strong electrolytes/net ionic equation help please

Feb 17th, 2015
DotaCN
Category:
Chemistry
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Question description


1. The compound cobalt(II) bromide is a strong electrolyte. Write the reaction when cobalt(II) bromide is put into water:

2. The compound calcium nitrite is a strong electrolyte. Write the reaction when calcium nitrite is put into water:

3. When aqueous solutions of aluminum sulfate and ammonium carbonate are combined, solid aluminum carbonate and a solution of ammonium sulfate are formed. The net ionic equation for this reaction is:

4.When solid Fe metal is put into an aqueous solution of SnSO4, solid Sn metal and a solution of FeSO4 result. Write the net ionic equation for the reaction.

5.Write the net ionic equation for the precipitation of lead iodide from aqueous solution:

6. Consider the reaction when aqueous solutions of ammonium bromide and copper(II) acetate are combined. The net ionic equation for this reaction is:

7. Consider the reaction when aqueous solutions of magnesium acetate and chromium(III) chloride are combined. The net ionic equation for this reaction is:

8. Consider the reaction when aqueous solutions of copper(II) sulfate and iron(III) acetate are combined. The net ionic equation for this reaction is:

9. Consider the reaction when aqueous solutions of lead(II) acetate and potassium sulfate are combined. The net ionic equation for this reaction is:

10. Consider the reaction when aqueous solutions of potassium hydroxide and barium acetate are combined. The net ionic equation for this reaction is:

11. Consider the reaction when aqueous solutions of iron(III) sulfate and sodium hydroxide are combined. The net ionic equation for this reaction is:

12. Consider the reaction when aqueous solutions of ammonium phosphate and potassium bromide are combined. The net ionic equation for this reaction is:

13. Consider the reaction when aqueous solutions of lead(II) acetate and sodium phosphate are combined. The net ionic equation for this reaction is:

14. Consider the reaction when aqueous solutions of ammonium sulfide and iron(III) iodide are combined. The net ionic equation for this reaction is:

15. Consider the reaction when aqueous solutions of potassium acetate and sodium sulfide are combined. The net ionic equation for this reaction is:

16. Consider the reaction when aqueous solutions of ammonium carbonate and potassium acetate are combined. The net ionic equation for this reaction is:

17. Consider the reaction when aqueous solutions of iron(II) acetate and chromium(III) sulfate are combined. The net ionic equation for this reaction is:

18. Write a net ionic equation to show that hydrobromic acid, HBr, behaves as an acid in water

19. Write a net ionic equation to show that carbonic acid, H2CO3, behaves as an acid in water. Consider only its first ionization.

20. You wish to make a 0.261 M hydrobromic acid solution from a stock solution of 6.00 M hydrobromic acid. How much concentrated acid must you add to obtain a total volume of 75.0 mL of the dilute solution?

21. A 0.4191 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9773 g.

What is the mass percentage of chlorine in the original compound?

22. A student determines the chromium(II) content of a solution by first precipitating it as chromium(II) hydroxide, and then decomposing the hydroxide to chromium(II) oxide by heating. How many grams of chromium(II) oxide should the student obtain if his solution contains 58.0 mL of 0.453 M chromium(II) nitrate?

23. An aqueous solution of calcium hydroxide is standardized by titration with a 0.196 M solution of perchloric acid.

If 29.8 mL of base are required to neutralize 26.1 mL of the acid, what is the molarity of the calcium hydroxide solution?

24. An aqueous solution of perchloric acid is standardized by titration with a 0.139 M solution of potassium hydroxide.

If 11.8 mL of base are required to neutralize 24.8 mL of the acid, what is the molarity of the perchloric acid solution?

25. In the laboratory, a student adds 45.0 mL of water to 24.8 mL of a 0.666 M perchloric acid solution. What is the concentration of the diluted solution ?



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