Acids and bases
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Transcript of Acids and bases
Acids and BasesBy: Faiq & Rizan
AcidsProduce H+ ions in water
Have a sour taste
Break down metals
Formula starts with H
Poisonous and corrosive to skin
pH less than 7
Acidturn blue litmus red
Dissolve in water to form solution which conduct electricity
React with reactive metal metals to form salt and hydrogen (explained)
Acids react with carbonates and hydrogen carbonates to form a salt, water and carbon dioxide (explained)
Acids react with metal oxides and hydroxides to form a salt and water only(explained)
AlkalisProduce OH- ions in water
Have a bitter taste and a slippery feel
Break down fats and oils
Formula ends with OH
Poisonous and corrosive to skin
pH greater than 7
Alkalisturn red litmus blue
React with acids to form salt and water only.(explained)
Heated with ammonium salts gives off ammonia gas.(explained)
React with a solution of one metal salt to give another metal salt and metal hydroxide.(explained)
pH scale
Acid have pH of <7
Alkalis have pH of >7
Theories of acids and bases
Arrhenius Concept of Acids and Bases
According to the Arrhenius concept of acids and bases, an acid is a substance that, when dissolved in water, increases the concentration of hydronium ion (H3O+).
Remember, however, that the aqueous hydrogen ion is actually chemically bonded to water, that is, H3O+.
Arrhenius Concept of Acids and Bases
A base, in the Arrhenius concept, is a substance that, when dissolved in water, increases the concentration of hydroxide ion, OH-(aq).
Bronsted-Lowry Acid and Bases
Bronsted-Lowry Acid can donate a proton
Bronsted-Lowry Base can accept a proton
Must contain a non-bonding pair of electrons
Conjugate base of an acid is the species remaining after the acid has lost a proton
Bronsted-Lowry Acid and Bases
Conjugate acid is the species formed after the base has accepted a proton
HCl + H2O ↔ H3O+ + Cl-
Water is conjugate base of H3O+ and Cl- is conjugate base of HCl
Bronsted-Lowry Acid and Bases
Water can act both as acid and base. Amphiprotic
Strong acids have weak conjugate base
Weak acids have strong conjugate base
ACID: Ethanol (C2H5OH) =>weak
CONJUGATE BASE: Ethoxide ion (C2H5O-) => strong
Lewis Acids and Bases
Bases can donate a pair of electrons
Acids can accept a pair of electrons
Covalent bond is formed
Many Lewis Acids don’t contain hydrogen
Properties of Acids and Bases
Properties of Acids and Bases
Neutralization reaction with bases
With hydroxides to form salt and water
CH3COOH + NaOH NaCH3COO + H2O
With metal oxides to form a salt and water
H2SO4 + CuO CuSO4 + H2O
With ammonia to form salt
HCl + NH3 NH4Cl
Properties of Acids and Bases
With reactive metals to form salt and hydrogen
2HCl + Mg MgCl2 + H2
With carbonates to form salt, CO2, water
2HCl + CaCO3 CaCl2 + CO2 + H2O
With hydrogen carbonates to form salt, CO2, water
HCl + NaHCO3 NaCl + CO2 + H2O
Strong Acids and Bases
Strong acid and base is completely dissociated (ionized) into its ions in aqueous solutions
Strong acids
HCl (Hydrochloric acid)
HNO3 (Nitric Acid)
H2SO4 (Sulfuric Acid)
Strong Acids and Bases
Strong bases
NaOH (Sodium Hydroxide)
KOH (Potassium Hydroxide)
Ba(OH)2 (Barium Hydroxide)
Weak Acids and Bases
Weak acids and bases is slightly dissociated into their ions in aqueous solution
Weak acids
CH3COOH (Ethanoic Acid)
H2CO3(Carbonic acid)
Weak Acids and Bases
Weak bases
NH3 (Ammonia)
C2H5NH2 (Amino ethane)
Acidic oxides
Acidic oxides are the oxides of non-metals. When combined with water, they produce acids, e.g.,
Acidic oxides are, therefore, known as acid anhydrides, e.g., Sulphur dioxide is sulphurous anhydride; Sulphur trioxide is sulphuric anhydride.
Basic oxides
Basic oxides are the oxides of metals. If soluble in water they react with water to produce hydroxides (alkalis).
Basic oxides do not reacts with alkalis.
Examples:
CaO + H2O Ca(OH)2
MgO + H2O Mg(OH)2
Amphoteric oxides
Amphoteric oxides are metallic oxides, which show both basic as well as acidic properties. When they react with an acid, they produce salt and water, showing basic properties. While reacting with alkalis they form salt and water showing acidic properties
Neutral oxides
These are the oxides, which show neither basic nor acidic properties, that is, they do not form salts when reacted with acids or bases, e.g., carbon monoxide (CO); nitrous oxide (N2O); nitric oxide (NO), etc., are neutral oxides.
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