Tuesday, May 17

Section 4: Answer the questions below and study for your solutions quiz.

1) If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the molarity of the diluted solution be?

2) If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will the molarity of the diluted solution be?

3) How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?

4) I have 345 mL of a 1.5 M NaCl solution. If I boil the water until the volume of the solution is 250 mL, what will the molarity of the solution be?

5) How much water would I need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution?

Monday, May 16

Sections 2H & 5: Answer the following questions in your notebook.

Molarity = moles of solute/L of solution

1. What does molarity mean?

2. What is the molarity of a solution that contains 4.53 moles of lithium nitrate in 2.85 liters of solution?

3. What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in 2.39 x 10-2 liters of solution?

4. A flask contains 85.5 g C₁₂H₂₂O₁₁ (sucrose) in 1.00 liters of solution. What is the molarity?

5. A beaker contains 214.2 grams osmium (III) fluoride in 0.0673 liters of solution. What is the molarity?

6. Calculate the molarity if a flask contains 1.54 moles potassium sulfate in 125 ml of solution.

7. A chalice contains 36.45 grams ammonium chlorite in 2.36 liters of solution - calculate the molarity.

**** SOLUTIONS QUIZ ALERT:

Section 4 - Wednesday

Sections 2H & 5 - Thursday

Thursday, May 12

Section 2H: If you were not in class today, you must stop by tomorrow during CP for a few minutes to collect your chromatography lab data. You will complete the lab over the weekend. 

Section 4: Finish your lab and answer the following questions in your notebook. You should use the equation we used at the end of class (also, never forget about your textbook - we're in chapter 12!):

Molarity = moles of solute/L of solution 

1.      What does molarity mean? 

2.      What is the molarity of a solution that contains 4.53 moles of lithium nitrate in 2.85 liters of solution?

3.      What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in 2.39 x 10^-2 liters of solution?

4.      A flask contains 85.5 g C₁₂H₂₂O₁₁ (sucrose) in 1.00 liters of solution.  What is the molarity?

5.      A beaker contains 214.2 grams osmium (III) fluoride in 0.0673 liters of solution.  What is the molarity?

6.      Calculate the molarity if a flask contains 1.54 moles potassium sulfate in 125 ml of solution.

7.      A chalice contains 36.45 grams ammonium chlorite in 2.36 liters of solution - calculate the molarity.

Wednesday, May 11

Sections 5: Use the Salts & Solubility phet simulation (link found here) to complete the FIRST PAGE ONLY of the worksheet posted under homework docs.

Also, answer the following two questions in your notebook:

1) On the solubility curve, for most substances, as temperature increases, solubility increases. Why do you think this happens?

2) Two of the curves trend in the opposite direction, these substances are gases. Why do you think gas solubility decreases when temperature increases?

Tuesday, May 10

Sections 2H & 4: Use the Salts & Solubility phet simulation (link found here) to complete the FIRST PAGE ONLY of the worksheet posted under homework docs.