate the moles of precipitate formed. b. Which ions are spectator ions? Calculate the concentration of the positively charged spectator ion. c. Determine the concentration of the reactant ion present in excess after the reaction is completed.

4 14. For the balanced reaction below, determine the element oxidized and the element reduced. In the spaces provided, give the initial and final oxidation states for the elements oxidized and reduced. Finally, state the moles of electrons transferred in the balanced chemical equation. Element oxidized: Initial oxidation state: Final oxidation state: Element reduced: Initial oxidation state: Final oxidation state: Moles of electrons transferred in the balanced chemical equation above: 15. Use the solubility rules to complete and balance the following precipitation reactions. Indicate which product is the precipitate by writing (s). If no precipitate forms, write NR. a. _ Na 2 CO 3 (aq) + _ AgNO 3 (aq) b. _ NaNO 3 (aq) + _ NiSO 4 (aq) c. _ FeSO 4 (aq) + _ Pb(NO 3 ) 2 (aq) 16. Write the total ionic equations for the reactions in question 15. If no reaction occurred, list every ion present in solution. 17. Identify the spectator ions in question 16. If no reaction occurred, every ion is a spectator ion.

5 18. For each of the reactions given below: 1) predict the products and balance the chemical equations; 2) classify the reaction as acid-base, gas-evolution, or precipitation reaction. a. AgNo3 (aq) + Na2CrO4 (aq) b. H2SO4 (aq) + NaOH (aq) c. K2CO3 (aq) + HClO4 (aq) 19. Chlorine gas reacts with silica, SiO 2, and carbon to give silicon tetrachloride and carbon monoxide. a. Balance the following equation:cl 2 (g) + SiO 2 (s) + C (s) SiCl 4 (l) + CO (g) b. How much CO gas can be produced from 15.0 g of silica? c. If the percent yield was 78.4%, what was the actual yield of CO?

6 1. The name of the acid HBrO is a. Bromite acid b. Hypobromous Acid c. Bromic Acid d. Hydrobromic Acid 2. The reaction between an alkali metal and water generally results in the formation of a. A metal hydroxide b. Hydrogen gas c. A and B d. Neither A nor B 3. A 6.00 mol sample of AgNO3 is mixd with 5.00 mol of Na3PO4 in water and solid Ag3PO4 forms as a precipitate. What is the maximum number of moles of silver phosphate that can form in this reaction? a mol b mol c mol d mol 4. Which of the following is a weak acid? a. HCl b. H2SO4 c. HNO3 d. None of the above 5. In which of the following species is the oxidation state of bromine +5? a. BrO4 - b. Br - c. BrO3 - d. BrCl 6. Which of the following elements is capable of having more than one oxidations state? a. O b. Sr c. F d. Na 7. In aqueous solution, acetic acid behaves as a. a strong electrolyte b. a weak electrolyte c. a nonelectrolyte d. a gas 8. Which of the following species is expected to be insoluble in water? a. KNO3 b. PbI2 c. LiBr d. NH4SO4 9. How many ml of a 4.00 M CaCl2 solution must be diluted with enough water to produce 1.00 L of a M CaCl2 solution? a ml b ml

7 c ml d ml 10. Provide the name or formula, as appropriate, for each of the following. a. HNO3 Nitric Acid b. HF Hydrofluoric Acid c. Chlorous acid HClO2 d. Carbonic acid H2CO3 11. In aqueous solutions do the following compounds behave as an electrolyte or nonelectrolyte? a. Mg(NO3)2 Electrolyte b. CH3CH2OH Nonelectrolyte c. HCl Electrolyte 12. In redox reactions, why must at least one species be oxidized and at least one other species be reduced? In other words, why cannot a redox reaction include only one species that are oxidized or only species that are reduced? 13. If ml of a M solution of ammonium phosphate (NH4)3PO4, is added to 50.0 ml of a M solution or NiCL2, a precipitate forms. a. Determine which reactant is limiting and calculate the moles of precipitate formed. b. Which ions are spectator ions? Calculate the concentration of the positively charged spectator ion. c. Determine the concentration of the reactant ion present in excess after the reaction is completed.

8 14. For the balanced reaction below, determine the element oxidized and the element reduced. In the spaces provided, give the initial and final oxidation states for the elements oxidized and reduced. Finally, state the moles of electrons transferred in the balanced chemical equation. Element oxidized: Initial oxidation state: Final oxidation state:

9 Element reduced: Initial oxidation state: Final oxidation state: Moles of electrons transferred in the balanced chemical equation above: Use the solubility rules to complete and balance the following precipitation reactions. Indicate which product is the precipitate by writing (s). If no precipitate forms, write NR. a. _ Na 2 CO 3 (aq) + _ AgNO 3 (aq) b. _ NaNO 3 (aq) + _ NiSO 4 (aq) c. _ FeSO 4 (aq) + _ Pb(NO 3 ) 2 (aq) 16. Write the total ionic equations for the reactions in question 15. If no reaction occurred, list every ion present in solution.

10 17. Identify the spectator ions in question 16. If no reaction occurred, every ion is a spectator ion. 18. For each of the reactions given below: 1) predict the products and balance the chemical equations; 2) classify the reaction as acid-base, gas-evolution, or precipitation reaction. a. AgNo3 (aq) + Na2CrO4 (aq) b. H2SO4 (aq) + NaOH (aq) c. K2CO3 (aq) + HClO4 (aq) 19. Chlorine gas reacts with silica, SiO 2, and carbon to give silicon tetrachloride and carbon monoxide. a. Balance the following equation:cl 2 (g) + SiO 2 (s) + C (s) SiCl 4 (l) + CO (g) b. How much CO gas can be produced from 15.0 g of silica?

11 c. If the percent yield was 78.4%, what was the actual yield of CO?

Net Ionic Reactions. The reaction between strong acids and strong bases is one example:

Net Ionic Reactions. The reaction between strong acids and strong bases is one example: Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you