1. C4a Acids and Bases neutralAcidic Basic (alkaline) 1 2 3 45 67 891011 12 13 14 strongweak neutral weak strong Solutions with a pH of ________ than 7 are acids. Solutions with a pH of ________ than 7 are alkalis/bases. Solutions with a pH of 7 are_________________. HIGHERWhat is an acid?Look at the formulae of these acids.Hydrochloric acid HCl Sulphuric acidH2SO4 What element do they all have in common? Nitric acidHNO3 Phosphoric acid H3PO4 Definition: What is an alkali?Definition:What is the difference between an alkalis and a base?We often use the words base and alkali to describe the same chemicals. The differenceis that an alkali is a base that _______________ in water.Alkalis watersoluble bases Bases s

2. Neutralisation An acid can be neutralised by adding enough _____________ An alkali can be neutralised by adding enough _____________ Adding acid to alkali makes the pH go _________ Adding alkali to acid makes the pH go _________General equation for neutralisation: HIGHER Ionic equation for neutralisation: Uses of sulfuric acid: 1. 2. 3. 3. Making Salts Summary Everything on this page has been studied before but if it is not familiar you MUST learnit! Acids to LearnHydrochloric acidHClSulphuric acid H2SO4Nitric acidHNO3Phosphoric acidH3PO4 Alkalis water Salts soluble bases Compounds formed between a metal and the non-metal part of an acid in a neutralisation reactionBasesAcidName of salt HCl chlorideH2SO4 sulphateHNO3nitrateH3PO4 phosphatemetal + acidsalt + hydrogen metal oxide + acidsalt + water metal hydroxide + acidsalt + water Metal carbonate + acid salt + water + carbon dioxide 4. Reacting acids with bases and carbonatesThe following are all of the names and symbols that the examiners can expect you to know. Any of these acids could react with any of the bases or carbonates in a neutralisation reactionAcidsBases Carbonates sulfuric acid potassium hydroxidesodium carbonate nitric acid sodium hydroxide calcium carbonate hydrochloric acid copper oxide ammonia AcidsBasesCarbonatesH2SO4KOHNa2CO3HNO3 NaOH CaCO3 HClCuONH3Reactions with Sulfuric Acid Dont forget state symbols: (aq) (g) (s)(l) sulfuric acid + potassium hydroxide +water H2SO4 (aq) + KOH(aq)+H2O(l) sulfuric acid + sodium hydroxide+ water H2SO4 (aq) + NaOH (aq)+H2O(l) sulfuric acid + copper (II) oxide + water H2SO4 (aq) + CuO(s) + H2O(l) sulfuric acid + ammonia H2SO4 (aq) + NH3(aq) sulfuric acid + sodium carbonate+ water + carbon dioxide H2SO4 (aq) + Na2CO3(s)+ H2O(l)+ CO2 (g) sulfuric acid + calcium carbonate + water + carbon dioxideH2SO4 (aq)+CaCO3(s)+ H2O(l) + CO2 (g) 5. Doyo bes urReactions with Hydrochloric Acidt, d ontpanHydrochloric acid + potassium hydroxide ic!HCl(aq) + KOH (aq)Hydrochloric acid + sodium hydroxideHCl(aq) + NaOH (aq)Hydrochloric acid + copper (II) oxideHCl(aq) + CuO (s)Hydrochloric acid + ammoniaHCl(aq) + NH3(aq)Hydrochloric acid + sodium carbonateHCl(aq) + Na2CO3(s)Hydrochloric acid + calcium carbonateHCl(aq) +CaCO3(s)Reactions with Sulfuric Acid nitric acid + potassium hydroxidenitric acid + sodium hydroxidenitric acid + copper (II) oxidenitric acid + ammonianitric acid + sodium carbonatenitric acid + calcium carbonateIf you got through that lot turn to your nearest neighbour and give them a well deserved high-5 ! 6. smallbeaker Changing the pH small funneldilute hydrochloric 1. Use a measuring cylinder to transferacid burette clamp30 cm3 of dilute sodium hydroxidesolution to a 250 cm3 beaker. 2. Fill a burette with dilute hydrochloricacid as shown in the diagram. By turningthe burette tap slightly check that thesolution is able to drip out of the tapsteadily. Close the tap and record the 100cm3 beakerreading on the burette.(acting as a drip- tray)Volume of HCl addedpH of solution Volume of HCl pH of solutionfrom burette in conical flask added from burettein conical flask 0 15.5 0.5 16.01.016.51.517.0 2.0 17.5 2.5 18.0 3.0 18.5 3.5 19.0 4.0 19.5 4.5 20.0 5.0 20.5 5.5 21.0 6.0 21.5 6.5 22.0 7.0 22.5 7.5 23.0 8.0 23.5 8.5 24.0 9.0 24.5 9.5 25.0 10.025.5 10.526.0 11.026.5 11.527.0 12.027.5 12.528.0 13.028.5 13.529.0 14.029.5 14.530.0 15.0 7. Analysis of experiment 1. Describe how the pH changes over the course of the experiment as the acid isadded to the alkali. 2. On the graph of your data mark the point on the curve where the pH is 7. What doyou notice about the position of this point? 3. At what point on your graph is acid in excess? Explain your answer. (H) 4. The products of this neutralisation reaction are sodium chloride solution andwater. Write a word equation for the reaction. 5. Write a symbol equation for the reaction. (H) 6. Suggest how the pH of a dilute solution of hydrochloric acid changes when asolution of sodium hydroxide is added to it until the sodium hydroxide is in excess.(H)