2.34: Know the Common Rules for Prediction the Solubility of Ionic Compounds in Water: Common Sodium, Potassium and Ammonium Compounds are Soluble, All Nitrates are Soluble, Common Chlorides are Soluble Except Those of Silver and Lead (II), Common Sulfates are Soluble, Except for those of Barium, Calcium and Lead (II), Common Carbonates are Insoluble, Except for those of Sodium, Potassium and Ammonium, Common Hydroxides are Insoluble Except for those of Sodium, Potassium and Calcium (Calcium Hydroxide is slightly Soluble)

SOLUBLE: When substance can dissolve in a given volume of solvent

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SOLUBILITY RULES:

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SOLUBLE	INSOLUBLE
All Sodium, Potassium and Ammonium	None
All Nitrates	None
Common Chlorides	Except for Silver and Lead (II)
Common Sulfates	Except for Barium, Calcium and Lead (II)
Except for Sodium, Potassium and Ammonium	Common Carbonates
Except for Sodium, Potassium and Calcium (Calcium Hydroxide is Slightly Soluble)	Common Hydroxides

2.35: Understand Acids and Bases in Terms of Proton Transfer

ACIDS AND BASES (ALKALIS)

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• When atoms or groups of atoms lose or gain Electrons, they form charged particles called Ions - either positively or negatively charged

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*ACIDS:

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• When Acids react, they will lose Electrons to form positive Hydrogen ions ( H+ )
• These H+ Ions make the Aqueous Solution Acidic

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    Example: Hydrochloric Acid

HCl (aq)   →    H+ (aq)    +    Cl- (aq)

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*BASES (ALKALIS):

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• When Alkalis react, they will gain Electrons to form negative Hydroxide ions ( OH- )
• These OH- ions make the Aqueous Solution an Alkali

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    Example: Sodium Hydroxide

NaOH (aq)   →    Na+ (aq)    +    OH- (aq)

2.36: Understand that an Acid is a Proton Donor and a Base is a Proton Accept

ACIDS AND BASES (ALKALIS)

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• When atoms or groups of atoms lose or gain Electrons, they form charged particles called ions - either positively or negatively charged

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Diagram:

       

Diagram showing the Role of Acids and Bases in the Transfer of Protons

*ACIDS:

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• Acids are Proton donors as they will react to lose Electrons to form positive H+ ions
• These H+ ions make the Aqueous Solution Acidic

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*BASES (ALKALIS):

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• Bases (Alkalis) are Proton acceptors as react to gain Electrons to form negative OH- ions
• These OH- ions make the Aqueous Solution Alkaline

2.37: Describe the Reactions of Hydrochloric Acid, Sulfuric Acid and Nitric Acid with Metals, Bases and Metal Carbonates (Excluding the Reactions Between Nitric Acid and Metals) to Form Salts

REACTING ACIDS WITH METALS

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Only Metals above Hydrogen in the reactivity series will react with Dilute Acids to form a Salt and Hydrogen Gas:

Acid    +    Metal   →    Salt    +    Hydrogen

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Examples of Reaction Between Acids and Metals:

ACID	NAME OF PRODUCTS	EQUATION FOR REACTION
HYDROCHLORIC ACID	Metal Chloride and Hydrogen	x   +   2HCl   →   xCl2   +   H2
SULFURIC ACID	Metal Sulfate and Hydrogen	x   +   H2SO4   →   xSO4   +   H2

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REACTING ACIDS WITH BASES (ALKALIS)

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Acids will react with Bases - all Metal Oxides and Metal Hydroxides, in a neutralisation reaction to produce a Salt and Water:

Acid    +    Base   →    Salt    +    Water

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Examples of Reaction Between Acids and Bases:

ACID	NAME OF PRODUCTS	EQUATION FOR REACTION
HYDROCHLORIC ACID	Metal Chloride and Water	xOH   +   HCl   →   xCl   +   H2O
SULFURIC ACID	Metal Sulfate and Water	xO   +   H2SO4   →   xSO4   +   H2O
NITRIC ACID	Metal Nitrate and Water	x(OH)2  +  HNO3  →  x(NO3)2  +  2H2O

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REACTING ACIDS WITH METAL CARBONATES

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Acids will React with Metal Carbonates to form Salts, Carbon Dioxide and Water:

Acid    +    Metal Carbonate   →    Salt    +    Carbon Dioxide    +    Water

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Examples of Reaction Between Acids and Bases:

ACID	NAME OF PRODUCTS	EQUATION FOR REACTION
HYDROCHLORIC ACID	Metal Chloride, Carbon Dioxide and Water	xCO3   +   2HCl   →   xCl2      +   CO2   +   H2O
SULFURIC ACID	Metal Sulfate, Carbon Dioxide and Water	xCO3   +   H2SO4   →   xSO4   +   CO2   +   H2O
NITRIC ACID	Metal Nitrate, Carbon Dioxide and Water	xCO3  +  HNO3  →  x(NO3)2  +   CO2   +   H2O

2.38: Know that Metal Oxides, Metal Hydroxides and Ammonia can Act as Bases, and that Alkalis are Bases that are Soluble in Water

ALKALI: Bases that are soluble in Water and dissolves to form Hydroxide ions (OH-)

                                Diagram showing the pH of Bases (Alkali)

Example: Metal Oxides

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Metal Oxides can act as a Base and is soluble in Water

Metal Oxide    +    Acid   →    Salt    +    Water

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Example: Metal Hydroxides

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Metal Hydroxides can act as a base and is soluble in Water

Metal Hydroxide    +    Acid   →    Salt    +    Water

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Example: Ammonia

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Ammonia can act as a base and is soluble in Water

Ammonia    +    Acid   →    Salt    +    Water