10
13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m NaCl

13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Embed Size (px)

Citation preview

Page 1: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

13.48 Calculate the number of moles of solute present in each of the following aqueous solutions:

(a) 185 mL of 1.50 M HNO3

(b) 50.0 mg that is 1.25 m NaCl

Page 2: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

13.31

(a) Explain why carbonated beverages must be stored in sealed containers.

(b) Once the beverage has been opened, why does it maintain more carbonation when refrigerated than at room temperature?

Page 3: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Henry’s Law Example

Calculate the concentration (solubility) of CO2 in a 2-liter that is bottled with a partial pressure of 4.0 atm @ 25 ºC. The constant for CO2 in water is 3.1 × 10-2

mol/L-atm

Page 4: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Henry’s Law Example

Calculate the concentration (solubility) of CO2 in a 2-liter that is bottled with a partial pressure of 4.0 atm @ 25 ºC. The constant for CO2 in water is 3.1 × 10-2 mol/L-atm

Sg = k Pg

Page 5: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Henry’s Law Example

Calculate the concentration (solubility) of CO2 in a 2-liter that is bottled with a partial pressure of 4.0 atm @ 25 ºC. The constant for CO2 in water is 3.1 × 10-2 mol/L-atm

Sg = k Pg

Sg = (3.1 × 10-2 mol/L-atm)(4.0 atm)

Page 6: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Henry’s Law Example

Calculate the concentration (solubility) of CO2 in a 2-liter that is bottled with a partial pressure of 4.0 atm @ 25 ºC. The constant for CO2 in water is 3.1 × 10-2 mol/L-atm

Sg = k Pg

Sg = (3.1 × 10-2 mol/L-atm)(4.0 atm)

Sg = 0.124 = 0.12 mol/L

Page 7: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Henry’s Law Example

Calculate the concentration (solubility) of CO2 in a 2-liter that is bottled with a partial pressure of 4.0 atm @ 25 ºC. The constant for CO2 in water is 3.1 × 10-2 mol/L-atm

Sg = k Pg

Sg = (3.1 × 10-2 mol/L-atm)(4.0 atm)

Sg = 0.124 = 0.12 mol/L

Concentration = 0.12 M

Page 8: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Complete the following thought questions on the example side of your notes:

1) As you increase temperature, solubility of a solid___________.

2) As you lower the temp, solubility of a gas ___________.

3) Solutions that form spontaneously are considered____________.

4) When more bonds form than break, the system (solution) ____________energy.

Page 9: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Determine the molality of glucose in the solution given the following information. 4.35 g glucose (C6H12O6) in 25.0 mL of water. Water has a density of 1.00 g/mL. (pg 544)

What is molality?

How do you get the units you need from the given data?

Page 10: 13.48 Calculate the number of moles of solute present in each of the following aqueous solutions: (a)185 mL of 1.50 M HNO 3 (b) 50.0 mg that is 1.25 m

Homework

13.39) Calculate the molarity for each of the following:

(a) 0.540 g Mg(NO3)2 in 250.0 mL of solution.

(b) 22.4 g LiClO4 • 3H2O in 125 mL of solution.