Solubility Main Concept:

Slides:

Advertisements

Similar presentations

PreAP Chem Go over Ksp wkst Buffers What to expect on the test Homework.

Advertisements

Water and solutions Water Polarity Solubility (like dissolves like)

Starter- Copy the paragraph (Correct the mistakes) Ionic substances have low melting points and high boiling points. This is because they are held together.

Precipitation Equilibrium

Christine Musich Science April 2013 Misconceptions: Is Dissolving the Same as Melting?

Chemistry 130 Solubility equilibria Dr. John F. C. Turner 409 Buehler Hall

The K sp of chromium (III) iodate in water is 5.0 x Estimate the molar solubility of the compound. Cr(IO 3 ) 3 (s)  Cr 3+ (aq) + 3 IO 3 - (aq)

Chapter 17 SOLUBILITY EQUILIBRIA (Part II) 1Dr. Al-Saadi.

Solubility Equilibria

A salt, BaSO4(s), is placed in water

© 2009, Prentice-Hall, Inc. Solubility of Salts (Ksp) Consider the equilibrium that exists in a saturated solution of BaSO 4 in water: BaSO 4 (s) Ba 2+

Solubility Product Constant Factors Affecting Solubility Selective Precipitation.

Ions In Solution.

Precipitation Analysis Considering the formation of solid from solution. Q vs. Ksp Ion Analysis.

Unit 7 - Chpt 16 - Solubility equilibria and Quantitative analysis Solubility equilibria and Ksp Predict precipitation Qualitative analysis HW set1: Chpt.

7.3 Making salts from solutions Soluble or insoluble? What do these terms mean? 17 September 2015 Fertilisers Water Treatment.

Solubility Allows us to flavor foods -- salt & sugar. Solubility of tooth enamel in acids. Allows use of toxic barium sulfate for intestinal x-rays.

11111 Chemistry 132 NT The most difficult thing to understand is the income tax. Albert Einstein.

SOLUTIONS A homogeneous mixture in which the components are uniformly intermingled.

Salts By Amy Badger.

Chapter 21 Neutralization Neutralization Reactions Salts in Solution.

Solubility Chapter 17. No only do acids and bases dissolve in aqueous solutions but so do ionic compounds –Many ionic compounds tend to be strong electrolytes.

Chapter 13 Chemical Equilibrium. REVERSE REACTION  reciprocal K.

Aqueous Equilibria Chapter 16 Solubility Equilibria.

Terms Solute Substance that has been dissolved in a liquid Solvent the solution (liquid or gas) part of the solute concentration Dissolves the solute Solubility.

Le Chatelier’s Principle

Solubility & SOLUBILITY PRODUCT CONSTANTS. Solubility Rules All Group 1 (alkali metals) and NH 4 + compounds are water soluble. All nitrate, acetate,

Types of Reactions. In Chemistry, we can identify a lot of different types of chemical reactions. We can put these chemical reactions into groups, so.

Chemistry 1011 Slot 51 Chemistry 1011 TOPIC Solubility Equilibrium TEXT REFERENCE Masterton and Hurley Chapter 16.1.

Some Terminology Soluble – Will dissolve in a solvent Insoluble – Will not dissolve in a solvent Solvent – The substance that dissolves the solute Solute.

PH notes pH = % Hydrogen. Many compounds are soluble (can dissolve) in water. When an ionic compound dissolves in water, ionic bonds are broken. As a.

Complex Ion Equilibria and Solubility A complex ion can increase the solubility of a salt. Ag + (aq) + 2 NH 3 (aq) Ag(NH 3 ) 2 + (aq) K f = [Ag(NH.

DO NOW: What is dissolution. What is precipitation

Additional Aspects of Aqueous Equilibria. Roundtable problems P.757: 3, 6, 12, 14, 18, 24, 30, 38, 44, 50, 54, 56, 58, 64, 68, 70, 72, 103.

Factors Affecting Solubility pH Common Ion Effect Formation of Complex Ions.

Common-Ion EffectCommon-Ion Effect  Similar to acids and bases  There is a “common ion” when 2 salt solutions are mixed together.

Chemical Equilibrium l The Nature of Chemical Equilibrium l Shifting Equilibrium l Equilibria of Acids, Bases, and Salts l Solubility Equilibrium.

Solubility Constant (Ksp). © 2009, Prentice-Hall, Inc. Solubility of Salts (Ksp) Consider the equilibrium that exists in a saturated solution of BaSO.

Section 15.1 Forming Solutions 1.To understand the process of dissolving 2.To learn why certain substances dissolve in water 3.To learn qualitative terms.

 Usually consider solids (salts)  Dissolving in water – “like dissolves like” ◦ Forming aqueous solutions.  Remember pure liquids and solids are not.

Precipitate Testing.

17.3 Acid-BaseTitrations A known concentration of base (or acid) is slowly added to a solution of acid (or base). For example, a standard solution of NaOH.

The Solubility Product Principle

Solubility Product Constant, Ksp

Acids and Bases Acids are compounds that produce hydronium ions in water [H3O+] **that have H+ as the cation** Sour taste Reactivity with metals (single.

Welcome Back!!! Bellwork:

17.4: Solubility Equilibria

Predicating Solubility

Lewis-Acid Base Chemistry and Complexation Equilibria

Solubility Equilibria

Clicker #1 When lead(II) nitrate and potassium iodide are mixed, what precipitate will form? Pb(NO3)2(aq) + KI(aq) → A) KNO3 B) KI C) Pb(NO3)2 D) PbI2.

Equilibrium System.

Titration A pH meter or indicators are used to determine when the solution has reached the equivalence point, at which the stoichiometric amount of acid.

Ksp: Solubility Product Equilbria

Clicker #1 When lead(II) nitrate and potassium iodide are mixed, what precipitate will form? Pb(NO3)2(aq) + KI(aq) → A) KNO3 B) KI C) Pb(NO3)2 D) PbI2.

Solubility and Complex Ion Equilibria

Solubility and Complex Ion Equilibria

Lesson # 5 The Solubility Product

Clicker #1 When lead(II) nitrate and potassium iodide are mixed, what precipitate will form? Pb(NO3)2(aq) + KI(aq) → A) KNO3 B) KI C) Pb(NO3)2 D) PbI2.

Acids and Bases Bundle 4: Water.

Ionic Equilibria III: The Solubility Product Principle

Chemistry: The Central Science

Chapter 15 Applied equilibrium.

Question: How do we know what ions are present in a solution?

Neeli Shah and Denise Ferguso 17.5 Factors That Affect Solubility

C4 – Chemical changes Key Concepts.

Buffers and titrations

Presentation transcript:

Solubility Main Concept: The solubility of a substance can be understood in terms of equilibrium.

Solubility Solubility Free Energy and Solubility Salts and Solubility Common Ions pH

- The dissolution of a substance in a solvent is a reversible reaction  has an associated equilibrium constant - For dissolution of salt, reaction quotient, Q, = solubility product, and equilibrium constant for reaction = Ksp (solubility-product constant) - solubility of a substance can be calculated from Ksp for dissolution reaction  can be used to reason qualitatively about relative solubility of different substances

- free energy change (ΔG°) for dissolution of a substance reflects breaking of forces holding solid together and the interaction of dissolved species with solvent - Also, entropic effects must be considered  solubility requires consideration of all of these contributions to the free energy

- All sodium, potassium, ammonium, and nitrate salts are soluble in water - salts  less soluble in solutions that have ions in common with salt  affects solubility of salts in seawater and other natural bodies of water  think Le Chatelier’s principle

- solubility of salt will be pH sensitive when one of the ions is an acid or base  Applications include high pH’s leading to iron hydroxide precipitate in acid-mine drainage and effects of acid rain on solubility of carbonates  think Le Chatelier’s principle - basic anions more soluble in acids - acidic cations more soluble in bases