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Topic : IGCSE Acids, Base , And Salt

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Published in: Chemistry
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Here we will dixieland about acid , base and salt and preparation of salts

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  1. HEMISTRY WITH TOPIC GCSE CHEMISTRY ACIDS , BASE , AN SALYS CAMBRID AQA , OXFORD , EDXCEL S LABUS
  2. WG4AT uS ACAO? o- An acid is defined as a substance whose water solution tastes sour, turns blue litmus red, and neutralizes bases. ANY subtances that give H + ions taste is sour litmus paper turns red
  3. OF ACAOS Definition of Acids: Proton donors. @ Indicators Have a pH between 1 (strong) and 6 (weak) Turns blue litmus red Turns methyl orange indicator red Colourless in Thymolphthalein Weak and Strong Acids Strong acids: completely dissociated in aqueous solution producing lots of Ions @ e.g: HCI (aq) —9 (aq) + Cl- (aq) Weak acids: partially dissociated in aqueous solution producing few Hi ions @ e.g: CH3COOH (aq) Hi (aq) + CH3COO- (aq) Chemical properties Acid + metal salt + hydrogen gas Acid + base salt + water Acid + metal carbonate —+ salt + carbon dioxide + water
  4. WG4AT uS ? Bases: substances which neutralise acids to form salt and water only. Definition of Bases: They are proton acceptors (form OH ions) @ Indicators Have a pH between 8 (weak) and 14 (strong) Turns red litmus blue Turns methyl orange indicator yellow Turns Blue in thymolphthalein
  5. Weak and Strong Alkalis (Soluble Bases) Strong alkalis: completely dissociates in aqueous solution, producing lots of OH- ions e.g.: NaOH (aq) Na+ (aq) + OH- (aq) Weak alkalis partially ionize in water producing OH- ions e.g: NH40H (aq) e NH4+ (aq) + OH- (aq) Chemical properties Base + acid —+ salt + water (+ C02 when base is a metal carbonate) Base + ammonium salt salt + ammonia gas + water
  6. Neutral Neutral substances are pH 7. pH scale pH is the concentration of ions per dm3 of solution Universal indicator solution is used to determine the pH of a substance by matching the color change to the pH color chart. 2 increasingly acidic 14 neutral increasingly alkal ne
  7. Types of Oxides Metal oxides are basic, e.g. Copper oxide and Calcium oxide Non-metal oxides are acidic, e.g. sulfur dioxide and carbon dioxide Aluminium and zinc form amphoteric oxides, e.g. zinc oxide Oxides that react with neither acids nor bases are neutral, e.g. nitrous monoxide and carbon monoxide
  8. COLOUR OF TRANSATAONS METALS copper (Il) Sulfate Blue Copper (Il) Oxide Black Copper (Il) Carbonate GREEN Manganese (IV) Oxide Black @ Iron (Il) Salts @ Iron (Ill) Salts Pale Green Brown or Orange
  9. Method A: Soluble Salts from Excess Insoluble Bases (metal, metal oxide, carbonates) Warm acid (increases the speed of reaction) Add an excess reactant + stir Filter mixture Transfer to evaporating basin Heat using a Bunsen burner Leave to cool until crystallisation point Wash crystals with distilled water Dry crystals on filter paper
  10. MkT+qoos Method B: Titration Place a known volume of alkali into a conical flask using a volumetric pipette. Add indicator (e.g. thymolphthalein) Titration: add acid using a burette until the endpoint has reached Record the volume of acid added Repeat without indicator Transfer to evaporating basin Heat with Bunsen burner Leave to cool until crystallisation point Wash crystals with distilled water Dry crystals on filter paper
  11. TO PREPARE @ Insoluble Salts Precipitation: Insoluble Solid forms between two aqueous solutions. Mix two soluble salts Filter to remove the precipitate Wash the precipitate with distilled water Leave to dry
  12. WATER OF CRYSTALLASATAON ANO RULES Water of Crystallisation A salt is a compound formed when a metal replaces all the hydrogen atoms of an acid. Naming salts involves two parts: the name of the metal and the acid-ending eg. calcium + hydrochloric acid = calcium chloride The Water of Crystallisation is the water molecules present in hydrated crystals.

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