5.3.1
Upcoming SlideShare
Loading in...5
×
 

5.3.1

on

  • 410 views

 

Statistics

Views

Total Views
410
Views on SlideShare
409
Embed Views
1

Actions

Likes
0
Downloads
8
Comments
0

1 Embed 1

https://jujo00obo2o234ungd3t8qjfcjrs3o6k-a-sites-opensocial.googleusercontent.com 1

Accessibility

Categories

Upload Details

Uploaded via as Microsoft PowerPoint

Usage Rights

© All Rights Reserved

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Processing…
Post Comment
Edit your comment

5.3.1 5.3.1 Presentation Transcript

  • Concentration
  • Concentration/Molarity/Molar Concentration
    • A measure of the amount of solute that is dissolved in a measured amount of solvent.
    • Dilute: a solution that contains a small amount of solute .
    • Concentrated: a solution that contains a large amount of solute.
  • Percent solutions
    • Percent means parts per one hundred.
    percent by volume = volume of solute volume of solution X 100 percent by mass = mass of solute volume of solution X 100 grams of solute dissolved in 100 mL solution
  • Examples
    • 10.0 mL of acetic acid is diluted to a total volume of 200 mL. What is the percent by volume of acetic acid?
    = = 5.00 % (v/v) % (v/v ) = volume of solute volume of solution X 100 0.010 L 0.200 L X 100
  • Parts per million
    • Very dilute concentrations can be recorded as parts per million. (ppm)
    • One ppm can be thought of as one drop in a bathtub of water.
    • 1 ppm = 1 mg/L
  • Examples
    • What mass of chlorine is present in 15.0 L of solution, if the solution is 6.00 ppm of chlorine?
    • 1 ppm = 1 mg/L
    • 6 ppm = 6 mg/L
    6 mg 15.0 L = 1 L x x = (6 mg) (15.0 L) 1 L = 90.0 mg
  • Examples
    • The label on a bottle of sparkling water lists the dissolved minerals as 440 ppm. What mass of minerals is present in a 200 ml glass of water?
    • 1 ppm = 1 mg/L
    • 440 ppm = 440 mg/L
    440 mg 0.200 L = 1 L x x = (440 mg) (0.200 L) 1 L = 88.0 mg
  • Concentration
    • concentration = # of mol of solute (mol)
    • # of litres of solution (L)
    • c = n
    • V
    • Units  mol/L or M
  • Examples
    • What is the concentration of a solution if 5.6 mol of NaCl are dissolved in 20.8 L of water?
    WS 20/5 - 1 c = 0.27 M c = n V c = 5.6 mol 20.8 L
  • Homework
    • Practice
    • P.205 # 1 – 6
    • P. 208 # 7 – 12
    • P. 210 # 13 - 16
  • Calculating ionic Concentrations
    • In solution electrolytic compounds exist as free, separate ions.
    • NaCl (aq) really means Na + (aq) and Cl - (aq)
    • In chemical reactions involving such a solution the ions react independantly.
  • Calculating ionic Concentrations
    • To calculate the ionic concentration of ions in solution:
      • Step 1: write a balanced dissociation equation
      • Step2: use a mole ratio from the equation to determine the ion concentration
  • Calculating ionic Concentrations
    • What is the concentration of each ion in 0.23 M Al 2 (SO 4 ) 3 solution?
    • Balanced dissociation eqaution:
      • Al 2 (SO 4 ) 3(s) -> 2 Al 3+ (aq) + 3 SO 4 2- (aq)
    • Use mole ratio:
    0.23 M Al2(SO4)3 1 mol Al2(SO4)3 2 mol Al 3+ = 0.46 M
  • Homework
    • Practice
    • P. 212 # 17 - 19
    • Section 5.3 Questions
    • P.214 # 1 – 17