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Solubility product constant - PowerPoint PPT Presentation


Chapter 21 “Neutralization”

Chapter 21 “Neutralization”

Chapter 21 “Neutralization”. Milbank High School. Section 21.1 Neutralization Reactions. OBJECTIVES: Explain how acid-base titration is used to calculate the concentration of an acid or a base. Section 21.1 Neutralization Reactions. OBJECTIVES:

By ganit
(218 views)

Chapter 21 “Neutralization”

Chapter 21 “Neutralization”

Chapter 21 “Neutralization”. Section 21.1 Neutralization Reactions. OBJECTIVES: Explain how acid-base titration is used to calculate the concentration of an acid or a base. Section 21.1 Neutralization Reactions. OBJECTIVES: Explain the concept of equivalence in neutralization reactions.

By ilya
(470 views)

Chapter 9 Chemical Equilibrium

Chapter 9 Chemical Equilibrium

Chapter 9 Chemical Equilibrium. 9.6 Equilibrium in Saturated Solutions. Saturated Solution. A saturated solution contains the maximum amount of dissolved solute contains solid solute is an equilibrium system: rate of dissolving = rate of recrystallization

By juro
(172 views)

Solubility Product Constant

Solubility Product Constant

Solubility Product Constant. Chemistry Mrs. Coyle. Solubility Equilibrium. AgCl(s) ↔ Ag + (aq) + Cl - (aq) The concentration of AgCl (s) is constant and AgCl is a strong electrolyte (dissociates almost completely), so K sp = [Ag + ] [Cl - ] K sp is the solubility product constant.

By meryl
(361 views)

Chapter Menu

Chapter Menu

Chemical Equilibrium. Section 17.1 A State of Dynamic Balance Section 17.2 Factors Affecting Chemical Equilibrium Section 17.3 Using Equilibrium Constants. Click a hyperlink or folder tab to view the corresponding slides. Exit. Chapter Menu. Section 17.1 A State of Dynamic Balance.

By rollo
(145 views)

Chemical Equilibrium

Chemical Equilibrium

Chemical Equilibrium. Reversible Reactions. Freezing Ice? Cooking an egg? Melting water?. Reversible reactions are those in which the products can react to re-form reactants. Ex : 2HgO (s) + heat -------------> 2Hg (l) + O 2 (g)

By ely
(92 views)

Chemistry 122

Chemistry 122

Chemistry 122. Solubility Equilibrium. The Solubility Product Constant. Solubility varies from one ionic compound to the next Some ionic compounds can dissolve quite significantly in water where others cannot They are either soluble or insoluble

By irish
(110 views)

Ionic Equilibrium in Solutions

Ionic Equilibrium in Solutions

Ionic Equilibrium in Solutions. K sp , K a and K b. Ionic Equilibrium. Much like with a system of equations, a solution is also an equilibrium NaCl ( aq )  Na + ( aq ) + Cl - ( aq ) The ions in this solution are constantly dissociating and re-associating. Ionic Equilibrium.

By kimo
(173 views)

Solubility Product Constant

Solubility Product Constant

Solubility Product Constant. Ksp. Ksp : review . What is the molar mass of H 2 O ? 2) How many moles are in 18 g of NaCl ? 3) How many g of CaCl 2 are found in 2 L of a 3 M solution of CaCl 2 ?

By zuwena
(145 views)

Applications of Aqueous Equilibria

Applications of Aqueous Equilibria

Applications of Aqueous Equilibria. Chapter 17 Pg. 719. Common Ion Effect. When a solution of a weak electrolyte is altered by adding one of its ions from another source, the ionization of the weak electrolyte is suppressed. This is referred to as the common ion effect.

By duena
(116 views)

Equilibrium

Equilibrium

Equilibrium. Chemical Equilibrium Review. Most chemical reactions do not go to completion. They appear to stop. • These reactions are reversible A chemical reaction that can occur in both the forward and reverse direction. Chemical Equilibrium.

By jeneil
(126 views)

Chapter 18 “Reaction Rates and Equilibrium”

Chapter 18 “Reaction Rates and Equilibrium”

Chapter 18 “Reaction Rates and Equilibrium”. Activated Complex. Activation Energy is being supplied. Section 18.1 Rates of Reaction. OBJECTIVES Describe how to express the rate of a chemical reaction. Section 18.1 Rates of Reaction. OBJECTIVES

By posy
(152 views)

Topic 10 – Part II

Topic 10 – Part II

Topic 10 – Part II. Applying Equilibrium Buffers Titrations Solubility Product. The Common Ion Effect. When the salt with the anion of a weak acid is added to that acid, It reverses the dissociation of the acid. Lowers the percent dissociation of the acid.

By lajos
(127 views)

ICE

ICE

ICE.

By midori
(158 views)

Chapter 18

Chapter 18

Chapter 18. Solubility and Complex-Ion Equilibria. Overview. Solubility Equilibria Solubility Product Constant Solubility and Common Ion Effect Precipitation Calculations Effect of pH on Solubility Complex-Ion Equilibria Complex Ion Formation Complex Ions and Solubility

By solada
(200 views)

Solubility Product Constant

Solubility Product Constant

Solubility Product Constant. Ksp. Adapted from Mrs. Kutcher’s South Kingston High School AP Chemistry PowerPoint http://hs.skschools.net/Teachers/mkutcher/Solubility%20Product%20Constant.ppt. Ksp, the solubility-product constant.

By kovit
(673 views)

Chapter 17 Equilibrium

Chapter 17 Equilibrium

Chemistry B2A. Chapter 17 Equilibrium. Collision. A + B  C. Effective collision: a collision that results in a chemical reaction. B. A. C. C. Effective Collision. 1. Concentration:. Effective Collision. 2. Energy & Temperature:.

By tassos
(153 views)

UNIT 12 REVIEW You Need: Marker Board Marker & Paper Towel Calculator

UNIT 12 REVIEW You Need: Marker Board Marker & Paper Towel Calculator

UNIT 12 REVIEW You Need: Marker Board Marker & Paper Towel Calculator. Write the equilibrium expression for the following reaction: 4 HCl(g) + O 2 (g)   2 Cl 2 (g) + 2 H 2 O(g). ANSWER: Keq = [Cl 2 ] 2 [H 2 O] 2 [HCl] 4 [O 2 ].

By ollie
(127 views)

UNIT 12 REVIEW Supplies: Marker Board Marker & Paper Towel Calculator

UNIT 12 REVIEW Supplies: Marker Board Marker & Paper Towel Calculator

UNIT 12 REVIEW Supplies: Marker Board Marker & Paper Towel Calculator. Write the equilibrium expression: 4 HCl(g) + O 2 (g)   2 Cl 2 (g) + 2 H 2 O(g). ANSWER: Keq = [Cl 2 ] 2 [H 2 O] 2 [HCl] 4 [O 2 ]. Write the equilibrium expression:. NCl 3 (g) + Cl 2 (g)   NCl 5 (g).

By halen
(101 views)

Additional Aqueous Equilibria CHAPTER 16

Additional Aqueous Equilibria CHAPTER 16

Additional Aqueous Equilibria CHAPTER 16. I. Buffers. A. Definitions Buffer- solutions that resist changes in pH when acid or base are added to it. - they are composed of a weak acid and its conjugate base or a weak base and its conjugate acid .

By ajay
(178 views)

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