Common Ion Effect On Solubility Pogil

™POGIL Activities for AP. Chemistry Equilibrium Systems Reaction Quotient.181. Created Date: 3/17/2016 2:16:16 PM.

  • POGIL: Acids,Bases,pH pOH POGIL: Ka and Kb POGIL: Hydrolysis POGIL: Buffers POGIL: Titration curves POGIL: Acid Base Indicators Unit 7: Equilibrium Part 3 ch 17 LAB/Activity Solubility equilibria Common ion effect Gibbs and equilibrium LAB: Ksp with spectroscopy POGIL: Ksp and solubility POGIL: pH dependent solubility POGIL: Gibbs and Equilibrium.
  • Common ion effect webcast 11/17 Work on K sp minilab. K minilab Finish K: sp: precipitation problems 11/18 POGIL Common Ion Effect on Solubility K: sp: practice problems to study for quiz 11/21 half day K: sp: Quiz Finish K: sp: minilab Read/highlight chapter 16 outline 11/22.

Common Ion Effect On Solubility Pogil Answers

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AP Chem Exam Review





Date Classwork Homework
4/26Done with Chapter 18!!! Woohoo! try as many of those free response questions as possible and review for the practice exam
Come to class tomorrow from 745-945 to take the practice exam.
Also take a look at the following animation, it helps explain galvanic cells pretty well...
http://www.mhhe.com/physsci/chemistry/animations/chang_2e/galvanic_cell.swf
4/25Chapter 18 finished most of the notes, the rest you should review on your own. Powerpoints can be found below. Chpt 18 notes pg 881 Q's 69-77 odd, 81, 85, and 87
Answer key to this hw and last nights homework is also posted
4/22Chapter 18, sections 18.1-18.3 Answer keys to some hw problems can be downloaded below.
Read chapter 18 notes on batteries, go through powerpoint and answer the following questions in the textbook
pg 879 Q's 39-59 odd
4/21 reviewed hw problems for 16 and 17
POGIL activity on chapter 17 and reviewed answers 		Read Chapter 18 sections 18.1 and 18.2. Look through powerpoint online
Answers Q's 17, 19, 29, 31, 33 and 35
4/20Finished notes on chapter 17
Started notes on chapter 18 		Complete questions in textbook, Chapter 17 Q's 51-59 odd, 65-75 odd and the multiple choice at the end of the chapter.
4/19 Continued with Chapter 17, sections 17.3-17.7 free response practice problem
4/18 Notes on chapter 17, sections 17.1-17.3
We will not meet during lunch tomorrow, we will meet on Wed, second lunch.
Review notes from chapter 6 and use textbook as well.
Chapter 17 pg 823, Q's 19,25,31,35,41, 45,47
Spring Break Assignment:
Read and take notes on Chapter 16. Learn the material and complete the free response questions found below. I have included the answer keys and other extra problems as well. 		Complete chapter 16 starting on pg 781, Q's 19-27 odd, 35, 37, 41, 49, 53, 61-67 odd, 69. I will leave it up to you to try and complete as many additional practice problems on your own.
4/4 Finished notes on chapter 15
Reviewed answers to practice problems and pre-lab questions 		Chapter 15 pg 752-3 Q 55, 57, 59 and 65
Labs need to be handed in before break
Assessment for Chapter 14/15 will be Thursday
3/29Notes on Titrations, strong-strong and weak-strong Complete POGIL titration packet found below
Read rest of chapter 15
Complete Pre-lab for lab below.
3/28Continued with Notes on Chpt 15.
Reviewed homework from last week		Chapter 15 Q's 37-49 odd


3/22 Notes on Chpt 15.2 Buffer solutions
POGIL packet on Buffers		 in textbook, Chapter 14 pg 706, 131-135 all, and 152
Chapter 15 pg 17-35 odd
Lab for tomorrow can be found below, acid base titration of acetic acid (vinegar)
3/21 Finished Chapter 14 and started Chapter 15.1, calculating pH for common ion solutionsComplete POGIL packet on common ion effect
3/15 completed practice problems in classcomplete the following questions in the textbook
Chapter 14 Q's 51, 61, 83-89 all, 91-95 odd and 143
3/14finished notes on 14.5-14.6 review notes and practice problems
3/11Finished 14.2 and started 14.3 Please look ahead for the rest of 14.3 and 14.4. Complete the practice problems in the textbook CHPT 14 Q's 39-46
3/10 liquid nitrogen demo
started chapter 14 acids and bases		complete POGIL packet on strength of acids
3/9 no classRead section 14.1 in textbook and try questions 35 and 37
Lab will be due next week, no pre-lab for tomorrow, we will move on to chapter 14 and there will also be a special demonstration!
3/8 quiz on chapter 13 and reviewed calculations for lab
3/7Finished data collection for lab quiz tomorrow on chapter 13
3/1 Reviewed chapter 13, read over lab for thursday and handed out practice test for chapter 13Complete pre-lab for Thursday
Powerpoint for chapter and worksheets can be found below
Please complete also the following practice problems in the textbook: 63-69 odd, 107
2/29Finished notes on Chapter 13 Le Chatelier's principle, reviewed homework and practiced in class no homework
2/25Notes on 13.4-13.6Complete the following questions in the textbook. Chapter 13 pg 645-48 Q 41-53 ODD, 61, 71, 73, 75, 79,
2/24 Continued with notes on 13.1, 13.2 and 13.3 Completed some practice problems and went over lab calculations. Also went over reaction Quotient
Answers to homework due today can be found below. 		No lab for tomorrow, we will do a lab on another day. Instead, complete the following textbook questions pg 644-645 Q's 23-29 odd, 33-37 odd and 39
The true values for the last lab; both should be first order
2/17 Quiz on Chapter 12 Kinetics
Started notes on Chapter 13		 Complete Pre-lab assignment for Lab on Friday ( which is a D day)
Complete the three free response questions found below on kinetics and you can also find notes on the Arrhenius Equation to review
Understand what the equation can be used for and the two different forms of it, also understand how it relates the the graph.

Finished chapter 12 study for quiz after break
2/10no class complete the following questions from the textbook
25-35 odd, 63, 65, 95
2/09Continued with Chapter 12 Kinetics 12.1 and started 12.2 finish worksheet from class




Learning Objective

  • Explain the common ion effect.

Key Points

  • The role that the common ion effect plays in solutions is mostly visible in the decrease of solubility of solids. Through the addition of common ions, the solubility of a compound generally decreases due to a shift in equilibrium.
  • The common ion effect also plays a role in the regulation of buffers. Buffering solutions contain either an acid or base, accompanied by its conjugate counterpart. Addition of more like conjugate ions will ultimately shift the pH of the solution.
  • The common ion effect must be taken into consideration when determining solution equilibrium upon addition of ions that are already present in the solution.

Terms

  • Le Chatelier’s principleThe principle used to predict the effect of a change in conditions on a chemical equilibrium.
  • bufferA solution used to stabilize the pH (acidity) of a liquid.
  • conjugate baseThe species that is created after the donation of a proton.
  • conjugate acidThe species created when a base accepts a proton.

Solubility

Solubility refers to the amount of material that is able to be dissolved in a particular solvent. For example, table salt (NaCl) placed in water eventually dissolves. However, if more table salt is continuously added, the solution will reach a point at which no more can be dissolved; in other words, the solution is saturated, and the table salt has effectively reached its solubility limit.

Chemical equilibrium is the chemical state where there are no net physical or chemical changes between the reactant and the products of a reaction. This is because the rate of the forward (reactant to product) and reverse (product to reactant) reactions are equal.

Solubility equilibrium refers to the state of chemical equilibrium between a chemical compound in the solid state and a solution composed of that dissolved compound. This equilibrium is established when the rates of migration between the solid and aqueous phases of the molecules (or ions) are equal.

Common Ion Effect

Common Ion Effect On Solubility Pogil Key

Whenever a solution of an ionic substance comes into contact with another ionic compound with a common ion, the solubility of the ionic substance decreases significantly. For example, this would be like trying to dissolve solid table salt (NaCl) in a solution where the chloride ion (Cl–) is already present. The amount of NaCl that could dissolve to reach the saturation point would be lowered. This phenomenon is the common ion effect and plays important roles in pharmaceutical and environmental areas. The common ion effect can be explained by Le Chatelier’s principle of chemical equilibrium:

[latex]AB_{(s) }leftrightarrow { A^+ }_{ (aq) } + { B^-}_{ (aq) }[/latex]

For a simple dissolution process, the addition of more of one of the ions (A+) from another compound will shift the composition to the left, reducing the concentration of the other ion (B–), effectively reducing the solubility of the solid (AB). For example, when calcium fluoride dissolves into calcium and fluoride ions, the solubility product expression is:

[latex]CaF_{2(s) }leftrightarrow { Ca^{+2} }_{ (aq) }+{ 2F^{-} }_{ (aq) }[/latex]

Pogil

This expression must always hold, even if some ionic species come from other sources. Therefore, if more [latex]Ca^{+2}[/latex] ions are placed in solution, the equilibrium will shift to the left, favoring the solid form and decreasing the solubility of the solid.

Buffer Solutions

A buffer solution is composed of a weak acid and its conjugate base, or a weak base and its conjugate acid. Addition of excess ions will alter the pH of the buffer solution. Therefore, the common ion effect takes a role in pH regulation. According to Le Chatelier’s principle, addition of more ions alters the equilibrium and shifts the reaction to favor the solid or deionized form. In the case of an an acidic buffer, the hydrogen ion concentration decreases, and the resulting solution is less acidic than a solution containing the pure weak acid.

For example in the reaction:

Common Ion Effect On Solubility Pogil

[latex]HCN_{(aq)}leftrightarrow {H^+}_{(aq)} + {CN^-}_{(aq)}[/latex]

The addition of cyanide ions (CN–) will suppress the ionization of hydrogen cyanide (HCN) and shift its equilibrium to the left. The percent dissociation of the hydrogen cyanide will decrease, therefore decreasing the H+ ions and increasing the pH of the solution.

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