Solutions: Concentration Chapter 14. Solution  Homogenous mixture of 2 or more substances in single phase  = 1 layer  Component present in largest.

Slides:



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

SOLUTIONS Chapter 15.
Physical Properties of Solutions Chapter 12 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
SOLUTIONS Chapter 15. What are solutions?  Homogeneous mixtures containing two or more substances called the solute and the solvent  Solute- is the.
Chem 106, Prof. T.L. Heise 1 CHE 106: General Chemistry u CHAPTER THIRTEEN Copyright © Tyna L. Heise All Rights Reserved.
Chapter 15 Solutions.
Physical Properties of Solutions
Solutions Chapter 13 and 14 Honors Chemistry. Solution Definition: a homogeneous mixture of 2 or more substances in a single physical state Definition:
Chapter 13 Solutions. Overview Solution Process energy changes, solution formation, chemical reactions Concentration mole fraction, molarity, molality,
To go with Chapter 13: Silberberg Principles of General Chemistry
Chapter 18 Solutions. I. Solutions A. Characteristics of solutions 1. Homogeneous mixture 2. Contains a solute and solvent 3. Can be a gas, liquid or.
Solutions Chapter 16 Copyright © The McGraw-Hill Companies, Inc.
SOLUTIONS SUROVIEC SPRING 2014 Chapter 12. I. Types of Solution Most chemical reaction take place between ions/molecules dissolved in water or a solvent.
Solutions Chapter 16. Desired Learning Objectives 1.You will be able to describe and categorize solutions 2.You will be able to calculate concentrations.
Physical Properties of Solutions.  Homogeneous mixtures: ◦ Solutions – ions or molecules (small particles) ◦ Colloids – larger particles but still uniform.
SOLUTIONS A homogeneous mixture in which the components are uniformly intermingled.
Solutions Solution: Homogeneous mixture, a mixture in which the components are uniformly intermingled. Solvent: Substance present in the largest amount.
CH 11: Properties of Solutions
SOLUTIONS AND SOLUBILITY. DEFINITIONS A solution is a homogeneous mixture A solute is dissolved in a solvent.  solute is the substance being dissolved.
Prentice Hall ©2004 CHAPTER 11 SOLUTIONS AND THEIR PROPERTIES Chapter 11Slide 1.
Solutions Ch.12 & 13. Liquids Condensed States Liquids and Solids Liquids and Solids Higher densities Higher densities Slightly compressible Slightly.
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.
C h a p t e r 11 Solutions and Their Properties. Kinds of Solutions01 Kind of SolutionExample Gas in gasAir (O 2, N 2, Ar …) Gas in liquidCarbonated water.
Chapter 18 Solutions. Liquids Miscible means that two liquids can dissolve in each other –water and antifreeze, water and ethanol Partially miscible-
Properties of Solutions
Chemistry 102(01) Spring 2002 n Instructor: Dr. Upali Siriwardane n n Office: CTH 311 Phone n Office Hours: n 8:00-9:00.
Physical Properties of Solutions Chapter 12. A solution is a homogenous mixture of 2 or more substances The solute is(are) the substance(s) present in.
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.
1 SOLUTIONS A N I NTRODUCTION. 2 Objectives 1. What are different ways of expressing the concentration of a solution? When is each used?
Section 13.1 Quantitative Expressions of Concentration Bill Vining SUNY Oneonta.
Prentice Hall © 2003Chapter 13 Hlanganani Tutu, C403 School of Chemistry
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.
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.
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.
Types of Mixtures Solutions Suspensions Colloids.
Chapter 13: Solutions Types of Solutions Mixture A blend of 2 or more kinds of matter, each of which retain its own identity & properties. Solution.
SOLUTIONS Chapter 13 and 14.
Ch. 13/14: Solutions Describing a Solution’s Composition.
Name & describe each of the 7 crystal structures.
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.
Why is salt spread on the roads during winter?. Ch 18 Solutions  Properties of Solutions  Concentrations of Solutions  Colligative Properties of Solutions.
SOLUTIONS SUROVIEC SPRING 2015 Chapter 12. I. Types of Solution Most chemical reaction take place between ions/molecules dissolved in water or a solvent.
1 Solutions 2 Does a chemical reaction take place when one substance dissolves in another? No, dissolving is a physical change because no new substances.
Chemistry Mrs. Nunez. Solution - Solution - homogeneous mixture Solvent Solvent - present in greater amount Solute Solute - substance being dissolved.
SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)
Unit # 4 Colligative Properties.. Colligative Properties - Properties that depend on the concentration of solute molecules or ions in solution, but do.
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.
Heterogeneous Mixtures Heterogeneous Mixtures: Not evenly blended Suspensions: a mixture containing particles that settle out if left undisturbed Colloids:
Solutions Mixtures: - Heterogenous Mixture: substances that make up the mixture are not spread uniformly throughout the mixture. - Homogenous Mixture:
Chapter 15: Solutions. Solutions Solution – a homogeneous mixture of two or more substances in a single physical state. Solution – a homogeneous mixture.
Physical Properties of Solutions Honors Unit 10. Solutions in the World Around Us.
CHAPTER THREE (12) Physical Properties of Solutions
CHAPTER 16 - SOLUTIONS Jennie L. Borders. SECTION 16.1 – PROPERTIES OF SOLUTIONS  Solutions are homogeneous mixtures that can be solids, liquids, or.
Physical Properties of Solutions Chapter 12 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Classifications of Mixtures Heterogeneous Mixtures—composed of different types of phases of substances - ex: Fruit salad Granite Homogeneous Mixtures—the.
Chapter 14 Solutions. What are solutions? A Solution is…
SOLUTIONS Chapter 15. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)
Solutions Textbook Chapter 14. Definitions n A solution is a homogeneous mixture n A solute is dissolved in a solvent. –solute is the substance being.
Properties of Solutions
Solutions Chapter 16.
Chapter 18 - Solutions.
Properties of Solutions
A homogeneous mixture in which the components are uniformly mixed
Solutions Details.
Presentation transcript:

Solutions: Concentration Chapter 14

Solution  Homogenous mixture of 2 or more substances in single phase  = 1 layer  Component present in largest amt = solvent  Other component(s) = solute  Alloys, air are all solutions (solns)

Colligative properties  = change of mp, bp, osmotic pressure of soln, change in vapor pressure  Irrespective of solute identity  Dependent on concentration

Concentration  Molarity (M) = moles solute/L of solution = mol/L  We’re all familiar with this  Drawback  won’t give you proper amount of solvent used to make soln  Molality (m) better

Problem  Give the concentration (in M) of grams of NaCl in 545 mL of water  MW of NaCl = g/mol

Molality  Molality (m) = moles solute/kg of solvent  Let’s look to the right   molality  molarity

Problem  Give the concentration (in m) of grams of NaCl in 545 mL of water  Density of 25°C = g/mL  MW of NaCl = g/mol

Mole fraction  Mole fraction of A (X A ) = n A /n tot  Amt of component A/total components  Soln contains 1.00 mol ethanol and 9.00 mol water

Weight percent  Ex: 46.1 g ethanol & 162 g water  Commonly used in household products like vinegar & bleach

Problem Concentrated sulfuric acid has a density of 1.84 g/cm 3 and is 95.0% (w/w) H 2 SO 4. MW H 2 SO 4 = g/mol.   Calculate the molarity and the molality of this solution.

Solution: molarity

Solution: molality

Problem A 10.7 molal solution of NaOH has a density of 1.33 g/cm 3 at 20°C. MW NaOH = g/mol & MW H 2 O = g/mol.   Calculate the mole fraction of NaOH, the weight percentage of NaOH and the molarity of the solution.

Solution

More practice  An aqueous soln of NaCl is created using 133 g of NaCl diluted to a total soln volume of 1.00 L.  Calculate the molarity, molality, and mass percent of the soln, given a density of 1.08 g/mL and MW of NaCl = g/mol.

Solution

Part per million  = PPM (in grams)  Ex: 1.0 ppm = 1.0 g of substance in system w/ 1.0 million g total mass STP water density  1.0 g/mL  So, mg/L and ppm are   Used predominately by environmental and analytical chemists

Solution process  One can add only so much solute to solvent  Since no more dissolves  soln said to be saturated  NaCl = 35.9 g/100 mL water (25°C)  Albeit, nothing changes visually, soln is constantly dissolving and re-solidifying ions

Solution process  Essentially, solubility = solute concentration in equilibrium w/undissolved solute in saturated soln  Unsaturated soln = soln w/less than saturated amt of solute  NaCl < 35.9 g/100 mL water (25°C)  Supersaturated soln = soln w/more solute than sat. soln  NaCl > 35.9 g/100 mL water (25°C)

Making supersaturated solutions  Pour in excessive amount of solute  Heat up the soln  Stir until all solute dissolves  Cool it slowly  No shaking, no jarring of soln  Gives lower freezing point  Once disturbed (energy in), causes crystallization to occur  excess crystallized out of soln  Exothermic  Heat packs of sodium acetate (can reach 50°C!)  heatpack.html heatpack.html heatpack.html  Your second lab deals with this

Liquids as solutes  Miscible = mixable  Immiscible = unmixable  Used in language too:  Mestizo, mischling  Ability to dissolve based on similar polarities (or lack thereof) of solute/solvent  Like dissolves in like

Let’s try these   Considering intermolecular forces, give reasons for the following observations:   a) Octane, C 8 H 18, is very miscible with CCl 4.   b) Methanol, CH 3 OH, mixes in all proportions with water.   c) Sodium bromide is not very soluble in diethyl ether (CH 3 CH 2 —O—CH 2 CH 3 ).   d) Octanol, C 8 H 17 OH, is not very soluble in water.