Presentation is loading. Please wait.

Presentation is loading. Please wait.

Solutions.

Published byArmando Dreer Sales Modified over 6 years ago

Similar presentations

Presentation on theme: "Solutions."— Presentation transcript:

1 Solutions

2 1. SOLUTION homogeneous mixture of two or more substances solute
solvent substance in a small amount substance in a large amount N gas phase O2 (air) Ag solid phase Au (alloys) H2O liquid phase NaCl (sea water)

3 iodine in ethyl alcohol (C2H5OH)
EXP1 iodine in ethyl alcohol (C2H5OH) does not conduct electricity (molecular solid) I2 EXP2 table salt in water (H2O) does conduct electricity (ionic solid) Na+Cl- EXP3

4 AQUEOUS SOLUTION solute water (H2O) solutes
solution conducts electricity solution does not conduct electricity electrolytes non-electrolytes

5 solution conducts electricity solution does not conduct electricity
electrolytes non-electrolytes solution conducts electricity solution does not conduct electricity

6 non-electrolyte weak electrolyte strong electrolyte
ionic compounds (NaCl, KF) NaOH HCl H2SO4 methanol sugar ethanol water CH3COOH HCOOH HF dark medium bright

7 SOLUTION EXP4 concentration

8 GAS PHASE SOLUTION Saturn solvent H2/He solute CH4, PH3

9 LIQUID SOLUTION Europa solvent H2O solute MgSO4

10 SOLID SOLUTION Triton solvent N2 solute CH4

11 Components of Solutions
Component: a substance that is part of the solution Solvent: present in the greatest amount Solute: other than solvent (lower amount)

12 Mixtures that are not Solutions
Colloids – appears to be a homogeneous mixture, but particles are much bigger, but not filterable. E.g. Fog, smoke, whipped cream, mayonnaise, etc. Suspension: larger particle sizes, filterable. E.g. mud, freshly squeezed orange juice.

13 Colloids Tyndall effect: ability of a Colloid to scatter light. The beam of light can be seen through the colloid.

14 Solubility and Solutions
Solubility: Amount of solute that dissolves in a solvent to produce a saturated solution. (Solubility often expressed in g/100 mL.) E.g g of I2 dissolved in 1000 g of H2O. Saturated solution: maximum amount of solute is dissolved in solvent. Trying to dissolve more results in undissolved solute in container.

15 Unsaturated solution: less than max
Unsaturated solution: less than max. amount of solute is dissolved in solvent. Supersaturation = more solute in solution than normally allowed; we call this a supersaturated solution.

16 Factors Affecting Solubility
Polar liquids tend to dissolve in polar solvents due to dipole-dipole and H-bonding interactions

17 Factors Affecting Solubility
Polar liquids tend to dissolve in polar solvents due to dipole-dipole and H-bonding interactions CH3CCH3 acetone || O CH3CH2OH ethanol Miscible: soluble in all proportions (liquids) Immiscible: do not dissolve in one another

18 Salt Dissolving in Water

19 Factors Affecting Solubility
Nonpolar liquids tend to be insoluble in polar liquids; e.g. hexane (C6H14) does not dissolve in water. Increasing the nonpolar character of a substance will decrease its solubility in water.

20 Solubility: Temperature Dependence
All solubilities are temperature dependent; Most solids are more soluble at higher temperatures. All gases are less soluble at higher temperatures.

21 Factors Affecting Solubility
Temperature Effects

22 Factors Affecting Solubility
Temperature Effects

23 Ways of Expressing Concentration
Concentration: intensive property that conveys the amount of solute relative to the amount of either solvent or solution Qualitative ways: Dilute Concentrated Quantitative ways: Numeric representation Several ways

24 Units of Concentration
Molarity Weight (mass) Percent (wt%) parts per million (ppm) and parts per billion (ppb) for small concentrations.

25 Molarity Convenient way to prepare solution in lab
1-L flask ( mL) Convenient way to prepare solution in lab add 0.5 mol solute dilute to mark get 0.5 M solution

26 Example How many grams of sulfur Hydride (H2S) must be dissolved in water to make 1L of a 0.12 M solution?

27 Example How many grams of sulfur Hydride (H2S) must be dissolved in 1L of water to make a 0.12 M solution? 0.12 mol x ( g/1 mol) = 4.09g= 4.1 Dissolve in enough water to make 1 litre

28 Parts per Million (ppm) and Parts per Billion (ppb)
= = 0.25 part per part

29 Mass percentage e.g. Solution of HCl that is 36% by mass contains 36 g of HCl for every 100 g solution

Download ppt "Solutions."

Similar presentations

Solutions & Concentration. Water  Polar molecule w/ polar bonds  Causes surface tension & ability to dissolve polar molecules and ionic compounds.

Solutions & Concentration. Water  Polar molecule w/ polar bonds  Causes surface tension & ability to dissolve polar molecules and ionic compounds.
SOLUTIONS Chapter 15.

SOLUTIONS Chapter 15.
Solution Chemistry (Chp. 7)

Solution Chemistry (Chp. 7)
Chapter 15 Solutions Chemistry B2A. Mixture: is a combination of two or more pure substances. Homogeneous: uniform and throughout Air, Salt in water Heterogeneous:

Chapter 15 Solutions Chemistry B2A. Mixture: is a combination of two or more pure substances. Homogeneous: uniform and throughout Air, Salt in water Heterogeneous:
II III I C. Johannesson The Nature of Solutions Solutions.

II III I C. Johannesson The Nature of Solutions Solutions.
Let’s study solutions Solutions homogeneous mixtures of two or more substances solvent & one or more solutes Solutes spread evenly throughout cannot separate.

Let’s study solutions Solutions homogeneous mixtures of two or more substances solvent & one or more solutes Solutes spread evenly throughout cannot separate.
Chapter 12-13: Mixtures and Aqueous Solutions What are they? Where do we find them? How do we describe them? We use solutions all the time.

Chapter 12-13: Mixtures and Aqueous Solutions What are they? Where do we find them? How do we describe them? We use solutions all the time.
1 Chapter 7: Solutions and Colloids. 2 SOLUTIONS Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms,

1 Chapter 7: Solutions and Colloids. 2 SOLUTIONS Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms,
Solutions. Classification of Matter Solutions are homogeneous mixtures.

Solutions. Classification of Matter Solutions are homogeneous mixtures.
Types of Mixtures, Rates of Solubility, and Molarity/Molality

Types of Mixtures, Rates of Solubility, and Molarity/Molality
Solutions CH 13. Two Types of Mixtures Homogeneous Same throughout, looks pure EX: Air Heterogeneous Different throughout EX: Sand.

Solutions CH 13. Two Types of Mixtures Homogeneous Same throughout, looks pure EX: Air Heterogeneous Different throughout EX: Sand.
NOTES: 16.1-16.2 – Solutions and Concentration.

NOTES: – Solutions and Concentration.
What Are Solutions? Solution: homogeneous mixture of 2 or more substances Solution: homogeneous mixture of 2 or more substances –Solid, liquid, or gas.

What Are Solutions? Solution: homogeneous mixture of 2 or more substances Solution: homogeneous mixture of 2 or more substances –Solid, liquid, or gas.
SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)

SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)
Classifications of Mixtures Heterogeneous Mixtures—composed of different types of phases of substances - ex: Fruit salad Granite Homogeneous Mixtures—the.

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 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 Chapter 14.
Types of Mixtures Solutions Suspensions Colloids.

Types of Mixtures Solutions Suspensions Colloids.
Solutions CPS Chemistry. Definitions  Solutions A homogeneous mixture of two or more substances in a single phase  Soluble Capable of being dissolved.

Solutions CPS Chemistry. Definitions  Solutions A homogeneous mixture of two or more substances in a single phase  Soluble Capable of being dissolved.
CHAPTER 13 SOLUTIONS. BASIC DEFINITIONS Solution Solution – a homogeneous mixture of 2 or more substances in a single phase Solute – The dissolved substance.

CHAPTER 13 SOLUTIONS. BASIC DEFINITIONS Solution Solution – a homogeneous mixture of 2 or more substances in a single phase Solute – The dissolved substance.

Similar presentations

Ads by Google