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.

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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?

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 -

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+

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)

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)

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)

Bases Bases neutralise acids forming a SALT + WATER NaOH (s) (+ H 2 O)  Na + (aq) + OH - (aq) NH 3 + H 2 O  NH 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)

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…………

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

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?  ………………………………………………………. … …

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.

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

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

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+

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 -

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.

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 OH - Mg(OH) 2 …………………… Ca(OH) 2(s) (+ H 2 O) …………………….. KOH (s) (+ H 2 O) ….. ……………… (aq)

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 OH - Mg(OH) 2  Mg OH - 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.

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 OH - NaOH + HCl  NaCl + H 2 O Ca(OH) 2 + HCl  CaCl 2 + 2H 2 O NH 3 + HNO 3  NH NO 3 -

Acids + Metal Hydroxides Acids react with metal hydroxides to produce a salt and water. HCl + Mg(OH) 2 --> KOH + H 2 SO 4 -->

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 -->

Acids + Metals Acids react with metals to produce a salt and hydrogen gas. 2HCl + 2Na --> 2HCl + Fe --> 6HCl + 2Fe -->

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

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 -->

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 -->

Acids + Metal Oxides Acids react with metal oxides to produce a salt and water. HCl + MgO--> CuO + H 2 SO 4 -->

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!

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

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

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

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

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

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

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.

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.