Solutions and Solubility Notes

I. Solutions

A. Solutions are also known as homogeneous mixtures.

(mixed evenly; uniform)

I. SolutionsB. Solute – the part of a

solution that dissolves.C. Solvent – the part of a

solution that dissolves the solute

D. Ex: Salt is the solute in salt water since the salt is dissolved.

I. SolutionsE. Substances may dissolve in water by dissociation, dispersion, and ionization.

F. For a solute to dissolve, the solute and solvent must attract.

I. Solutions

G. Dissociation is the process where ionic compounds separates into its ions.

•Ex. NaCl will separate into Na+ and Cl- ions when dissolved in water

I. SolutionsH. Ionization is the process where neutral atoms gain or lose electrons.

I. Ionization differs because it is a chemical process; new substances are formed.

I. SolutionsH. Dissolving is a physical process

(no change in composition; no reaction).

I. Ionic compounds conduct electricity when dissolved in water. (charges are free to move)

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Substances that dissolve are called soluble.Ex) sugar is soluble in water

Substances that do not dissolve are called insoluble.Ex) oil is insoluble in water.

II. Properties of Liquid Solutions

A. Three properties of a solutions that may differ from the solute and solvent are: conductivity, freezing point, and melting point

II. Properties of Liquid Solutions

B. A solution of sodium chloride conducts electricity because ions are able to move freely.

C. Adding salt to wet roads decreases the freezing point of water.

II. Properties of Liquid Solutions

D. Adding ethylene glycol to a car’s radiator increases the boiling point of water. (prevents overheating)

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III. Rates of Dissolving

A. Three factors that affect the rate of dissolving are: surface area, stirring/shaking, and temperature.

III. Rates of Dissolving

B. Increasing the surface area results in more collisions between solute and solvent particles. This increases the rate of dissolving.

III. Rates of Dissolving

C.You can increase the surface area by using smaller particles of solute.

Ex. Small grains of sugar have more surface area than a sugar cube.

III. Rates of DissolvingD. Stirring increases the rate of dissolving due to more collisions between solute and solvent particles.

E. Increasing the temperature causes the particles to move faster, which results in more collisions.

IV. Solubility

A.Solubility is the maximum amount of solute that will dissolve in a given amount of solvent.

IV. SolubilityUnsaturated solutions do not have the maximum amount of solute; may dissolve more.

Saturated solutions contains as much solute as can be dissolve.

IV. Solubility

Supersaturated solutions have more solute than can be dissolved.

IV. Solubility

C.Factors that affect solubility include polarity, temperature, and pressure.

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The basic rule for dissolving is “like dissolves like”.

Polar substances like water will only dissolve other polar substances.

Water cannot dissolve nonpolar substances like oil.

Water is referred to as the universal solvent since it can dissolve so many different substances.

IV. Solubility

Generally solubility of solids increases as the temperature increases.

Gases are generally more soluble at lower temperatures.

IV. Solubility

Increasing the pressure on a gas increases its solubility.

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Vocab Notes Begin Here

Notes for Concentration

Concentrated solutions contain a larger amount of solute.

Dilute solutions contain a smaller amount of solute.

Concentrations are commonly expressed by volume, weight, or Molarity.

Notes for Acid• Acids produce hydronium ions

(H3O+) when dissolved in water.

* may also say hydrogen ions (H+)

• Properties of acids include sour taste, reactivity with metals, changing the color of an indicator.

Notes for Acids

• Acids are proton donors.

• Acids turn litmus paper red.

Notes for Base• Bases produce hydroxide

ions (OH-) when dissolved in water. • Properties of bases include

bitter taste, slippery feel, and change colors of indicators.

Notes for Base

Bases turn litmus paper blue.

Bases are proton acceptors.

Neutralization Notes

• The reaction between an acid and base is called neutralization and produces a salt and water.

Salt Notes

•Salts are formed when positive ions from an acid combine with negative ions from a base.

Salt Notes

Many different types of salt exist.

Table salt is one example. Sodium chloride.

Sodium ion is from a strong base, and the chloride ion comes from a strong acid.

pH NotesThe pH scale measures hydronium/hydrogen ion concentration.•Acids pH 0-7•Bases pH 7-14•Neutral pH exactly 7

•Strong acids have lower pH; stronger bases have higher pH.