Properties, Concentrations, and Dilutions. Solute and Solvent Solute is the substance being dissolved. Solvent is the substance doing the dissolving.

Slides:



Advertisements
Similar presentations
Solutions. Review of Properties of Water Is a polar molecule Has extensive hydrogen bonding Many of water’s unusual properties are due to hydrogen bonding.
Advertisements

Solutions.
SOLUTIONS Chapter 15.
Christopher G. Hamaker, Illinois State University, Normal IL
Chapter 18 Solutions. Section 18.1 Properties of Solutions l OBJECTIVES: – Identify the factors that determine the rate at which a solute dissolves.
Starter S-161 Define A.Saturated solution B.Miscible C.Supersaturated solution.
Solutions C-16 Properties of solutions Solutions … Mixture (but special)  Solute + solvent Homogeneous (molecular level) Do not disperse light.
Inquiry Activity Things that determine how fast a substance will dissolve 1. Stirring (agitation) 2. temperature 3. surface area of the dissolving particles.
Concentrations of Solutions
Unit 10 Review Describe the following terms Solution Solvent Solute Soluble Insoluble Miscible Immiscible Homogeneous mixtures of 2 or more substances.
Chapter 16 Solutions Killarney High School. Section 16.1 Properties of Solutions l OBJECTIVES: – Identify the factors that determine the rate at which.
Slide 1 of 46 © Copyright Pearson Prentice Hall Concentrations of Solutions > Molarity The _________________ of a solution is a measure of the amount of.
15 Solutions Section 2 Describing Solution Composition.
Chemistry 16.2.
Slide 1 of 39 Chemistry © Copyright Pearson Prentice Hall Properties of Solutions > Slide 2 of 39 Solution Formation What factors determine the.
Solutions and their Behavior Chapter Identify factors that determine the rate at which a solute dissolves 2. Identify factors that affect the solubility.
Solution Formation The compositions of the solvent and the solute determine whether a substance will dissolve. The factors that determine how fast a substance.
Chapter 16 Properties of Solutions 1. Solution Formation Solutions are homogeneous mixtures that may be solid, liquid, or gaseous. The compositions of.
End Show © Copyright Pearson Prentice Hall Slide 1 of 46 Concentrations of Solutions Water must be tested continually to ensure that the concentrations.
Chapter 16 Solutions 16.2 Concentrations of Solutions
Properties of Solutions.   compositions of both the solvent and the solute determine whether a substance will dissolve (like dissolves like).  Stirring.
Solutions. Parts of Solutions b Solution- b Solution- homogeneous mixture. b Solute b Solute- what gets dissolved. b Solvent b Solvent- what does the.
Chapter 16 Properties of solutions. Making solutions l A substance dissolves faster if- l It is stirred or shaken. l The particles are made smaller. l.
Solubility and Concentration Chemistry Mrs. Coyle.
II III I I. The Nature of Solutions Solutions. A. Definitions  Solution -  Solution - homogeneous mixture Solvent Solvent - present in greater amount.
Solutions Chapter 14. solution Homogeneous mixture of 2 or more substances in a single physical state –particles in a solution are very small –particles.
NOTES: – Solutions and Concentration.
16.1 Properties of Solutions
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)
Properties of Solutions There are many factors that affect whether a substance will dissolve and the rate at which it dissolves.
Chapter 16 Solutions. Section 16.1 Properties of Solutions l OBJECTIVES: – Identify the factors that determine the rate at which a solute dissolves.
Chapter 16 “Solutions”.
Solutions Chapter 13 & 14. Solution  A uniform mixture that may contain solids, liquids, or gases  Also called a homogeneous mixture  Composed of a.
Solutions Chapter 14.
Solutions The composition of the solvent and the solute determine whether a substance will dissolve. Stirring, temperature, and surface area of dissolving.
Chapter 15 Solutions. 1.To understand the process of dissolving 2.To learn why certain substances dissolve in water 3.To learn qualitative terms describing.
1 Properties of Solutions Chapter Learning Objectives? What solubility is and how it is determined Recognize various levels of saturation and.
Chapter 16.  A sinkhole forms when the roof of a cave weakens from being dissolved by groundwater and suddenly collapses. One recorded sinkhole swallowed.
Solutions. Classification of Matter Solutions are homogeneous mixtures.
Solutions. Classification of Matter Solutions are homogeneous mixtures.
Why is salt spread on the roads during winter?. Ch 18 Solutions  Properties of Solutions  Concentrations of Solutions  Colligative Properties of Solutions.
Properties of Solutions A Solution l A solution is made up of a solute and a solvent. l The solvent does the dissolving. l The solute is the substance.
Chapter 16: Solutions 16.1 Properties of Solutions.
SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)
Solutions Mixtures: - Heterogenous Mixture: substances that make up the mixture are not spread uniformly throughout the mixture. - Homogenous Mixture:
Solutions. Solution Formation The compositions of the solvent and the solute determine whether a substance will dissolve. The factors that determine how.
Chapter 16 “Solutions”. Properties of Solutions l OBJECTIVES: – Identify the factors that determine the rate at which a solute dissolves.
CHAPTER 16 - SOLUTIONS Jennie L. Borders. SECTION 16.1 – PROPERTIES OF SOLUTIONS  Solutions are homogeneous mixtures that can be solids, liquids, or.
Chapter 16 “Solutions”. Solution formation l The “nature” (polarity, or composition) of the solute and the solvent will determine… 1. Whether a substance.
Solutions Chapter 14 Dr. Schuerch. Properties of Solutions Solution Formation –Solutions are homogeneous mixtures that may be solid, liquid, or gas The.
Chapter 16- Solutions. Solutions Homogeneous mixtures Can be solid, liquid, or gaseous Contains: Solute: dissolved particles in a solution Solvent: dissolving.
SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)
Solutions Chapter 15.
Chemistry 16.2.
Chapter 16-Solutions.
Section 2 - Concentrations of Solutions
Chapter 16 “Solutions”.
Chapter 13 “Solutions”.
Solubility & Concentration
Solutions.
Solubility & Concentration
A dilute solution is one that contains a small amount of solute.
Making solutions What the solute and the solvent are
II. Solubility & Concentration
Solubility & Concentration
Part 1 Solutions.
Solubility & Concentration
Starter S-161 Define Saturated solution Miscible
A ______________ solution contains a ____________ amount of solute.
Presentation transcript:

Properties, Concentrations, and Dilutions

Solute and Solvent Solute is the substance being dissolved. Solvent is the substance doing the dissolving. Example: Salt and Water. We dissolve salt in water. Therefore, the salt is the solute and the water is the solvent. Why is water called the universal solvent? REVIEW

Forming a Solution The composition (what they are made out of) of the solvent and solute determine whether a substance will dissolve. How FAST will the substance dissolve? This depends on three things: 1. Stirring: Increase of decrease rate? 2. Temperature: Increase or decrease rate? 3. Particle Size: The more surface area exposed, the faster it will dissolve. PART 1: PROPERTIES OF SOLUTIONS

What amount of a substance will dissolve? Particles move from a solid into a solution. But how much can be dissolved? Solubility describes the amount of substance that can be dissolved by a certain quantity of a solvent at a certain temp and pressure until the solution becomes saturated. PART 2: SOLUBILITY

Different Types of Solutions: Saturated Solution: The maximum amount of solute that can be dissolved at a specific temp and pressure. Unsaturated Solution: A solution that contains less solute than required to be a saturated solution and a certain temp and pressure. Supersaturated Solution: contains more solute than it can theoretically hold at a given temperature. Miscible Solution: when two liquids will dissolve into one another. There is no separation. Immiscible: liquids that are not soluble in each other. You can tell if it is immiscible by observing layers. SOLUBILITY

Miscible Immiscible Oil and Water Water and Acetone

SOLUTIONS Supersaturated Solution

Learn how to make your own rock candy using Chemistry at home. (AKA Crystal Meth… Not really. Just kidding.) GOOD NEWS: BREAKING BAD FANS eo.about.c om/chemi stry/How- to-Make- Rock- Candy.htm

What do YOU think? What type of solution is being utilized? How are they making that solution? ROCK CANDY EXPLAINED

1. Temperature: Solubility of MOST substances increases as temperature increases. You can dissolve more solute in the solvent as you increase the temperature. Think about how we made our rock candy. EXCEPTION: Gas solubility increases as temperature decreases. FACTORS THAT AFFECT SOLUBILITY

2. Pressure: Changes in pressure doesn’t affect the solubility of solids and liquids, but it greatly influences the solubility of gases. As pressure increases, the solubility of gases also increases. Use Henry’s Law for calculations. S = solubility P = pressure Directly Proportional FACTORS THAT AFFECT SOLUBILITY

How would I describe solubility in terms of UNITS? Solubility is usually expressed in grams of solute per 100g of solvent. Example: 36g of sodium chloride in 100g of water at 25 degC. Examples in terms of saturation: If 36g of NaCl is added to 100g water, it will dissolve completely, but if I added 1 more gram of NaCl, only 0.2g of that will dissolve. Therefore, 36.2g of NaCl in 100g of water is a SATURATED solution. How would I make it super saturated?? SOLUBILITY OF SOLUTIONS

Concentration: a measure of the amount of solute that is dissolved in a given quantity of solvent. Dilute Solution: a weak concentration. Contains small amount of solute. Concentrated Solution: strong concentration. Contains a large amount of solute. PART 3: CONCENTRATIONS Dilute Concentrated

MOLARITY Moles of solute dissolved in 1 Liter of solution. CONCENTRATIONS

LET’S MAKE A SOLUTION Let’s determine the molarity of a solution that we make. Let’s start with 10 grams of sodium chloride and add it to a 1-L volumetric flask half filled with distilled water.

LETS MAKE A SOLUTION Swirl the flask carefully to dissolve the solute.

LETS MAKE A SOLUTION Fill the flask with water exactly to the 1-L mark. What is the concentration of the solution in molarity?

Answer: 0.171M

This will work with ANY volumetric flask. Big or small. We can then calculate the molarity (concentration) of our solution. LETS MAKE A SOLUTION How do we convert mL to L?

Find the number of moles of solute in a solution… WHAT IF YOU KNOW THE MOLARITY? We can also convert moles to grams.

Diluting a solution reduces the number of moles per unit volume. The number of moles of solute remains unchanged. Dilution equation: DILUTIONS

To prepare 100 ml of MgSO 4 from a stock solution of 0.171M NaCl, a student first measures 10 mL of the stock solution with a 10-mL pipet.

DILUTIONS She then transfers the 10 mL to a 100-mL volumetric flask.

DILUTIONS Finally, she carefully adds water to the mark to make 100 mL of solution. What is the final concentration?

Use M1 x V1 = M2 x V2 Answer:

Some volume measuring devices… Buret Graduated Cylinder Volumetric Flask Glass Pipets TO MEASURE VOLUME

DILUTION CALCULATION

These are not as common as molarity, but are used sometimes. Percent by volume: Percent by mass: PERCENT CONCENTRATIONS OF SOLUTIONS

Percent by volume: (volume/volume) PERCENT CONCENTRATION CALCULATIONS

Percent by mass: (mass/mass) Suppose you want to make a 2000g solution that has a 2.8% (m/m) concentration of glucose in water. How many grams of glucose should you use? PERCENT CONCENTRATION CALCULATIONS

Page 499 # 42, 44, 46, 48, 49a, 51, 52, 53a,b, 54a, 55a CLASS WORK