1. The compound silver fluoride is a strong electrolyte. Write the reaction when
ID: 501391 • Letter: 1
Question
1. The compound silver fluoride is a strong electrolyte. Write the reaction when solid silver fluoride is put into water:
2. The compound potassium carbonate is a strong electrolyte. Write the reaction when solid potassium carbonate is put into water:
3. In the laboratory you dissolve 24.5 g of ammonium chloride in a volumetric flask and add water to a total volume of 500 mL.
What is the molarity of the solution? ______ M.
What is the concentration of the ammonium cation? _____ M.
What is the concentration of the chloride anion? _____ M.
4. In the laboratory you dissolve 23.5 g of iron(II) sulfate in a volumetric flask and add water to a total volume of 375 mL.
What is the molarity of the solution? ______ M.
What is the concentration of the iron(II) cation? ______ M.
What is the concentration of the sulfate anion? ______ M.
5. In the laboratory, a student dilutes 19.5 mL of a 8.24 M nitric acid solution to a total volume of 200.0 mL. What is the concentration of the diluted solution?
________M
6. How many milliliters of 9.40 M hydroiodic acid solution should be used to prepare 4.00 L of 0.700 M HI?
_______mL
7. In the laboratory you dilute 4.56 mL of a concentrated 6.00 M nitric acid solution to a total volume of 175 mL. What is the concentration of the dilute solution?
________ M
8. You wish to make a 0.280 M nitric acid solution from a stock solution of 3.00 M nitric acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution?
________mL
9. In the laboratory a student combines 24.7 mL of a 0.360 M magnesium iodide solution with 16.0 mL of a 0.661 M potassium iodide solution.
What is the final concentration of iodide anion ?
_________ M
10. In the laboratory a student combines 48.1 mL of a 0.428 M potassium hydroxide solution with 23.4 mL of a 0.489 M potassium bromide solution.
What is the final concentration of potassium cation ?
_______M
11. Write the net ionic equation for the following molecular equation.
(Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.)
12. Write the net ionic equation for the following molecular equation.
(Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.)
HNO3 is a strong electrolyte. HClO is a weak electrolyte.
Use H+ for the hydronium ion.
13. When aqueous solutions of ammonium phosphate and copper(II) nitrate are combined, solid copper(II) phosphate and a solution of ammonium nitrate are formed. The net ionic equation for this reaction is:
(Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.)
14. When aqueous solutions of potassium hypochlorite and nitric acid are mixed, an aqueous solution of potassium nitrate and hypochlorous acid results. Write the net ionic equation for the reaction.
(Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.)
Use H+ for the hydronium ion
15. Write a net ionic equation to show that nitric acid, HNO3, behaves as an acid in water.
16. Write a net ionic equation to show that hydrofluoric acid , HF , behaves as an acid in water.
17. Write a net ionic equation to show why solid barium hydroxide, Ba(OH)2 (s), forms a basic solution when it dissolves in water.
18. The substance triethanolamine is a weak nitrogenous base like ammonia.
Write a net ionic equation to show how triethanolamine, C6H15O3N, behaves as a base in water.
19. Write a net ionic equation for the reaction that occurs when aqueous solutions of barium hydroxide and nitric acid are combined. (Use H+ instead of H3O+.)
20. Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrocyanic acid and potassium hydroxide are combined.
21. Write a net ionic equation for the reaction that occurs when aqueous solutions of ammoniaand hypochlorous acid are combined.
22. Write a net ionic equation for the reaction that occurs when aqueous solutions of hydroiodic acid and ammonia are combined.
23. What volume of a 0.115 M barium hydroxide solution is required to neutralize 23.0 mL of a 0.371 M nitric acid solution?
24. What volume of a 0.242 M nitric acid solution is required to neutralize 26.4 mL of a 0.194M calcium hydroxide solution?
25. An aqueous solution of barium hydroxide is standardized by titration with a 0.115 M solution of nitric acid.
If 23.0 mL of base are required to neutralize 28.1 mL of the acid, what is the molarity of thebarium hydroxide solution?
26. An aqueous solution of nitric acid is standardized by titration with a 0.194 M solution ofcalcium hydroxide.
If 26.4 mL of base are required to neutralize 19.5 mL of the acid, what is the molarity of thenitric acid solution?
27. Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP.
How many grams of KHP are needed to exactly neutralize 22.1 mL of a 0.449 M barium hydroxide solution ?
28. Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP.
What volume of a 0.350 M barium hydroxide solution is needed to exactly neutralize 3.91grams of KHP ?
29. A student is asked to standardize a solution of potassium hydroxide. He weighs out 0.939 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid).
It requires 32.5 mL of potassium hydroxide to reach the endpoint.
A. What is the molarity of the potassium hydroxide solution? ______ M
This potassium hydroxide solution is then used to titrate an unknown solution ofhydroiodic acid.
B. If 20.2 mL of the potassium hydroxide solution is required to neutralize 16.0 mL ofhydroiodic acid, what is the molarity of the hydroiodic acid solution? ______ M
30. A student is asked to standardize a solution of sodium hydroxide. He weighs out 0.939 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid).
It requires 27.5 mL of sodium hydroxide to reach the endpoint.
A. What is the molarity of the sodium hydroxide solution? ______ M
This sodium hydroxide solution is then used to titrate an unknown solution of hydrobromic acid.
B. If 14.7 mL of the sodium hydroxide solution is required to neutralize 23.4 mL ofhydrobromic acid, what is the molarity of the hydrobromic acid solution? _______ M
Explanation / Answer
1)
AgF when put in water will dissociate into Ag+ and F-
AgF(S) <——> Ag+ (aq) + F- (aq)
2)
K2CO3 (s) <———> 2K+ (aq) + CO32- (aq)
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