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Acids, bases and salt preparations
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ACIDS, BASES AND SALT PREPARATIONS SOLUBILITY RULES Soluble Compounds of sodium, potassium, and ammonium Acid All nitrates PROTON TRANSFER ACIDS: All chlorides, except... All sulfates except... Sodium, potassium, and ammonium carbonates Zinc Iron Sodium, potassium, and calcium hydroxides ALKALIS: Acid • Proton donors • Proton acceptors Magnesium O-H Sulfuric acid DONOR (ACID) ionise in solution producing protons, Ht ions. HP ACCEPTOR (BASE) Insoluble ...silver and lead (II) ionise in solution producing OH ions which can accept protons. ...barium, calcium, and lead (II) REACTIONS OF ACIDS • only metals above hydrogen in the reactivity series will react with dilute acids. the more reactive the metal, the more vigorous the reaction. METAL + ACID SALT + HYDROGEN Hydrochloric Metal chloride and acid hydrogen All other carbonates Sulfuric Acid Mg + H₂SO, Zn + H₂SO, MgSO₂ + H₂ ZnSO₂ + H₂ FeSQ, + H₂ Fe + H₂SO, SUMMARY OF METALS WITH ACIDS All other hydroxides Metal sulfate and hydrogen CE HAS LOST A PROTON HO HAS GAINED A PROTON, FORMING HO Hydrochloric Acid Mg + 2HCL→→→→→ MgCl₂ + H₂ Zn +2HCL→→→→→ ZnCl₂ + H₂ Fe + 2HCL FeCl₂ + H₂ Name of products Equation for reaction M+2HCL >>> MCL₂ + H₂ M + H₂SO₂ →→→→MSO, + H₂ → Examples with HCL and H₂SO4 ACIDS + BASES (NEUTRALISATION) METAL HYDROXIDE + ACID SALT + WATER METAL OXIDE + ACID → SALT + WATER METAL CARBONATE + ACID →→ SALT + WATER + CO₂ AMMONIA (gas) + ACID → AMMONIUM SALT PREPARING SALTS (SOLUBLE) FROM AN INSOLUBLE BASE • Soluble salts can be prepared by reacting an acid with an insoluble base HEAT ACID IN WATER BATH ADD INSOLUBLE BASE IN EXCESS MIX 10...
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Alternative transcript:
REACT REMEMBER: the acid that you use HYDROCHLORIC ACID SULFURIC ACID NITRIC ACID o FILTER 10 REMOVE UNREACTED BASE will depend on what salt you want: CHLORIDE SALTS SULFATE SALTS NITRATE SALTS GENILY HEAL TO EVAPORATE WATER FROM AN ACID AND AN ALKALI • acids react with alkalis to form a salt and water →You cannot use an excess of one of the reactants because both reactants are solutions and cannot be separated by filtration. METHOD USING TITRATIONS O carry out a titration to work out precise volumes of aud and alkali needed for neutralisation to occur. LEAVE TO CRYSTALLISE WASH AND DRY 2 Mix the appropriate volumes of acid and alkali so that they react completely and we are left with a solution containing salt and water. USING TWO SOLUBLE SALTS • called a precipitation reaction Evaporate off the water by gently heating the solution and allow to cool so that the soluble salt will crystallise. Filter the solid salt, wash and dry. sulid, insoluble sall produced is the precipitate. EXAMPLE: Making Silver chloride J a soluble sall that contains Silver: Silver nitrate a soluble chloride sale: magnesium/sodium /potassium chloride. METHOD: Dissolve magnesium chloride in water (do the same with the silver nitrate) (2 add both solutions together and stir 3 a precipitate of silver chloride should form remove precipitate by filtration, wash and dry in an oven. PREPARATION OF COPPER (11) SULFATE FROM COPPER (11) CARBONATE METHOD: measure 25cm³ of dilute sulphuric acid into a beaker and add 25cm³ of distilled water. 22 Add a small spatula of copper (11) oxide, place on a tripod and gauze and warm gently whilst stirring. continue adding the solid until there is excess solid left over. •4 leave to cool and filter into an evaporating dish CRYSTALLISATION: the marking points I hear the solution to concentrate it by evaporating off about half the water or until crystals appear on a dipped glass rod leave the solution to cool and crystallise. filler to separate the crystals from solution. pat crystals dry with filter paper.
Acids, bases and salt preparations
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Detailed notes on this topic including the exact marking points for crystallisation 6 markers
Detailed notes on this topic including the exact marking points for crystallisation 6 markers
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ACIDS, BASES AND SALT PREPARATIONS SOLUBILITY RULES Soluble Compounds of sodium, potassium, and ammonium Acid All nitrates PROTON TRANSFER ACIDS: All chlorides, except... All sulfates except... Sodium, potassium, and ammonium carbonates Zinc Iron Sodium, potassium, and calcium hydroxides ALKALIS: Acid • Proton donors • Proton acceptors Magnesium O-H Sulfuric acid DONOR (ACID) ionise in solution producing protons, Ht ions. HP ACCEPTOR (BASE) Insoluble ...silver and lead (II) ionise in solution producing OH ions which can accept protons. ...barium, calcium, and lead (II) REACTIONS OF ACIDS • only metals above hydrogen in the reactivity series will react with dilute acids. the more reactive the metal, the more vigorous the reaction. METAL + ACID SALT + HYDROGEN Hydrochloric Metal chloride and acid hydrogen All other carbonates Sulfuric Acid Mg + H₂SO, Zn + H₂SO, MgSO₂ + H₂ ZnSO₂ + H₂ FeSQ, + H₂ Fe + H₂SO, SUMMARY OF METALS WITH ACIDS All other hydroxides Metal sulfate and hydrogen CE HAS LOST A PROTON HO HAS GAINED A PROTON, FORMING HO Hydrochloric Acid Mg + 2HCL→→→→→ MgCl₂ + H₂ Zn +2HCL→→→→→ ZnCl₂ + H₂ Fe + 2HCL FeCl₂ + H₂ Name of products Equation for reaction M+2HCL >>> MCL₂ + H₂ M + H₂SO₂ →→→→MSO, + H₂ → Examples with HCL and H₂SO4 ACIDS + BASES (NEUTRALISATION) METAL HYDROXIDE + ACID SALT + WATER METAL OXIDE + ACID → SALT + WATER METAL CARBONATE + ACID →→ SALT + WATER + CO₂ AMMONIA (gas) + ACID → AMMONIUM SALT PREPARING SALTS (SOLUBLE) FROM AN INSOLUBLE BASE • Soluble salts can be prepared by reacting an acid with an insoluble base HEAT ACID IN WATER BATH ADD INSOLUBLE BASE IN EXCESS MIX 10...
ACIDS, BASES AND SALT PREPARATIONS SOLUBILITY RULES Soluble Compounds of sodium, potassium, and ammonium Acid All nitrates PROTON TRANSFER ACIDS: All chlorides, except... All sulfates except... Sodium, potassium, and ammonium carbonates Zinc Iron Sodium, potassium, and calcium hydroxides ALKALIS: Acid • Proton donors • Proton acceptors Magnesium O-H Sulfuric acid DONOR (ACID) ionise in solution producing protons, Ht ions. HP ACCEPTOR (BASE) Insoluble ...silver and lead (II) ionise in solution producing OH ions which can accept protons. ...barium, calcium, and lead (II) REACTIONS OF ACIDS • only metals above hydrogen in the reactivity series will react with dilute acids. the more reactive the metal, the more vigorous the reaction. METAL + ACID SALT + HYDROGEN Hydrochloric Metal chloride and acid hydrogen All other carbonates Sulfuric Acid Mg + H₂SO, Zn + H₂SO, MgSO₂ + H₂ ZnSO₂ + H₂ FeSQ, + H₂ Fe + H₂SO, SUMMARY OF METALS WITH ACIDS All other hydroxides Metal sulfate and hydrogen CE HAS LOST A PROTON HO HAS GAINED A PROTON, FORMING HO Hydrochloric Acid Mg + 2HCL→→→→→ MgCl₂ + H₂ Zn +2HCL→→→→→ ZnCl₂ + H₂ Fe + 2HCL FeCl₂ + H₂ Name of products Equation for reaction M+2HCL >>> MCL₂ + H₂ M + H₂SO₂ →→→→MSO, + H₂ → Examples with HCL and H₂SO4 ACIDS + BASES (NEUTRALISATION) METAL HYDROXIDE + ACID SALT + WATER METAL OXIDE + ACID → SALT + WATER METAL CARBONATE + ACID →→ SALT + WATER + CO₂ AMMONIA (gas) + ACID → AMMONIUM SALT PREPARING SALTS (SOLUBLE) FROM AN INSOLUBLE BASE • Soluble salts can be prepared by reacting an acid with an insoluble base HEAT ACID IN WATER BATH ADD INSOLUBLE BASE IN EXCESS MIX 10...
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SuSSan, iOS User
Love this App ❤️, I use it basically all the time whenever I'm studying
Alternative transcript:
REACT REMEMBER: the acid that you use HYDROCHLORIC ACID SULFURIC ACID NITRIC ACID o FILTER 10 REMOVE UNREACTED BASE will depend on what salt you want: CHLORIDE SALTS SULFATE SALTS NITRATE SALTS GENILY HEAL TO EVAPORATE WATER FROM AN ACID AND AN ALKALI • acids react with alkalis to form a salt and water →You cannot use an excess of one of the reactants because both reactants are solutions and cannot be separated by filtration. METHOD USING TITRATIONS O carry out a titration to work out precise volumes of aud and alkali needed for neutralisation to occur. LEAVE TO CRYSTALLISE WASH AND DRY 2 Mix the appropriate volumes of acid and alkali so that they react completely and we are left with a solution containing salt and water. USING TWO SOLUBLE SALTS • called a precipitation reaction Evaporate off the water by gently heating the solution and allow to cool so that the soluble salt will crystallise. Filter the solid salt, wash and dry. sulid, insoluble sall produced is the precipitate. EXAMPLE: Making Silver chloride J a soluble sall that contains Silver: Silver nitrate a soluble chloride sale: magnesium/sodium /potassium chloride. METHOD: Dissolve magnesium chloride in water (do the same with the silver nitrate) (2 add both solutions together and stir 3 a precipitate of silver chloride should form remove precipitate by filtration, wash and dry in an oven. PREPARATION OF COPPER (11) SULFATE FROM COPPER (11) CARBONATE METHOD: measure 25cm³ of dilute sulphuric acid into a beaker and add 25cm³ of distilled water. 22 Add a small spatula of copper (11) oxide, place on a tripod and gauze and warm gently whilst stirring. continue adding the solid until there is excess solid left over. •4 leave to cool and filter into an evaporating dish CRYSTALLISATION: the marking points I hear the solution to concentrate it by evaporating off about half the water or until crystals appear on a dipped glass rod leave the solution to cool and crystallise. filler to separate the crystals from solution. pat crystals dry with filter paper.