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Acids & Bases What is an acid? (It is defined by its behavior in water.) What is a base? What does neutralization mean? What are the products of a neutralization reaction? Are the following acids or bases? Metal oxides, metal hydroxides and carbonates Metal oxides, metal hydroxides and carbonates What is a salt and how does it relate to an acid?
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Acids - Ionisation All acids ………….. in solution to give …………. HCl --> …………….. (100%) Cl - H+H+ H+H+ H2OH2O H+H+ Cl + H H H+H+ H+H+ Cl -
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Acids - Ionisation All acids ionise in solution to give H + ions. HCl H + + Cl - (100%) Cl - H+H+ H+H+ H2OH2O H+H+ Cl + H H H+H+ H+H+
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Acids - Ionisation All acids …………… in solution to give …… ions. HCl ……+ Cl - Cl - (100%) HCl (+ H 2 O) H 2 O) ……… (aq) (aq) + Cl - (aq) H 2 O H 2 O + …….. H3O+H3O+H3O+H3O+ Nitric Acid: Acid: HNO 3 HNO 3 H+ H+ H+ H+ + NO 3 - NO 3 - (nitrate anion) Sulphuric Acid: Acid: H 2 SO 4 H 2 SO 4 2H + 2H + + ………….. ………….. (sulphate anion) Carbonic Acid: H 2 CO 3 H 2 CO 3 ……..+ ………… (…..……… anion) Ethanoic acid: CH 3 COOH CH 3 COOH ……. ……. + ……………… (………………….... (………………….... anion)
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Acids - Ionisation All acids ionise ionise in solution to give H+ H+ H+ H+ ions. HCl H+ H+ H+ H+ + Cl - Cl - (100%) HCl (+ H 2 O) H 2 O) H 3 O + (aq) H 3 O + (aq) + Cl - (aq) H 2 O H 2 O + H+ H+ H+ H+ H3O+H3O+H3O+H3O+ Nitric Acid: Acid: HNO 3 HNO 3 H+ H+ H+ H+ + NO 3 - NO 3 - (nitrate anion) Sulphuric Acid: Acid: H 2 SO 4 H 2 SO 4 2H+ 2H+ 2H+ 2H+ + SO 4 2- SO 4 2- (sulphate anion) Carbonic Acid: H 2 CO 3 H 2 CO 3 2H+ 2H+ 2H+ 2H+ + CO 3 2- CO 3 2- (carbonate anion) Ethanoic acid: CH 3 COOH CH 3 COOH H + H + + CH 3 COO - (ethanoate anion)
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Bases Bases …………………….. acids. NaOH (s) (+ H 2 O) ………. (aq) + ……. (aq) NH 3 + H 2 O …………….. + OH - NaOH + HCl NaCl + ……….. NH 3 + HNO 3 ……....... + NO 3 - Liberate ……….. - ions in water. HF + KOH ……. + …….. H 2 CO 3 + 2KOH ………… + ……… Ca(OH) 2(s) (+ H 2 O) ………. (aq) + ….OH - (aq) Mg(OH) 2(s) (+ H 2 O) ……… (aq) + …….. - (aq)
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Bases Bases neutralise acids forming a SALT + WATER NaOH (s) (+ H 2 O) Na + (aq) + OH - (aq) NH 3 + H 2 O NH 4 + + OH - NaOH + HCl NaCl + H2OH2O NH 3 + HNO 3 NH4+ NH4+ + NO 3 - Liberate OH - ions in water. HF + KOH KF + H 2 O H 2 CO 3 + 2KOH K 2 CO 3 + 2H 2 O Ca(OH) 2(s) (+ H 2 O) Ca 2+ (aq) + 2OH - (aq) Mg(OH) 2(s) (+ H 2 O) Mg 2+ (aq) + 2OH - (aq)
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Bases Soluble bases are called alkalis. Metal Hydroxides Metal Oxides Metal Carbonates Metal Hydrogen Carbonates Ammonia NaOHCaO CaCO 3 NaHCO 3 NH 3 Ca(OH) … Na … O Na …. CO 3 Ca(HCO 3 )... CH 3 NH 2 Zn(OH) … Al …….. Li …. CO 3 Mg ………… Al………. Fe (III).. Al …. (CO 3 ) …. Al ………… NH 4 ……. Mn. (4+) NH 4……….. NH 4…………
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Bases Soluble bases are called alkalis. Metal Hydroxides Metal Oxides Metal Carbonates Metal Hydrogen Carbonates Ammonia NaOHCaO CaCO 3 NaHCO 3 NH 3 Ca(OH) 2 Na 2 O Na 2 CO 3 Ca(HCO 3 ) 2 CH 3 NH 2 Zn(OH) 2 Al 2 O 3 Li 2 CO 3 Mg(HCO 3 ) 2 Al(OH) 3 Fe 2 O 3 Al 2 (CO 3 ) 3 Al(HCO 3 ) 3 NH 4 OH MnO 2 (NH 4 ) 2 CO 3 NH 4 HCO 3
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Acids & Bases What is an acid? ………………………………….......................................................................... What is a base? ………………………………….......................................................................... What does neutralization mean? ………………….......................................................................... What are the products of a neutralization reaction? ………………………………… Are the following acids or bases? …………….. Metal oxides, metal hydroxides and carbonates Metal oxides, metal hydroxides and carbonates What is a salt and how does it relate to an acid? ………………………………………………………. ….......................................................................... …..........................................................................
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Acids & Bases What is an acid? Acids react with water to release H + ions. What is a base? A substance that neutralizes an acid. What does neutralization mean? Cancel out the acidic properties. What are the products of a neutralization reaction? A salt and water. Are the following acids or bases? bases Metal oxides, metal hydroxides and carbonates Metal oxides, metal hydroxides and carbonates What is a salt and how does it relate to an acid? A metal ion bonded to the non metal ion of an acid.
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Acid strength & pH H 3 O + concentration (mol/dm 3 ) Strong acids Weak acids Diluting a strong acid by a factor of ten only changes its pH by one unit. 1 0.1 0.01 10 -3 10 -4 10 -5 10 -6 10 -7 10 -8 10 -9 10 -10 10 -11 10 -12 10 -13 10 -14 1 0.1 0.01 10 -3 10 -4 10 -5 10 -6 10 -7 10 -8 10 -9 10 -10 10 -11 10 -12 10 -13 10 -14 0 -1 -2 -3 -4 -5 -6 -7 -8 -9 -10 -11 -12 -13 -14 0 -1 -2 -3 -4 -5 -6 -7 -8 -9 -10 -11 -12 -13 -14
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Acids – Strength 2 Cl - Strong Strong acid all molecules dissociated Lots of H + ionsLots of H + ions H Cl Cl - H+H+ H+H+ 4H-F HF H+H+H+H+ F-F- Weak Weak acid Hardly any molecules dissociate few H + ionsfew H + ions / dm 3. HF HF H + - + F ( partially - hardly any) hydrofluoric acid fluoride ion
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Cl - Acids - ionisation 2 Cl - 200HCl Dilute Strong acid all molecules dissociated few molecules / dm 3. Concentrated Strong Acid: All molecules dissociated Many molecules per dm 3 H Cl H+H+ Cl - H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+
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Acids - Concentrated/Dilute All acids ionise in solution to give H + ions. HCl --> H + + Cl - 2H-Cl H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ Cl - H+H+ H+H+ H+H+ H+H+ 10H-Cl H+H+ Cl -
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Weak Acids - Ionisation HF --> F - + H + ( partially - hardly any) hydrofluoric acid fluoride ion Concentrated Weak acid Hardly any dissociation Lots of molecules/dm 3 2H-F F-F- HF H+H+ F-F- H+H+ HF - 20HF Dilute Weak acid Hardly any molecules dissociate few molecules / dm 3.
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Base Strength Strong bases ionise ………………………. Weak bases ionise only partially. NaOH (s) (+ H 2 O) ……... Na + (aq) + OH - (aq) NH 3 + H 2 O ……. NH 4 + + OH - Mg(OH) 2 …………………… Ca(OH) 2(s) (+ H 2 O) …………………….. KOH (s) (+ H 2 O) ….. ……………… (aq)
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Base Strength Strong bases ionise completely. Weak bases ionise only partially. NaOH (s) (+ H 2 O) Na + (aq) + OH - (aq) NH 3 + H 2 O NH 4 + + OH - Mg(OH) 2 Mg 2+ + 2OH - Ca(OH) 2(s) (+ H 2 O) Ca 2+ (aq) + 2OH - (aq) KOH (s) (+ H 2 O) K + (aq) + OH - (aq) GI metal hydroxides tend to be STRONG BASES GII metal hydroxides tend to be WEAK BASES.
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Bases Bases ________ ________. Liberate ________ in water. Soluble bases are called _________. Strong bases ______________. Weak bases ionise only __________. NaOH (s) (+ H 2 O) --> Na + (aq) + OH - (aq) Ca(OH) 2(s) (+ H 2 O) --> Ca 2+ (aq) + 2OH - (aq) NH 3 + H 2 O --> NH 4 + + OH - NaOH + HCl NaCl + H 2 O Ca(OH) 2 + HCl CaCl 2 + 2H 2 O NH 3 + HNO 3 NH 4 + + NO 3 -
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Acids + Metal Hydroxides Acids react with metal hydroxides to produce a salt and water. HCl + Mg(OH) 2 --> KOH + H 2 SO 4 -->
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Acids + Metal Hydroxides Acids react with metal hydroxides (base) to produce a salt and water. 2HCl + Mg(OH) 2 --> MgCl 2 + 2H 2 O K 2 SO 4 + 2H 2 O2KOH + H 2 SO 4 -->
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Acids + Metals Acids react with metals to produce a salt and hydrogen gas. 2HCl + 2Na --> 2HCl + Fe --> 6HCl + 2Fe -->
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Acids + Metals Acids react with metals to produce a salt and hydrogen gas. 2HCl + 2Na --> 2 NaCl + H 2 2HCl + Fe --> FeCl 2 + H 2 6HCl + 2Fe --> 2FeCl 3 + 3H 2
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Acids + Carbonates Acids react with carbonates to produce a salt, water and carbon dioxide gas. HCl + Na 2 CO 3 --> Na 2 CO 3 + HNO 3 -->
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Acids + Carbonates Acids react with carbonates to produce a salt, water and carbon dioxide gas. 2HCl + Na 2 CO 3 --> 2 NaCl + H 2 O + CO 2 2NaNO 3 + H 2 O + CO 2 Na 2 CO 3 + 2HNO 3 -->
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Acids + Metal Oxides Acids react with metal oxides to produce a salt and water. HCl + MgO--> CuO + H 2 SO 4 -->
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SALTS ACID + BASE SALT +..... HNM + MNMO MNM + H 2 (O) +.. HCl + NaOH NaCl +..... Non metal part of SALT comes from ACID! METAL part of the SALT comes from BASE!
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Acids + Metal Oxides Acids react with metal oxides to produce a salt and water. 2HCl + MgO--> white MgCl 2 + H2OH2O colorless CuSO 4 + H 2 O blue CuO + H 2 SO 4 --> black
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SALTS A SALT is a compound formed when a metal is ionically bonded to a non-metal. Salts are formed in many acid-base reactions. Acid +......... ............ +................... Acid +.................... ............ +................... Acid +..................... ............ +................... Acid +...................... .......... +.......................+.............. Acid +.................................... .......... +.......................+.............. SALTACIDBASEACIDBASESALT MgCl 2 HClMg(OH) 2 Fe(NO 3 ) 2 H 2 SO 3 NaOH MgCO 3 H 2 CO 3 CaO Al 2 (SO 4 ) 3 H 2 CO 3 CaCO 3 (NH 4 ) 3 PO 4 H 2 SO 4 Mg.........
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SALTS A SALT is a compound formed when a metal is ionically bonded to a non-metal. Salts are formed in many acid-base reactions. Acid + Metal SALT + hydrogen Acid + Metal Oxide SALT + water Acid + Metal hydroxide SALT + water Acid + Metal carbonate SALT + carbon dioxide + water Acid + Metal hydrogen carbonate SALT + carbon dioxide + water SALTACIDBASEACIDBASESALT MgCl 2 HCl Mg(OH) 2 Fe(NO 3 ) 2 H 2 SO 3 NaOH MgCO 3 H 2 CO 3 CaO Al 2 (SO 4 ) 3 H 2 CO 3 CaCO 3 (NH 4 ) 3 PO 4 H 2 SO 4 Mg.........
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SALTS A SALT is a compound formed when a metal is ionically bonded to a non-metal. Salts are formed in many acid-base reactions. Acid + Metal SALT + hydrogen Acid + Metal Oxide SALT + water Acid + Metal hydroxide SALT + water Acid + Metal carbonate SALT + carbon dioxide + water Acid + Metal hydrogen carbonate SALT + carbon dioxide + water SALTACIDBASEACIDBASESALT MgCl 2 HCl Mg(OH) 2 MgCl 2 Fe(NO 3 ) 2 H 2 SO 3 NaOH Na 2 SO 3 MgCO 3 H 2 CO 3 CaO CaCO 3 Al 2 (SO 4 ) 3 H 2 CO 3 CaCO 3 (NH 4 ) 3 PO 4 H 2 SO 4 Mg MgSO 4
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SALTS A SALT is a compound formed when a metal is ionically bonded to a non-metal. Salts are formed in many acid-base reactions. Acid + Metal SALT + hydrogen Acid + Metal Oxide SALT + water Acid + Metal hydroxide SALT + water Acid + Metal carbonate SALT + carbon dioxide + water Acid + Metal hydrogen carbonate SALT + carbon dioxide + water SALTACIDBASEACIDBASESALT MgCl 2 HClHCl Mg(OH) 2 MgCl 2 Fe(NO 3 ) 2 HNO 3 H 2 SO 3 NaOH Na 2 SO 3 MgCO 3 H 2 CO 3 CaO CaCO 3 Al 2 (SO 4 ) 3 H 2 SO 4 H 2 CO 3 CaCO 3 (NH 4 ) 3 PO 4 H 3 PO 4 H 2 SO 4 Mg MgSO 4
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SALTS A SALT is a compound formed when a metal is ionically bonded to a non-metal. Salts are formed in many acid-base reactions. Acid + Metal SALT + hydrogen Acid + Metal Oxide SALT + water Acid + Metal hydroxide SALT + water Acid + Metal carbonate SALT + carbon dioxide + water Acid + Metal hydrogen carbonate SALT + carbon dioxide + water SALTACIDBASEACIDBASESALT MgCl 2 HClMgOHCl Mg(OH) 2 MgCl 2 Fe(NO 3 ) 2 HNO 3 Fe(OH) 2 H 2 SO 3 NaOH Na 2 SO 3 MgCO 3 H 2 CO 3 Mg(OH) 2 H 2 CO 3 CaO CaCO 3 Al 2 (SO 4 ) 3 H 2 SO 4 Al 2 (CO 3 ) 3 H 2 CO 3 CaCO 3 (NH 4 ) 3 PO 4 H 3 PO 4 NH 3 H 2 SO 4 Mg MgSO 4
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Acids & Bases – Every day uses Acids: Bases: Make a presentation slide (one slide only) showing some everyday uses of acids & bases – in our homes as well as in industry.
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Acids & Bases – Every day uses Acids: Vinegar on chips & wasp stings (alkali) Sulphuric acid drain cleaner, car batteries Hydrochloric acid pools, cleaning cement off brickwork Bases: sodium hydroxide soap making, oven & drain cleaning Sodium hydrogencarbonate, cooking, bee stings (acidic) Calcium oxide/hydroxide (lime/slaked), increasing soil or water pH, self heating cans, Bicarbonate of soda fight indigestion (stomach acid) Make a presentation PowerPoint or OneNote showing some everyday uses of acids & bases – in our homes as well as in industry.
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