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How to calculate unknown concentration from titration - volumetric stoichiometry

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How to calculate unknown concentration from titration - volumetric stoichiometry

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Side link to decomposition of metal carbonates

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Side link to decomposition of metal carbonates

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SimpleChemConcepts - Online Chemistry Videos

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O Level Pure Chemistry. IP Chemistry: Thermal Decomposition of Metal Carbonates

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Compare
HCl vs CH₃COOH  (same basicity (monobasic), but different strength)
HCl vs H₂SO₄ (different basicity but similar strength)

Note:
-Often related to rate of reaction questions
-Check which is the limiting reactant

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Acidic and Basic oxides of non-metals and metals

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MEMORISE solubility table!

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1. Unreactive metals such as copper or silver (except copper can react with concentrated nitric acid)
2. Lead, barium and calcium do not react with sulfuric acid due to insoluble layer which forms and prevents further reaction. (remember solubility table!)

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The salt is produced when H⁺ in the acid is replaced by a metallic ion (Na⁺, K⁺, Zn²⁺) to give hydrogen gas.

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https://www.youtube.com/watch?v=yirkozUyG74

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Neutralization reaction

The reaction of an acid and a base to form water is called a neutralization reaction.

When an acid and a base react, hydrogen ions from the acid (H⁺) and hydroxide ions from the base (OH ⁻) react in a 1:1 ratio to produce water. . At this time, if there are more hydrogen ions than hydroxide ions, it is acidic, if hydrogen ions and hydroxide ions are the same, it is neutral, and if hydrogen ions are less than hydroxide ions, it is basic. Therefore, the neutral point where the number of hydrogen ions and hydroxide ions are the same is where the neutralization reaction takes place, and this point is called the neutralization point.

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The reaction of an acid and a base to form water is called a neutralization reaction. When an acid and a base react, hydrogen ions from the acid (H+) and hydroxide ions from the base (OH -) react in a 1:1 ratio to produce water. .

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Dissociate completely in water to give hydroxide ions

eg. sodium hydroxide, potassium hydroxide

NaOH (aq) → Na+ (aq) + OH⁻(aq)

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Partially dissociate in water to give hydroxide ions

eg. aqueous ammonia, ammonium hydroxide

H₂O + NH₃  ⇌ OH− + NH₄⁺

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Monbasic
DIbasic
Tribasic
The basicity of an acid refers to the maximum number of hydrogen ions produced by a molecule of the acid in aqueous solutions.

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Basicity of Acids - Acids, Bases and Salts (CBSE Grade 07 Chemistry)

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due to free moving ions. Acids and alkalis make good electrolytes

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- turns red litmus paper blue
- bitter taste and soapy feel

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- turns blue litmus paper red
- sour taste and corrosive

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carbon dioxide, sulfur dioxide, nitrogen dioxide, sulfur trioxide, silicon(IV) oxide

Acid oxides react with bases and alkalis

Soluble in water to give acids

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NO, CO - non-metal oxides that do not dissolve in water and are commonly monoxides

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Zinc oxide, aluminium oxide, Lead(II) oxide
Remember (ZAL)
React with acids AND alkalis

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All metal oxides are basic as they react with acids.

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Bases are metal oxides and metal hydroxides. Most bases are insoluble. Soluble bases are alkalis.
Insoluble bases: MgO, CaO, ZnO, CuO, Al²O3,
Soluble bases: Na₂O, K₂O (all group I metal oxides)

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Eg. hydrochloric acid, sulfuric acid, nitric acid
H₂SO₄(aq)--> 2H⁺(aq)+SO₄ ²⁻(aq)

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Eg. Ethanoic acid
CH₃COOH ⇌ H⁺ + CH₃COO⁻

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Alkalis are soluble bases, KOH, NaOH, NH₃(aq)

Note: limewater or Ca(OH)₂ is partially soluble

ionises in water to produce hydroxide ions

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HCl, H₂SO₄, HNO₃, H₂SO₃, CH₃COOH

Ionise in water to give hydrogen ions