Types of Mixtures Solutions Suspensions Colloids.

Slides:



Advertisements
Similar presentations
Ch. 13 Solutions What is a solution?
Advertisements

Solutions & Concentration. Water  Polar molecule w/ polar bonds  Causes surface tension & ability to dissolve polar molecules and ionic compounds.
SOLUTIONS Chapter 15. What are solutions?  Homogeneous mixtures containing two or more substances called the solute and the solvent  Solute- is the.
Chapter 15 Solutions.
Solutions. Mixtures A substance made up of 2 or more elements or compounds that are not chemically combined and can be separated 2 classifications 1.
CHAPTER 13 Mixtures and Concentrations. Types of Mixtures Solutions Suspensions Colloids.
Chapter 12: Solutions.
Ch 12.1 Types of Mixtures.
Physical Properties of Solutions Unit 10 Why are some compounds more effective in melting ice than others?
Solutions C-16 Properties of solutions Solutions … Mixture (but special)  Solute + solvent Homogeneous (molecular level) Do not disperse light.
Chapter 12 Solutions 12.1 Types of Mixtures.
Solutions Chapter 16. Desired Learning Objectives 1.You will be able to describe and categorize solutions 2.You will be able to calculate concentrations.
CHAPTER 17 and 18 WATER AND AQUEOUS SOLUTIONS.  Water 1. Structure of water (H 2 O) a. two atoms of hydrogen b. One atom of oxygen c. Bent structure.
Characteristics of solutions Solution – homogeneous mixture Solution – homogeneous mixture a) parts of a solution i) solute – substance being dissolved.
Physical Properties of Solutions.  Homogeneous mixtures: ◦ Solutions – ions or molecules (small particles) ◦ Colloids – larger particles but still uniform.
Chapter 25. High surface tension, low vapor pressure, and high boiling points.
Aqueous Solutions Solution: Homogeneous mixture; solid liquid, or gas Soluble: Capable of being dissolved Solute: Substance that is dissolved, present.
SOLUTIONS A mixture worth getting your hands wet in.
1 Ch. 7: Solutions Chem. 20 El Camino College. 2 Terminology The solute is dissolved in the solvent. The solute is usually in smaller amount, and the.
II III I C. Johannesson The Nature of Solutions Solutions.
Solutions. Classification of Matter Solutions are homogeneous mixtures.
SOLUTIONS Chapter 12. Solutions Homogeneous mixtures of two or more substances in a single phase  Example: salt water  The salt is interspersed among.
Types of Mixtures, Rates of Solubility, and Molarity/Molality
NOTES: – Solutions and Concentration.
Solutions From Chapters 12 and 13. Reading Chapter 12 –Section 1 (pp ) –Section 4 (pp ) Chapter 13 –all (pp )
Mixtures and Solutions Chapter 14. Heterogeneous Mixtures  Suspensions –Mixture containing particles that settle out if left undisturbed. –Particles.
Classifications of Mixtures Heterogeneous Mixtures—composed of different types of phases of substances - ex: Fruit salad Granite Homogeneous Mixtures—the.
Solutions Chapter 13 & 14. Solution  A uniform mixture that may contain solids, liquids, or gases  Also called a homogeneous mixture  Composed of a.
Solutions CPS Chemistry. Definitions  Solutions A homogeneous mixture of two or more substances in a single phase  Soluble Capable of being dissolved.
Solutions Chm 3.2. Solutions Solute – substance dissolving Solute – substance dissolving Solvent – substance solute is dissolved in Solvent – substance.
Solutions Homogeneous mixtures containing two or more substances. –Solvent- The substance that dissolves –Solute- The substance being dissolved.
SOLUTIONS Chapter 13 and 14.
Modern Chemistry Chapter 12- Solutions
CHAPTER 13 SOLUTIONS. BASIC DEFINITIONS Solution Solution – a homogeneous mixture of 2 or more substances in a single phase Solute – The dissolved substance.
Solutions. Classification of Matter Solutions are homogeneous mixtures.
Unit 8 Solution Chemistry
Why is salt spread on the roads during winter?. Ch 18 Solutions  Properties of Solutions  Concentrations of Solutions  Colligative Properties of Solutions.
Solutions. Solutions Definition: Homogeneous mixture of two or more substances in a single phase. Like Dissolves Like (i.e. nonpolar molecules dissolve.
Chapter 16: Solutions 16.1 Properties of Solutions.
Solutions. Solutions are: A homogeneous mixture of two or more substances in a single phase Composed of: 1.Solvent- the substance that does the dissolving.
Chemistry Chapter 15 Solutions Solutions A. Characteristics of Solutions -composed of two parts 1.The substance that is dissolved is the solute.
Ch 12.1 Types of Mixtures. Heterogeneous vs. Homogeneous Mixtures Heterogeneous Mixture: mixture does not have a uniform composition. Ex: Milk and soil.
Heterogeneous Mixtures Heterogeneous Mixtures: Not evenly blended Suspensions: a mixture containing particles that settle out if left undisturbed Colloids:
Chapter 12 Solutions. Review Types of mixtures: Heterogeneous mixtures: do not have a uniform composition Homogeneous mixtures: have a uniform composition,
Solutions Mixtures: - Heterogenous Mixture: substances that make up the mixture are not spread uniformly throughout the mixture. - Homogenous Mixture:
Physical Properties of Solutions Honors Unit 10. Solutions in the World Around Us.
Solutions. What is a solution? A homogeneous mixture A homogeneous mixture Composed of a solute dissolved in a solvent Composed of a solute dissolved.
Solutions. Definitions Solution: homogeneous mixture of 2 or more substances in a single physical state Solute: the substance dissolved in the solution.
Classifications of Mixtures Heterogeneous Mixtures—composed of different types of phases of substances - ex: Fruit salad Granite Homogeneous Mixtures—the.
Chapter 13-1 Types of Mixtures. solutions  Soluble: capable of being dissolved  Solution: a homogenous mixture of two or more substances in a single.
Solutions. SoluteSolven t Solubility ConcentratedDilute : the ability to be dissolved temperature dependent a lot of solute little solute gets dissolved.
Solution Notes Solution HW OBJECTIVES. HETEROGENEOUS MIXTURES Contain substances that exist in distinct phases. Two types are heterogeneous mixtures are.
Chapter 14 Solutions Types of Mixtures Solution Concentration Factors Affecting Solvation Colligative Properties of Solutions.
Do Now Create a list (at least 4 items) of 5 common solutions, give a reason for why you think each one is a solution.
Chapter 14 Solutions. What are solutions? A Solution is…
SOLUTIONS.
Solutions.
SECTION 1. TYPES OF MIXTURES
Do Now Create a list (at least 4 items) of 5 common solutions, give a reason for why you think each one is a solution.
Heterogeneous vs. Homogeneous
Solutions.
Solutions.
Ch. 13 Solutions What is a solution?
Properties of Solutions
Mixtures (Solutions) Heterogeneous Homogeneous Solution Heterogeneous
Heterogeneous vs. Homogeneous
Chapter 16: Mixtures & Solutions
Chapter 16: Mixtures & Solutions
Solutions.
Solutions.
Presentation transcript:

Types of Mixtures Solutions Suspensions Colloids

Solutions are: A homogeneous mixture of two or more substances in a single phase Composed of: 1.Solvent- the substance that does the dissolving 2.Solute- the substance that is being dissolved Example: In sugar water, water is the solvent and sugar is the solute.

Suspensions A mixture in which the particles are so large that they settle out unless the mixture is constantly stirred or agitated. Ex. a jar of muddy water

Colloids A mixture in which the particles are intermediate in size between those in solutions and suspensions. Ex. paints, milk, mayonaise, fog, chesse

Tyndall Effect Colloids appear to be homogeneous mixtures (aka solutions) because the individual particles can not be seen…however, they are not true solutions. The particles are large enough to scatter light. This effect is known as the Tyndall effect.

Types of Solutions: Type of solution is determined by the solvent. Gaseous-mixture of two or more gases Liquid- solvent is a liquid Solid- solvent is a solid Examples of: 1.Gaseous- air, scuba tanks 2.Liquid- tea, Kool- aid, cokes, salt water 3.Solid- metal alloys, amalgams (dental fillings)

Some solutions conduct electricity : Electrolytes- a solution that conducts electricity as a result of the formation of ions in solution (examples: salt water, vinegar) Nonelectrolyte- a solution that does not conduct electricity because there is no formation of ions in solution (example: sugar in oil)

Electrolyte Nonelectrolyte

Factors that Affect Rates of Dissolving Solids in Liquids: 1.Surface Area- increasing surface area increases the rate of dissolving 2.Agitation- stirring or shaking increases rate of dissolving 3.Heat- heating the solvent will increase the rate of dissolving

Solubility The amount of a substance that is dissolved at solution equilibrium in a specific amount of solvent at a specified temperature. Factors Affecting Solubility: 1.Nature of Solute and Solvent- “like dissolves like”- polar dissolves polar-nonpolar dissolves nonpolar 2.Pressure- changes in pressure have little affect on dissolving solids in liquids but an increase in pressure will increase the solubility of gases in liquids 3.Temperature a)Increasing temp., decreases gas solubility b)Increasing temp., increases solid solubility

3 Classifications of Solutions Saturated- a solution that contains the max. amount of dissolved solute at a given temp. Unsaturated- a solution that contains less solute than a saturated solution at a given temp. Supersaturated- a solution that contains more dissolved solute than a saturated solution at a given temp.

Solubility Curves: Show how much solute can go into solution with a given amount of solvent at different temperatures.

Solubility Curve:

Colligative Properties A property that depends on the number of solute particles but is independent of their nature 3 Colligative Properties 1.Vapor Pressure Lowering 2.Freezing Point Depression 3.Boiling Point Elevation

Vapor Pressure Lowering- the vapor pressure of a solvent containing a nonvolatile solute is lower than the vapor pressure of the pure solvent at any temp. Freezing Point Depression- the freezing point of a solvent containing a solute will be lower than the pure solvent Boiling Point Elevation- the boiling point of a solvent containing a solute will be higher than the pure solvent

Solution Concentration: Concentration is a measurement of the amount of solute in a given amount of solvent or solution Can be expressed qualitatively or quantitatively Qualitative Terms: 1.Dilute- relatively small amount of solute compared to solvent 2.Concentrated- relatively large amount of solute in a solvent

Quantitative Terms: Percent by Mass Molarity Molality

Percent by Mass The number of grams of solute dissolved in 100 g of water Percent by mass = mass solute x100 mass solute + mass solvent

Examples: A solution of sodium chloride is prepared by dissolving 5 g of salt in 550 g of water. What is the concentration as given by percent by mass? Answ: 0.9% What is the percent by mass of a solution prepared by dissolving 4 g of acetic acid in 35 g of water. Answ: 10%

Molarity Symbolized by M Units of mol L Describes how many moles of solute are present per liter of solution

Examples: What is the molarity of 3.5 L of solution that contains 90 g of sodium chloride? Answ: 0.44 M How many moles of HCl are present in 0.8 L of a 0.5 M HCl solution? Answ: 0.4 mol How many grams of sodium chloride will be required to make 555 mL of a 1.45 M solution? Answ: 47.1 g

More Examples: How many liters of solution can be prepared if 78.9 g of sodium chloride is used to make a 3.00 M solution? Answ: 0.45 L What is the molarity of a solution that is prepared by using 20 g of sodium hydroxide in enough water to make a 2 L solution? Answ: 0.25 M

Dilution Problems Use the equation: M1V1 = M2V2 Where M1 = molarity 1, V1= volume 1….all volumes must be in liters.

Examples: What is the molarity of a solution that is made by diluting 50 mL of a 4.74 M solution to 250 mL? Answ: M

Molality Symbolized by m Units are mol solute kg of solvent Describes how many moles of solute are present per kg of solvent.

Examples: A solution contains 17.1 g of sucrose (C 12 H 22 O 11 ) dissolved in 125 g of water. Find the molal concentration. Answ: m How much iodine must be added to prepare a m solution of iodine in carbon tetrachloride (CCl 4 ) if 100 g of CCl 4 is used? Answ: 12.2 g

More Examples: What is the molality of a solution composed of 2.55 g of acetone (CH 3 ) 2 CO, dissolved in 200 g of water? Answ: m What quantity, in grams, of methanol (CH3OH) is required to prepare a M solution in 400 g of water? Answ: 3.12 g

How many grams of AgNO 3 are needed to prepare a m solution in 250 mL of water? (Hint.. 1 mL of water = 1g and 1 L of water = 1 kg) Answ: 5.31 g Honors: What is the molality of a solution that contains 200 g of carbon tetrachloride in 800 mL of chloroform? The density of chloroform is g/mL.

Examples: 2H 3 PO 4 + 3Ca(OH) 2  Ca 3 (PO 4 ) 2 +6 H 2 O 1.If 2 L of 4 M phosphoric acid is used, how many grams of water could be formed? 2.If 6 g of calcium hydroxide is used, how many liters of a 5 M acid solution would be needed?

More Examples: 3. When 200 mL of 6 M phosphoric acid is used, how many mL of a 3 M calcium hydroxide solution would be required? 4. What is the molarity of 0.6 L of calcium phosphate produced when 500 mL of 3 M phosphoric acid is used?

More Examples: Na 2 CO 3 + HCl  NaCl + H 2 O + CO 2 5. If the above reaction was performed at STP and 2 L of carbon dioxide gas was collected, what was the molarity of the 200 mL of HCl used?