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 (polar)______19. magnesium phosphate (ionic) ______
12. hydrogen sulfide (polar)______20. CH3OH (polar) ______
13. C2H6(nonpolar)______21. Ammonia (polar) ______
14. strontium nitrate (ionic)______22. hydrogen bromide (polar) ______
15. sulfur dioxide (polar) ______23. phosphorus trihydrogen (polar) ______
16. CH3Br (polar)______24. silicon tetrabromide (nonpolar) ______
17. NaCl (ionic)______25. phosphorus trichloride (polar) ______
18. FeCl3(ionic)______26. sodium nitrate (ionic) ______
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 and DilutionsProblems)
Molarity
- Tell how you would prepare a 0.5L of 0.50 M ammonium carbonate solution. Include all necessary equipment and amount of chemical (in grams).
- What is the molarity of each of the following solutions?
- 40.0 grams of sodium hydroxide in 1.50 L of solution
- 4.10 grams of magnesium chloride in 0.30L of solution
- If 0.885 moles of copper (II) sulfate are dissolved in enough water to make 0.070 L of solution, what is the molarity of the solution?
- What is the molarity of a 0.40L solution in which 3.70 moles of sodium acetate are dissolved?
- How many grams of calcium nitrate are needed to make 3.30 L of a 0.10 M solution?
Dilutions
- 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?
- If 27.5mL of 16.0 M nitric acid stock solution is added to water to make a 327.5mL solution, what is the molarity of the diluted solution?
- 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?
Solutions Worksheet #3 (Colligative Properties)
Solvent / Boiling Point (°C) / Freezing Point (°C)Water / 100 / 0
Benzene / 80.l / 5.48
Acetic Acid / 118.l / 16.6
Nitrobenzene / 210.88 / 5.70
Phenol / 182 / 43
2. What is the freezing point of a solution that contains sucrosedissolved in water with a FPD of 12.1°C?
3. What is the boiling point of a solution that consists ofsucrose in water with a BPE of 0.986°C?
4. What is the freezing point of a solution that contains C9Hl0O2 dissolved in benzene with a FPD of 3.07°C?
5. An organic compound dissolved in water has a boiling point ofl00.52°C. What is the BPE for this solution?
6. An organic compound dissolved in water has a freezing point of -3.72°C. What is FPD for this solution?
7. An organic compound is dissolved in nitrobenzene. The freezing point of the solution is 4.75°C. What is the FPD for this solution?
8. What is the freezing point of sodium chloridedissolved in acetic acid with a FPD of 11.9°C ?
9. What is the boiling point of glucosedissolved in phenol with a BPE of 1.11°C?
10. Aluminum sulfate is dissolved in acetic acid. The boiling point of the solution is 122.4°C. What is the BPE for this solution?
Classification of Matter and Solutions Test Review
Read over all sets of notes Know the definition of all terms that appear in the notes (solubility, electrolyte, solution…..)
Some answers are given in ( ).
1. Would the following substances dissolve in water? Why or why not? Be specific
a. Sodium phosphate (yes, ionic)d. sodium chloride (yes, ionic)
b. Mercurous perchlorate (yes, ionic)e. Iron (II) nitrate (yes, ionic)
c. CH4 (no, nonpolar)f. CH5OH (yes, polar)g. C6H6 (no, nonpolar)
2. Tell whether each of the following aqueous solutions would be a STRONG, WEAK, or NON-Electrolyte.
a. Al2(SO4)3 (strong, ionic) b. H2SO4 (strong, strong acid) c. C6H12O6(non, molecular)
3. Determine if the following is an element, compound, solution, or heterogeneous mixture.
a. gold(element)d. sodium acetate(compound)
b. 6.0 M hydrochloric acid(solution)e. oil and water (heterogeneous mixture or suspension)
c. milk (heterogeneous mixture or colloid)
4. If 0.37 grams of potassium hydroxide are added to enough water to make 0.020L of solution, what is its molarity?
5. When 153 grams of a soluble compound are added to enough water to make 0.575L of solution the molarity of the solution is known to be 2.50 M. What is the molar mass of the soluble compound?
7. Tell exactly how you would prepare 0.250L of a 1.5 M hydrochloric acid solution beginning with a stock hydrochloric acid solution that is 12.0 M.
8. If 30.0 mL of 12.0 M HCl stock solution is diluted to a volume of 500. mL, what is the molarity of the dilute solution?
15. What is the BPE of a solution of sodium chloride dissolved in acetic acid if the boiling point of the solution is 127.3°C?
16. When a non-ionizing compound is dissolved in phenolthe freezing point of the solution is 40.7°C. What is the FPD for this solution?
17. What is the FPD of a solution of C10H8dissolved in benzene if the freezing point of the solution is -21.0°C?
18. Define solubility:
19. What factor increasesthe solubility of solid solutes?
20. What factor increases the solubility of gaseous solutes? What factor decreases the solubility of gaseous solutes?
21. What factors increase the rate of dissolving of solid solutes?
22. What is the difference in saturated, unsaturated, and supersaturated solutions.
23. What is the difference between a solution, colloid, and a suspension. What technique can be used to determine if a substance is a solution, colloid, or a suspension?
24. Is making a solution a physical or chemical change? Why?
1. One reason water is an effective solvent is that it —
A contains an oxygen atomB is a polar molecule
C has a freezing point of 0°CD can evaporate easily
2. What characteristic of water remains the same no matter what is dissolved in it?
A The ratio of hydrogen to oxygenB The ability to refract light
C The hydroxide ion concentrationD The freezing temperature
3. Which factor makes water an effective solvent?
A The presence of molecular oxygen B Its lack of covalent bonds
C The polar nature of its molecules D Its abundance on Earth’s surface
4. As a scuba diver goes deeper underwater, the diver must be aware that the increased pressure affects the human body
by increasing the —
A body’s temperature B amount of dissolved gases in the body
C amount of suspended solids in the body D concentration of minerals in the body
5. A recipe calls for 210 grams of sugar to be dissolved in 0.25 liter of water. After the mixture is stirred, some sugar crystals remain in the water. What can be added to the mixture to help dissolve the remaining sugar crystals?
A Thermal energyB 2.0 g of baking soda
C Ice cubesD 2.0 g of sodium chloride