Solutions Worksheet #1 (Solutions, Electrolyte’s, and ...



Solutions Worksheet #1 (Classification of Matter, Types of Solutions)

1. Use solubility rules to determine which of the following will produce a precipitate?

(A) 3KBr(aq) + AlPO4(aq) → K3PO4 + AlBr3 (B) ZnCl2(aq) + MgSO4(aq) → ZnSO4 + MgCl2

(C) Na2CO3(aq) + CaCl2(aq) → CaCO3 + 2NaCl (D) NH4OH(aq) + KCl(aq) → KOH + NH4Cl

Which of the above will form a solution NOT a chemical reaction?_______________ Explain.

2. When the following chemicals are mixed together which will form a precipitate (reaction) and which will be a solution? Use solubility rules!

(A) CaBr2(aq) + NaNO3(aq) (B) Ag2CO3(aq) + Li2SO4(aq)

Classification of Matter: Determine if the following is an element, compound, solution, or heterogeneous mixture.

3. liquid mercury_______________________ 8. sodium chloride_______________________________

4. air_____________________________ 9. bread_________________________________

5. brass_____________________________ 10. Kool-Aid___________________________________

6. salt water_____________________________ 11. water______________________________________

7. iodine vapors________________________ 12. dry ice_____________________________________

Making a Solution (Like Dissolves Like): Which type of solvent would be used (polar or nonpolar) to dissolve the following solutes?

11. CH3Cl_______________________________ 19. magnesium phosphate___________________

12. hydrogen sulfide_______________________ 20. CH3OH______________________________

13. C2H6________________________________ 21. ammonia______________________________

14. strontium nitrate________________________ 22. hydrogen bromide_______________________

15. sulfur dioxide___________________________ 23. phosphorus trihydrogen___________________

16. CH3Br________________________________ 24. silicon tetrabromide_______________________

17. NaCl_________________________________ 25. phosphorus trichloride_____________________

18. FeCl3_________________________________ 26. sodium nitrate_____________________________

Types of Solutions (Electrolytes): Tell whether each of the following aqueous solutions would be a STRONG, WEAK, or NON-Electrolyte.

27. Al2(SO4)3___________ 33. HMnO4_________________ 39. C6H12O6____________

28. Cu(OH)2________________ 34. Sr(OH)2_____________ 40. H2CrO4______________

29. SO2 (l)__________________ 35. HClO2 _______________ 41. Fe(NO3)3________________

30. C12H22O11___________ 36. HNO3___________________ 42. H2C2O4______________

31. H2Se_________________ 37. CsOH___________________ 43. CH4 (l)__________________

32. HI____________________ 38. Be(OH)2________________

Solutions Worksheet #2

(Molarity, Dilutions, Percent Solutions, Molality Problems)

Molarity

1. Tell how you would prepare a 500. mL of 0.50 M ammonium carbonate solution. Include all necessary equipment and amount of chemical (in grams).

2. What is the molarity of each of the following solutions?

a. 40.0 grams of sodium hydroxide in 1.50 L of solution

b. 4.10 grams of magnesium chloride in 300. mL of solution

3. If 0.885 moles of copper (II) sulfate are dissolved in enough water to make 70.0 mL of solution, what is the molarity of the solution?

4. What is the molarity of a 400. mL solution in which 3.70 moles of sodium acetate are dissolved?

5. How many grams of calcium nitrate are needed to make 3.30 L of a 0.10 M solution?

Molarity of Ions in Solution

6. Calculate the molarity of the ions in the following solutions:

a. 0.917M aluminum sulfate

b. 1.25M aluminum chloride

Dilutions

7. If 30.0 mL of 12.0 M HCl stock solution are diluted to a volume of 500. mL, what is the molarity of the dilute solution?

8. If 27.5 mL of 16.0 M nitric acid stock solution is added to 300. mL of water, what is the molarity of the diluted solution? (V1 will be 27.5 mL. But for V2 don’t forget to add the volume of the water and the nitric acid to get the total V2 volume.)

9. If 50.0 mL of a stock sulfuric acid solution whose molarity is 15.0 M is diluted until the molarity of the new solution is 2.50 M, what is the volume of the new solution?

Molality

10. How many grams of water must be added to 455 grams of potassium sulfate in order to make a 1.50 m solution?

11. If 300. grams of magnesium acetate are added to 5000. grams of water, what is the molality of the solution?

12. How many grams of lithium nitrate are required to add to 800. grams of water in order to prepare a 2.00 m solution?

Percent Solutions

13. If 40.0 grams of ammonium hydroxide are added to 200. mL of water, what is the percent by mass of this solution?

14. An alcohol-water solution is by volume 40.0% isopropyl alcohol. There are 500. mL of the solution. How many mL of alcohol were added to water when preparing the solution?

15. If 35.0 mL of ethanol, C2H5OH, were added to 65.0 mL of water, what is the percent by volume of the solution?

Solutions Worksheet #3 (Colligative Properties)

FPD and BPE

1. Determine the number of particles the following solutions become? If you do not know the formula for the chemical, use the internet or a textbook to look it up.

a. sucrose (sugar) b. C9Hl0O2 c. an organic compound

d. sodium chloride e. glucose f. aluminum sulfate

Of the following which ones will cause the BPE or FPD to change the most? Why?

a. sucrose (sugar) b. C9Hl0O2 c. an organic compound

d. sodium chloride e. glucose f. aluminum sulfate

|Solvent |Boiling Point (°C) |Kb (° C/m) |Freezing Point ( °C) |Kf (°C/m) |

|Water |100 |0.5l2 |0 |l.86 |

|Benzene |80.l |2.53 |5.48 |5.12 |

|Acetic Acid |118.l |3.07 |16.6 |3.90 |

|Nitrobenzene |210.88 |5.24 |5.70 |7.00 |

|Phenol |182 |3.56 |43 |7.40 |

2. What is the freezing point of a solution that contains 6.50 moles of sucrose, C12H22O11, dissolved in l.00 kg of water?

3. What is the boiling point of a solution that consists of 989 g of sucrose in 1500. grams of water?

4. What is the freezing point of a solution that contains 4.50 grams of C9Hl0O2 dissolved in 50.0 g of benzene?

5. Forty grams of an organic compound dissolved in l.00 kg of water have a boiling point of l00.52°C. What is the molar mass of the solute?

6. 35.0 grams of an organic compound dissolved in 500. g of water has a freezing point of -3.72°C. What is the molar mass of the solute?

7. An organic compound with a molar mass of l40. g/mole is dissolved in l000. grams of nitrobenzene. The freezing point of the solution is 4.75°C. How many grams of the compound were dissolved in nitrobenzene?

8. What is the freezing point of 67.3 grams of sodium chloride dissolved in 755 grams of acetic acid?

9. What is the boiling point of l4.0 grams of glucose, C6H12O6, dissolved in 250. g of phenol?

10. How many grams of aluminum sulfate need to be dissolved in l500. grams of acetic acid in order to raise the boiling point by 4.3°C?

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