[PDF] [PDF] Review Chap 11 Phase diagrams Phase diagrams display the state

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Model 1: Phase Diagrams for Water and Carbon Dioxide 1 Liquid 2 See H2O diagram below The temperature is greater than the normal boiling point so 

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[PDF] Review Chap 11 Phase diagrams Phase diagrams display the state

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Review Chap 11 Phase diagrams

Phase diagrams display the state of a substance at various pressures and temperatures, and the places where equilibria exist between phases.

The solid - liquid line marks the

melting point at each pressure

The liquid - vapor line is the

boiling point at that pressure

The high critical temperature

and critical pressure are due to strong van der Waals forces between water molecules Phase Diagram of WaterInterpreting a Phase Diagram

Using the phase diagram for

methane CH 4

What is the temperature and

pressure of the critical point?

The critical point is where

the liquid, gaseous, and supercritical fluid phases coexist.

It is marked point 3 and is

approximately 80C and 50 atm.What is the temperature and pressure of the triple point

The triple point is the point

where the solid, liquid, and gaseous phases coexist. It is marked point 1 and is at

180 C and 0.1 atm

Is methane a solid, liquid, or

gas at 1 atm and 0 C?

The intersection of 0 C and

1 atm is marked point 2

It is in the gaseous regionIf solid methane at 1 atm is heated while the pressure is held constant, will it melt or sublime?

Starting at P = 1 atm and

moving horizontally, liquid region is reached at T180C

Then into the gaseous region,

at T160 C.

So, solid methane melts

In order for methane to

sublime, the pressure must be below the triple point pressureIf methane at 1 atm and 0 C is compressed until a phase change occurs, in which state is the methane when the compression is complete?

Moving vertically up from point

2,which is 1 atm and 0 C, the

first phase change we come to is from gas to supercritical fluid.

This phase change happens when

the critical pressure (~50 atm) is exceeded

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Chapter 13 Solutions and Their Properties

•SOLUBILITY RULES - Chapter 4 •SOLUBILITY- factors that affect - Pressure (HENRY'S LAW) - Temperature •CONCENTRATION - Molecular weight •COLLIGATIVE PROPERTIES - Molecular solutions - Ionic solutions •COLLOIDS

Solutions, Mixtures, & Colloids

(a) A MIXTURE is heterogeneous (b) A SOLUTION is homogeneous (c) A colloidal dispersion is between a solution and a mixture

Types of Aqueous Solutions

•ELECTROLYTE- A substance that dissolves in water to produce IONS

Example: HCl(aq), NaOH(aq), NaCl(aq)

•NON ELECTROLYTEA substance that

DOES NOT produce IONS, remain as

molecules, when dissolved in water.

Example: sugar

Which of the following will be water soluble

NaCl AgCl CH 3 OH CH 3 Cl CCl 4

Yes - all sodium salts are water soluble

No - Silver, Mercury & Lead are not

water soluble

Yes - "Like water" {polar compound

Yes - "Like water" {polar compound

No - Not "Like water" { not polar

What is in an aqueous solution of

NaCl MgI 2 Al(NO 3 3 HClO 4 (NH 4 2 SO 4 Na (aq) + Cl (aq) Mg 2+ (aq) + 2 I (aq) Al 3+ (aq) + 3 NO 3- (aq) H (aq) + ClO 4- (aq) 2NH 4+ (aq) + SO 42-
(aq)

Classify each of the following as a heterogeneous

mixture or homogeneous mixture (a solution).

Air .........................

Tomato juice ............

Iodine crystals ...........

Mud .....................

18 Carat White Gold ...Mixture (homogeneous)

Mixture (heterogeneous)

Pure substance

Mixture (heterogeneous)

Mixture (homogeneous)

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Predicting Solubility Patterns

Predict whether each of the following substances is more likely to dissolve in the nonpolar solvent carbon tetrachloride (CCl 4 ) or in water: C 7 H 16 Na 2 SO 4 HCl I 2 a hydrocarbon, so it is molecular and nonpolar. therefore more soluble in the nonpolar CCl 4 a compound containing a metal and nonmetals, is ionic therefore more soluble in polar water a polar diatomic molecule therefore more soluble in polar water a nonpolar diatomic molecule therefore more soluble in the nonpolar CCl 4

Expressing Concentration (based on weight)

1 2 3 2

10 of %xsolutionofweightsoluteweightweight

6

10 of xsolutionofweightsoluteweightppm

9

10 of xsolutionofweightsoluteweightppb

Mole Fraction (x) , Molarity (M)

and Molality (m) moles of number Total

Aof Moles

A X

SOLUTION ofLiterssolute of MolesMolarity

SOLVENT of Kilogramssolute of Moles=Molality

A solution is made by dissolving 4.35 g glucose

(C 6 H 12 O 6 ) in 25.0 mL of water at 25 C. Calculate the molalityof glucose in the solution. (25.0 mL of water)(1.00 g/mL) = 25.0 g = 0.0250 kg solvent

A solution with a density of 0.876 g/mL contains

of toluene (C 7 H 8 ) and 225 g of benzene. Calculate the molarityof the solution The volume of the solution is obtained from the massquotesdbs_dbs14.pdfusesText_20