Equilibrium Unit Ch. 15 Sections 1-7, and Ch. 17 Sections 4-6
Monday
Tuesday
Wednesday
Thursday
NO SCHOOL
2/2
2/3
2/4
Final Reflection Ch. 15 Basics
PPT of Practice
Sect 1-6: Q, Kc, Kp, kf, kr
Problems
Hetero vs Homo
Hess’s Law (solve for K)
Sect 7 intro: Le Chatelier’s
Principle (only changes in mass
of reactants or products)
Friday
2/5
Ch. 15 Sect 5
Le Chatelier’s Principle:
Concentration
Pressures
Temperatures
How to Achieve a Desired
Outcome
2/11 NO SCHOOL
2/8
2/9
2/10
Notes on
PPT of Practice Go over HW;
TEST
Ch. 17 Sect 4-6
Problems
Students Ask Questions
Ch. 15, 17b
HW:
Preview to Ch. 15
Worksheet #1
Based on Wedn and Thurs:
Ch. 15 #1, 2, 4, 13, 15a, 17, 28, 29, 31, 33, 41, 45, 51, 53
Based on Friday:
Ch. 15 #7, 9, 12, 19, 61, 62, 68, 74, 84 (100 … good challenge)
Based on Monday and Tuesday Ch. 17 #51, 53, 59, 73, 74
Based on Friday-Tuesday
Worksheet #2
Learning Objectives (What you could be expected to do on the TEST)
Make observations in lab (or read description of observation)
Communicate the change via
- Symbols
- Particle views
- Skeleton equations
- Balanced molecular equations
- Total ionic equations
- Net ionic equations
Justify the choice of how the change was communicated
Based on how it can be utilized for the given circumstance.
Or translate from any one of those above to another.
Ch. 15
Explain what equilibrium is, and the origin of the equilibrium constant K
Law of Mass Action: reaction rate is proportional to the product of the masses of reactants
Equilibrium: when the rate of a forward reaction is equal to the rate of the reverse reaction.
At equilibrium, the product of masses ratio of reactants to products remains constant.
This ratio is now called the “equilibrium constant” (K)
Write the equilibrium expression for any chemical reaction.
Differentiate between the reaction quotient (Q) and the equilibrium constant (K).
Calculate Q or K given appropriate tabular or graphical data for a system.
Given K and current concentrations, calculate equilibrium concentrations.
Compare K and Q to predict
The relative rates of the forward and reverse reactions.
the direction a reaction will proceed toward equilibrium.
Explain why using the equilibrium expression (If Q > K, shift to reactants. Why?)
Based on the relative size of K, determine which chemical species will have relatively large or small concentrations at
equilibrium.
Use Le Chatelier’s Principle
Predict the direction a reaction that was at equilibrium will proceed after a “stress on the system”
Design a set of conditions that will optimize a desired result (more or less of any product or reactant)
“Stress on a system” = change in temp, conc, pressure of gas, etc.
Direction of reaction proceeds = shift to reactants or shift to products
Use Le Chatelier’s Principle and ideas of Kinetics to qualitatively explain why changes in concentration,
temperature, and partial pressure of gases (or overall pressure of system) lead to a shift to reactants or products.
Use Le Chatelier’s Principle to explain the effect of change in conditions on Q or K:
Conditions being concentration, pressure, and/or temperature.
Use Le Chatelier’s Principle to explain why a relationship between Q and K will lead to a directional shift in
reaction. (If Q > K, shift to reactants … explain why using Le Chatelier’s Principle)
Ch. 17 Sections 4-6
Translate between Ksp and solubilities.
Calculate using Ksp formula (solubility-product constant).
Write the Ksp formula for the dissolution of any salt.
Write the ionic equation for the dissolution of any salt.
Estimate relative values for any salt, given its chemical formula
rank solubilities given Ksps
rank Ksps given solubilities
explain when and why ranking of solubility does and does not follow Ksp ranking
Identify a solution as saturated, supersaturated, or unsaturated given its concentration and solubility or Ksp
“Common ion Effect”
Describe the effect of other chemicals on the solubility of a salt.
Calculate the effect using Ksp formula.
Quantitatively describe the relative effect, justifying your claim using Ksp formula.
Qualitatively describe the relative effect, justifying your claim using Le Chatelier’s Principle.
Include in “other chemicals” [OH-] or [H+], as communicated by pH.
Apply the “common ion effect” to explaining applications like:
- Iron hydroxides of acid-mine drainage
- Acid rain and carbonate solubility
- Ocean water solubilities
- Water softening
Perform calculations involving precipitation reactions to
Predict whether a precipitate will form when solutions are mixed, by comparing Q and Ksp.
Calculate the ion concentrations required to begin precipitation