Aim: What are solubility factors?

Slides:



Advertisements
Similar presentations
IPC 9.B Relate the concentration of ions in a solution to physical and chemical properties such as pH, electrolytic behavior, and reactivity.
Advertisements

Solubility Honors Chemistry Mrs. Jacobus. Components of a Solution  Solute is the substance being dissolved – powder  Solvent is the dissolving agent.
Chapter16 Solutions 16.1 Properties of Solutions.
Solubility and Solubility curves
Hydrogen bonding… (a) occurs only between water molecules (b) is stronger than covalent bonding (c) can occur between NH 3 and H 2 O (d) results from strong.
Solubility and Solubility curves. Solubility The solubility of a substance is the mass required to make a saturated solution in a given quantity of solvent.
Solubility Do Now: p.4. Remember…likes dissolve like Things that dissolve in water – Soluble ionic – Acids (ex HCl) – Bases (ex. NaOH) – Polar covalent.
Solutions Homogeneous mixtures that may be solid, liquid or gaseous Solute: The part of the solution that is dissolved Solvent: The part of the solution.
SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)
SOLUTIONS Section 8.1 and
1)How many grams of solute are needed to saturate the given mass of H 2 O at the given temperature. A. at 40 o C 40 g KCl 100 g H 2 O B. at 10 0 C 80 g.
Topic: Solubility and Table G Do Now: label as soluble and insoluble 1. CH 4 2. AgCl 3. C 12 H 22 O NaNO 3 5. KOH.
Solubility Curves. A solubility curve (see Table G) shows the maximum amount of solute that will normally dissolve in a given amount of a solvent over.
SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved Solvent = dissolving agent.
Solubility.
06 – using a solubility TABLE & SOLUBILITY CURVES
Solubility Honors Chemistry Mrs. Jacobus. Components of a Solution  Solute is the substance being dissolved – powder  Solvent is the dissolving agent.
Solutions. A solution is a homogeneous mixture where all particles exist as individual molecules or ions. Mixtures in chemistry are combinations of different.
 Solution Terminology: Solute, solvent, saturated, unsaturated, supersaturated, aqueous, homogeneous, heterogeneous, soluble, insoluble, miscible (alcohol.
30/09/99 Solubility curves
Solutions.
SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)
Properties of Solutions. Solutions Solutions are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed uniformly.
Solubility How much of a solute will dissolve in a solvent at a given temperature  High solubility – soluble more solute dissolves  Low solubility –
Solubility The maximum quantity of the substance, expressed in grams, that will dissolve in a certain solvent at a specific temperature. S-C-9-1_Solubility.
Ch. 8 Solutions, Acids, & Bases I. How Solutions Form  Definitions  Types of Solutions  Dissolving  Rate of Dissolving.
Solubility Practice Problems
Section 1C.1 & C.2 Reading Solubility Curves
Reading Solubility Curves
using a solubility TABLE & SOLUBILITY CURVES
How much is the solubility of potassium
Ch. 8 Solutions, Acids, & Bases
Solubility Solubility is the amount of solute that dissolves in 100 g of solvent to form a saturated solution at a given temperature. Ex. The maximum amount.
Solubility The maximum quantity of the substance, expressed in grams, that will dissolve in a certain solvent at a specific temperature.
Warm Up 11/1/17 1. What is an acid? 2. What is a base?
Solutions and Solubility Curves
Solubility CN What is solubility?
Unit 4: Solutions and Kinetics
Unit 2 Lesson 2 Solutions Video Disk Unit 6 Demo Magic Sand
Solubility & Saturation
Solubility Notes Unit 5.
READ SOLUBILITY CURVES
SOLUTIONS AND SOLUBILITY
A. Factors Affecting Solubility
Bellwork 1. What do you remember about the difference between homogeneous mixtures and heterogeneous mixtures?
Hydrogen bonding… (a) occurs only between water molecules
Solutions.
Unit 4: Solutions and Kinetics
Solutions and Kinetics
Solubility and Solubility Curves
Solubility.
Can be solid, liquid, or gas.
Quiz – Solubility Graph Review
64g / 100g H2O 51g / 100g H2O How much is the solubility of potassium
Which statement describes KCl(aq)?
Concentration and Solubility
Hydrogen bonding… (a) occurs only between water molecules
Solutions, Acids, & Bases
Solubility Curves.
The substance being dissolved in a solution.
Aim: How does temperature affect the solubility of solids, liquids, and gases? Do Now: Increasing temperature of a solution _______________the solubility.
Chemistry, Ch. 13: Solutions
Factors Affecting Solubility
Unit 6: Solutions Solubility.
Solutions.
Warm Up Give an example of a polar substance.
Reading Solubility Curves
Aim: How to describe the different types of solutions
Unit 8 – Solutions Chapter 15
What is Solubility? The maximum amount of a substance that will dissolve in a certain amount of solvent at a given temperature is called that substances.
Presentation transcript:

Aim: What are solubility factors? Do now: Define what a solution is and list some properties of solutions.

Solubility is the property of a solid, liquid, or gaseous chemical substance called solute to dissolve in a liquid solvent to form a homogeneous solution of the solute in the solvent.

The solubility of a substance fundamentally depends on the used solvent as well as on temperature and pressure.

The extent of solubility ranges widely, from infinitely soluble (fully miscible) such as ethanol in water, to poorly soluble, such as silver chloride in water. The term insoluble is often applied to poorly or very poorly soluble compounds.

Nature of reactants Solution type Non-polar Solvent Polar Solvent Ionic

Like dissolves Like.

Temperature As temperature increases solids become more soluble in water As temperature increases gasses become less soluble in water.

Pressure Pressure has little or no effect on the solubility of solid or liquid solutes. As pressure increases, the solubility of gasses in liquids increases.

◦Factors affecting the rate of solubility 1. Size of solute particles 2. Stirring 3. Amount of solute 4. Temperature

HOW DO WE READ SOLUBILITY GRAPHS

Learning Check 1) What mass of solute will dissolve in 100mL of water at the following temperatures? a. KNO3 at 70C = ____________ b. NaCl at 100C= ____________ c. NH4Cl at 90C= ____________ d. Which of the above three substances is most soluble in water at 15C. = ____________

Choose (saturated, unsaturated, super saturated) 1. a. What is the solubility of KCl at 5C? _______ b. What is the solubility of KCl at 25C? _______ c. What is the solubility of Ce2(SO4)3 at 10C? _______ d. What is the solubility of Ce2(SO4)3 at 50C? _______ 2. At 90C, you dissolved 10 g of KCl in 100. g of water. Is this solution saturated or unsaturated?

Saturated or Unsaturated? Solution Saturated or Unsaturated? If unsaturated: How much more solute can dissolve in the solution? a solution that contains 70g of NaNO3 at 30C (in 100 mL H2O) a solution that contains 50g of NH4Cl at 50C (in 100 mL H2O) a solution that contains 20g of KClO3 at 50C (in 100 mL H2O) a solution that contains 70g of KI at 0C (in 100 mL H2O)