Agenda for Thursday 3.22.18

Read
  Chapter 16.7, pp 524-527
Do
  Problem 44, pg 534, and the titration problem below:

You have a large flask full of NaOH, which you’d like to use for titrant.  You think it’s close to .1 M, but you’re not really sure.  Fortunately, you have a small amount of pure benzoic acid, so you plan to do a titration.  You weigh a small, precise amount of this monoprotic acid into a flask, and dissolve it in approximately 20 mL of distilled water. 
Here’s what you need to know:

• molar mass of benzoic acid: 122.12 g/mol
• mass of benzoic acid: 0.230 g
• mL of NaOH titrated: 18.55 mL

What is the molarity of NaOH? (precise)

PowerPoint for Fishy#1

Tomorrow

• Fishy Quiz #2
• Quickie 10-point pH/pOH calculation quiz

Homework due 3.21.18

Read
  Chapter 16.5, 16.6. , pp 521 - 524
Do
  Problems 38, 39, 41, 42bd pg 534

Homework due 3.20.18

Read

  Chapter 16.4 pp 513 - 520
Do
  Problems 28, 29, 30, 31b, 31d, 32b, 32d, 34b, 35b, 36b

The ideal pH for discus is around 6.5

Click here to download/view Study Guide for Chapter 16

Homework due 3.19.18

Read
  Chapter 16.3, pp 510-513
Do
  Problems 21, 22bd, 23bd, 24bc, 25bc

Homework/Agenda for Friday, 3.16.18

Read
  Chapter 16.2, pp 506 - 510
Do
  Problems 13, 15, 16

Ice Cream Lab!
If you don't bring in your supplies, you may not get any ice cream!

Homework/Agenda for Thursday 3.15.18

Chapter 15 Homework Harvest 

Do Chapter 16 HW on new piece of paper!

Read

  Chapter 16.1, pp 503-506

Do

  Problems 3, 7bd, 8bc, 11bd, 12, bd

The Death of Caesar (1798) by Vincenzo Camuccini

Homework due 3.9.18

Henry's Law

Henry's law is one of the gas laws formulated by William Henry in 1803 and states: "At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid." An equivalent way of stating the law is that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid:

C=kPgas

where

• C is the solubility of a gas at a fixed temperature in a particular solvent (in units of M or mL gas/L)
• k is Henry's law constant (often in units of M/atm)
• Pgas is the partial pressure of the gas (often in units of atm)

---

Homework

Do

  Problems 53, 55, 57bd, 58bc

  [note: there are potentially good quiz questions in tonight's homework!]

homework due 3.8.18

Read
  Chapter 15.10, pp 495 - 496
Do
  Problems 50, 51, 59

Calculation of Freezing Point Depression

If the solution is treated as an ideal solution, the extent of freezing-point depression depends only on the solute concentration that can be estimated by a simple linear relationship with the cryoscopic constant ("Blagden's Law"):

ΔT_F = K_F · b · i,

where:

• ΔT_F, the freezing-point depression, is defined as T_{F (pure solvent)} − T_{F (solution)}.
• K_F, the cryoscopic constant, which is dependent on the properties of the solvent, not the solute. (Note: When conducting experiments, a higher K_F value makes it easier to observe larger drops in the freezing point. For water, K_F = 1.853 K·kg/mol.^[7])
• b is the molality (moles solute per kilogram of solvent)
• i is the van 't Hoff factor (number of ion particles per individual molecule of solute, e.g. i = 2 for NaCl, 3 for BaCl₂)

Homework for Wednesday 3.7.18

Read
  Chapter 15.8, 15.9, pp 488-495
Do
  Problems 39, 41bd, 44bc, 48, pg 501

note:  The topic of Normality is considered 'extra credit.'

Homework/Agenda for Tuesday 3.6.18

Homework Harvest on Tuesday for Chapters 13, 14

Read  
  Chapter 15.7, pp 485 - 488  
Do 
   Problems 35, 37, pg 500

Homework/Agenda for Monday 3.5.18

Read 
  Chapter 15.6, pp 481 - 485 
Do 
  Problems 31b, 32, 34, pg 500 

Homework Harvest on Tuesday for Chapters 13, 14