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Solution and Solubility

Questions:

Properties of solutions?

Did the solute changed the properties of the solvent? how? which ones?

Colligative Properties

What are solutions

Solutions are homogeneous mixtures of two or more pure substances

Solute: is disperse evenly in the solvent. Solvent is the substance that dissolves and is in the greater amount.

What are solutions?

Check Point: Solvent and Solute

You make ice-tea:

Solvent: the solvent is the water

Solute: is the ice-tea powder

Sea water

solute vs solvent

Solvent: water

Solute: salts, minerals and other

Air is a homogeneous solution

what is the solvent, what is the solute?

Solvent: N2

Solute: O2, CO2, H2

Conclusion

A solution is made up of a solvent and a solute.

The solute dissolves in the solvent and it is the one with the smaller amount.

The Solvent is the one in the greater amount and does the dissolving.

A solution is an Homogeneous mixture where all substances are in the same phase.

Conclusion

A solution of CuSO4

SOLUBILITY

is the ability of a solute to dissolve in a solvent.

What is Solubility?

Can we influence Solubility?

FACTORS THAT AFFECT SOLUBILITY

PRESSURE

SURFACE AREA; SIZE OF PARTICLE

TEMPERATURE

FACTORS THAT AFFECT SOLUBILITY

NATURE OF SOLVENT/SOLUTE (POLARITY)

Stirring increases the speed of dissolving

FACTOR 1: Temperature

FOR SOLID SOLUTES:

AS TEMPERATURE INCREASES SOLUBILITY INCREASES

Temperature

For gas solutes:

as temperature increases solubility decreases

Factor 2:

Particle Size/Surface Area

the smallest the size of the particle the faster it will dissolve.

Surface Area

Particle Size

Big Crystal

Powder

Granulated

Factor 3: Pressure

Pressure only helps gases.

As pressure increases, it increases the solubility of gasses.

Pressure

LOW

HIGH

Factor 4: Polarity

Golden Rule: "Like dissolves like"

need a polar solvent to dissolve polar solutes.

Ionic dissolve in water. Non-polar solvent to dissolve a non-polar solute

Polarity of solute and solvent

Solvent Polar

needs polar solute

Non-polar solute

needs polar solvent

Ionic works best in Polar like water

Can you dissolve a styrofoam cup?

Polarity of solvent problems

Polystyrene

Factor 5: stirring

Stirring Increases solubility

Types of Solutions Based on Amount of Solute

Type of Solutions

https://www.slideshare.net/itutor/solution-solubility

Solubility Rules

SOLUBILITY RULES

Table on the left all substance containing ... are soluble except (exceptions are insoluble)

Soluble Compounds

Soluble

Insoluble Compounds

Insoluble

https://forms.gle/M5HydfN3J7B4nqgo7

Problems

  • Is ZnCl2 soluble or insoluble?
  • Is Potassium Nitrate Soluble or insoluble?
  • Is Calcium Carbonate soluble or insoluble?
  • Does ClO4- tend to form a precipitate?
  • Which of these substances is likely to form a precipitate?

a) CaSO4 b) table salt c) AgBr d) CuSO4

  • Predict whether a precipitate will form as a result of this reaction:

2AgNO3+Na2S→Ag2S+2NaNO

Solubility Curve Introduction

Terms:

unsaturated

saturated

super saturated

Solubility Curve

Problem

Problem

Determine if the solution is saturated, unsaturated or super saturated;

1. 18 grams of potassium nitrated dissolved in 100 ml of water at 20 C

2, 42 g of Potassium chloride in 100 g of water at 30 C

3. How much more is required to make a saturated solution of NaCl if you started with 12 g at 20 C?

SOLVENT

Solvents uses and benefits

the word solvent derives from a Latin word that means to loosen. You can find solvent in a variety of industries such as in paints, inks, cleaners, dry cleaning and medicine.

There are three main type of solvent:

  • Hydrogenated/organic
  • Oxygenated
  • Halogenated

Solubility rules can be used to predict precipitates in precipitation reactions

Examples: Predict the products of the following reaction and write the net ionic equation:

AgNO3 (aq) + KBr (aq) ==> AgBr (s) + KNO3 (aq)

NET IONIC: Ag(aq) +Br(aq) ==> AgBr (s)

Predicting Precipitates

Colligative Properties

  • Reduces the vapor pressure of the solvent in the solution.

  • Lowers the freezing point of the solution.

  • Raises the boiling point of the solution.

How do solutes affect the properties of solutions?

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