Chemical Reactions Course Content 2024 PDF

Chemical Reactions Year 10 Science Semester Two 2023 Unit Outline Chemical reactions Types Rates Equations States Predicting products Rates and changing conditions Procedure for titration reaction Assessment SIS task 2 Unit test...

Chemical Reactions Year 10 Science Semester Two 2023 Unit Outline Chemical reactions Types Rates Equations States Predicting products Rates and changing conditions Procedure for titration reaction Assessment SIS task 2 Unit test  Lesson 1 Starter 1) IONIC 1) What type of compound is this? (Ionic/Covalent) 2) 3 (Cu, N, 2) How many elements make up this compound? O) 3) Using your ion table, name this compound 3) Copper Nitrate 4) If a piece of pure Iron was added to a solution of 4) It would this, what would happen? displace the ANSWERS NEXT ANSWERS NEXT: copper to for Iron 3 Nitrate  Word and Chemical Equations Learning Intentions To be able to write word equations To write correct balanced compounds 4 Word Equations Word equations tell you the names of the reactants as well as the names of the products. It is important to remember that a chemical change has occurred, you cannot use = but must use  to show the change from reactants to products. 5 Conservation of Mass In any chemical equation, no mass can be created or destroyed, it can only be rearranged. The bonds between the atoms in the reactants are broken, then the atoms make new bonds with other atoms to form the products. https://www.youtube.com/watch?v=2S6e11NBwiw (4:36) Whatever we started with, must be present at the end. (Examples of amazing chemical reactions - 6 https://www.youtube.com/watch?v=0Bt6RPP2ANI) Combination Reactions Combination reactions generally involve two reactants joining to make one product. The individual masses of the reactants will combine to make the new product. For example, magnesium, a shiny silver metal, burns in air to form a white powder, magnesium oxide. Your teacher will now demo a combination reaction for you; the reaction of Zinc and Sulphur. Look for evidence that a chemical reaction has taken place. Time permitting DEMO 7  Chemical Formulae To be able to write balanced chemical equations, you also need to know some general formulae and recognise what atoms are present in the formulae. You will always be given a list of cations (positive) and anions (negative) for assessments for this unit –see your Ammonium Barium Aluminium Al 3+ NH 4 + booklet Ba for 2+ this Iron (III) Hydrogen Calcium Fe3+ H+ Ca2+ Sodium Copper (II) Na+ Cu2+ Potassium Lead K+ Pb2+ Silver Magnesium Ag+ Mg2+ Sodium Zinc Bromide Na + Br- Carbonate Zn 2+ Phosphate Chloride Mercury Cl- CO32-(II) Iron PO43- Iodide Hg + I- Fe 2+ Oxide Nitride 8 Copper (I) Hydroxide Manganese O2-2+ N3- Cu + Mn OH- Sulphate Nickel Nitrate SO 2- Ni 2+4 What’s the formula? Last semester, you learnt to work out formulae from ions Have some more practice: For example, sulphuric acid is made up of H+ and SO42- What is the formula when the following ions ions. react? To decide on the formula, you can either swap and drop the charges…1.Na+ and O2- 2H+ + SO42-  H2SO4 2.Ba2+ and OH- Or, balance the charges, in this case by having 2 hydrogen ions for every sulphate ion. 2 x H+ bonded with3.Al 3+ andthe SO42- gives Clmolecule - H2SO4 This method helps you to see that 2 H are needed in 9 the reactants for conservation 4.Ca2+ and of mass. N3- Naming Compounds There are a few general naming rules you need to help you with this: 1. If there are two atoms of the same element, the name stays the same. For example, N2 is nitrogen. 2. If there are two elements joined together, the name usually ends in –ide. For example, MgO is magnesium oxide, KCl is potassium chloride. 3. If there are more than two elements joined together and one of them is oxygen, the name usually ends in –ate. For example, MgCO3 is magnesium carbonate. 4. The ion sheet can help you name a compound, as you join the 10 two names of the ions together. Chemical Formulae Task 1: Complete Lesson 1 Worksheet: ‘Naming Ionic Formulae’ worksheet Task 2: Complete Lesson 1 Worksheet: ‘Creating Balanced Ionic Formulae’ 11 Lesson 2 - 3 Learning Intentions To be able to write and balance symbol equations for chemical reactions and include state symbols 12 Lesson starter: name these compounds KBr AlBr3 MgSO4 NaNO3 K2CO3 Al(OH)3 13  Balanced Equations Balanced equations use formula to represent the reactants and products Reminder: In all chemical equations the reactants are written on the left hand side of an arrow and the products on the right hand side. An arrow is used to illustrate a chemical change. 14  Balancing Chemical Equations Chemical equations must be balanced. There must be the same number of atoms on the left and right hand sides of the equation. There must also be the same number of each type of atom on the left and right hand sides. During a reaction, no atoms are lost or made, so the mass of the 15 products must equal the mass of the reactants.  Balancing Chemical Equations Remember: There must be the same number of atoms on the left and right hand sides of the equation. There must also be the same number of each type of atom on the left and right hand sides. To balance this equation, we need to multiply the 16 individual atoms by a number that will result in there being the same number of each type of atom on each side of the equation.  Balancing Chemical Equations Remember: There must be the same number of atoms on the left and right hand sides of the equation. There must also be the same number of each type of atom on the left and right hand sides. You can only balance equations by placing numbers in front of a formula. This multiplies each part of the formula 17 by that number. You cannot alter the subscript numbers as these tell us the ratio of atoms in a specific molecule. Worked Example Na + O2  Na2O Na = 1 Na = 2 O=2 O=1 I can multiply O on the right hand side by 2… Na + O2  2 Na2O ……but this now gives me 4 Na Na = 1 Na = 4 O=2 O=2 So I need to multiply the Na on the left by 4…. 4 Na + O2  2 Na2O Na = 4 Na = 4 The equation is now balanced. 18 O=2 O=2 Combination Reactions – students complete in booklet Use your ion table to complete the combination reactions below Then try the following combination reactions: Magnesium + oxygen  magnesium oxide 2Mg + O2  2MgO Oxygen + carbon  carbon dioxide O2 + C  CO2 Calcium oxide + water  calcium hydroxide CaO + H2O  Ca(OH)2 Sodium + chlorine  sodium chloride 2 Na + Cl2  2 NaCl 19 State Symbols When writing balanced equations, there are four state symbols that show the physical state of the reactants and products. l liquid s solid g gas The state symbols should be written in subscript and in brackets after each reactant and product as shown: 2Na (s) + Cl2 (g)  20 2NaCl (s) NaOH (aq) + HCl (aq)  NaCl (aq) + H O Writing equations 1. Start with the word equation and name all of the reactants and products. 2. Replace the words with formula and write the symbol equation. 3. Check to see if the equation is balanced by counting the number of each atom on each side of the equation. 4. If the number of each atom is the same on each side, the equation is balanced. If not, add coefficients in front of the formulae to balance the equation. 5. Add physical state symbols. 21 Worksheets 1-3 -Balancing Symbol Equations (stage 1), (stage 2) and A world of reactions. Complete Worksheets Lesson 2 Balancing Symbol Equations 1 If confident move onto Balancing Equations 2 which follows.Success Criteria: I can write balanced chemical equations 22 Knowledge Check When James dropped a lump of magnesium into a test tube of hydrochloric acid, a solution of magnesium A ‘lump’ chloride was formed. James noticed a of gasmagnesium being shows it was formed. a solid. A solution of magnesium chloride shows it is aqueous so it is dissolved For this reaction: in water. There must also have been water present in the reactants (aq). 1. Write a word equation 2. Write a balanced formula equation 3. Add state symbols Magnesium + hydrochloric Success Criteria: acid  magnesium chloride + hydrogen I can write balanced chemical equations with state 23 symbols Mg (s) + 2 HCl (aq)  MgCl2 (aq) + H2 (g) Extra Practice Jefferson – choose your difficulty level in practising balancing equations games. Use this Balancing equations link to learn more about balancing chemical equations. Worksheets available from the 24 portal in the “extension” area. Success Criteria I can write a word equation I can write a symbol equation I can balance a symbol equation I can include state symbols in a symbol equation 25  Different types of Lesson 3-4: Reactions Lesson starter: Balance these equations! (no states necessary for these) 1) ____ AlBr3 + ____ K  ____ KBr + ____ Al 2) ____ FeO + ____ PdF2  ____ FeF2 + ____ PdO 3) ____ P4 + ____ Br2  ____ PBr3 4) ____ LiCl + ____ Br2  ____ LiBr + ____ Cl2 26 5) ____ PbBr2 + ____ HCl  ____ HBr + ____ PbCl2 ANSWERS NEXT slide  Different types of Lesson 3-4: Reactions Answers 1) 1 AlBr3 + 3 K  3 KBr + 1 Al 2) 1 FeO + 1 PdF2  1 FeF2 + 1 PdO 3) 1 P4 + 6 Br2  4 PBr3 4) 2 LiCl + 1 Br2  2 LiBr + 1 Cl2 5) 1 PbBr2 + 2 HCl  2 HBr + 1 PbCl2 27  Different types of Lesson 3-4: Reactions Learning Intentions: 1. To be able to recognise different types of reactions and work out what the products of them will be. 2. Construct word and balanced symbol equations with state symbols for each reaction. 28 A world of reactions Everything on our planet is involved in a cycle; we don’t eradicate elements or make new ones, we just turn them into something else. Even new, manmade elements are made from ones that already exist. So for this to happen, lots of different types of chemical reactions are constantly happening, to break down old compounds and make new ones. 29 Types of Reactions There are many different types of reactions. In this unit we will look at some examples of these and by the end you should be able to: Have an awareness of the safety precautions you need to take when carrying out an investigation by reading the symbols on the containers of chemicals. Recognise the type of reaction by knowing the reactants and products. Write a word equation for any type of reaction Construct a symbol equation for any type of reaction (you will always be given a list of ions to help you decide on the formula) Correctly balance the equation so the number of each 30 type of atom is the same on each side of the arrow. Add state symbols to the equation. Types of Reactions The types of reactions we look at in this unit are below, use the table in your booklet to record examples, equations and information regarding these reaction types. Combination: A + B  AB Decomposition: AB  A + B Displacement: AB + C  AC + B (single) and AB + CD  AD + CB (double) Precipitation: AB (aq) + CD (aq)  AD (aq) + CB (s) Neutralisation: Acid + Base  Salt + water 31 Combustion: Fuel (containing C and H) + O2  CO2 (g) + H2O (g) Combination – don’t forget to complete your table in the booklet We have already looked at this one earlier in the unit. A + B  AB Two elements combine to form a new compound 4Ag + O2 → 2Ag2O 32 Decomposition Reactions – don’t forget to complete your table in the booklet If something decomposes, it breaks down. Therefore, a decomposition reaction is identified by having only one reactant as this breaks down to become multiple products. It’s a bit like a food item being broken down into protein/ carbohydrate/fat and micronutrients. The elements or compounds produced can then go on to be made into something else. https://www.youtube.com/watch?v=UTfMrx7275w 33 (students fill table with pre-done equation for balancing and states only) Displacement Reactions – don’t forget to complete your table in the booklet Displacement reactions are when an element takes the place of another Cu O + Zn Cu + Zn O Single displacement reactions readily occur. The difference between single and double displacement reactions is illustrated below Single displacement: A + BC  AC + B Double displacement: AB + CD  AD + CB 34 https://www.youtube.com/watch?v=2MawIDT5DFU Precipitation – don’t forget to complete your table in the booklet Is a type of displacement reaction where a solid is formed Usually visible by a colour change https://www.youtube.com/watch?v=34d5ofcRhbU 35 Neutralisation - don’t forget to complete your table in the booklet Acid and base react to produce water pH Scale gives us colours to show acidity: https://www.youtube.com/watch?v=PdprNTwb4Ks We will be looking at this in more detail later in the unit. 36 Combustion – don’t forget to complete your table in the booklet Combination of a fuel with oxygen Heat and light produced Fuel (containing C and H) + O2  CO2 (g) + H2O (g) https://www.youtube.com/watch?v=yl89heCsBpQ 37 Lesson 5 - Pyrophoric Iron Practical Using the practical information sheet in your booklet – Carry out the decomposition reaction Complete the questions that follow 38 Lesson 6-7 – Precipitation Reactions Lesson starter: identify these types of reactions A) B) C) 39 Answers are on the next slide Lesson 6-7 – Precipitation Reactions Lesson starter: identify these types of reactions A) A) Answer: Decomposition B) B) Answer: Displacement C) C) Answer: Combination 40 Lesson 6-7 – Precipitation Reactions LEARNING OBJECTIVES: To identify when precipitation reactions will take place (solubility) To write correctly balanced chemical equations for precipitation reactions including state symbols Note: solubility table is at the back of the booklet 41  Precipitation Reactions Precipitation reactions are a special type of displacement reaction; the chemicals in each compound ‘swap partners’ to form new compounds, one of which is a solid. 42 Precipitation Reactions The precipitation reaction involves two aqueous solutions combining to form a precipitate. Aqueous; a compound dissolved in water to form a solution, like sugar water. Precipitate; a solid. It can be as lumps that sink to the bottom of a test tube, a fine powder that makes the solution look like paint or can be suspended in solution to make it look cloudy at the top. We know that certain chemicals are soluble in water and 43 others are not, so when we mix them we can work out which combined to form the insoluble precipitate. Solubility of ions – for Q2&3 – this table is included with your test 44 Teacher guided - example for the following reaction Calcium Chloride + Potassium Carbonate  CaCl2 (aq) + K2CO3 (aq) → 45 Practical Complete Investigation 5.1: Will it precipitate? And complete Q1. Remember to look at the hazard labels on the chemicals to assess what risks they may pose to you and decide what reasonable precautions you need to take to minimise risk. For Q2, you need to identify which new compound is the precipitate. To do that, you are not expected to remember the solubility of ions. However, you will be given a table of solubility of common ions and need to interpret it to discern which compound is the solid. When you write your symbol equation, you still need to add the state symbol (s) to identify this as the solid, whereas all other 46 compounds are aqueous (aq). Knowledge Check The following compounds are combined: sodium chloride and silver nitrate. A solid is formed. 1. Write a word equation for the reaction 2. Write a symbol equation for the reaction 3. If necessary, balance your equation 4. Add state symbols. Silver nitrate + sodium chloride  silver chloride + sodium nitrate Success Criteria: AgNO3(aq) + NaCl(aq)  AgCl(s) + I can recognise different types of reactions NaNO3(aq) Complete Worksheet 5.4 Precipitation 47 Balancing review For each of the following, balance the equation, Original Equation Balanced Equation Sr + O2  SrO Fe + O2  Fe2O3 CuO + H2  Cu + H2O Fe2O3 + CO  Fe+CO2 48 Worksheet 1 – Lesson 6-7 (Post Practical Worksheet /Homework task) 49 Success Criteria I can write a word equation for different types of reactions I can write a symbol equation for different types of reactions I can balance a symbol equation for different types of reactions I can include state symbols in a symbol equation for different types of reactions 50 Lesson 8 - Extracting metals Lesson starter: can we identify these common metals? A) Which metal used in jewelry turns black/tarnished on exposure to air over time? B) Which common metal which turns brown/red on exposure to air over time? C) Which very unreactive metal turns green over time 51 when exposed to air? Lesson 8 - Extracting metals Lesson starter: A) Which metal used in jewelry turns black/tarnished on exposure to air over time? Answer: Silver B) Which metal which turns brown/red on exposure to air over time? Answer: Iron C) Which metal turns green over time when exposed to air? 52 Answer: Copper Lesson 8 - Extracting metals Learning Intention To be able to use reactivity to explain why different extraction techniques are used for different metals. Part 1: https://youtu.be/NOKzDSwT3_0 Part 2: https://youtu.be/XZ0bWc-eAFo 53 Carbon reduction A type of displacement reaction Iron oxide + carbon  Carbon dioxide + Iron Copper oxide + carbon  Carbon dioxide + Copper Why do these reactions work? Would these two chemicals react: Why/Why not? Aluminium oxide + Carbon 54 Reactivity series (you don’t need to remember the order) 55 Complete – Worksheet 1 - Lesson 8 Lesson 8 worksheet regarding - Metal displacement in your booklet 56 Success Criteria I can state that metals less reactive than carbon can be extracted using carbon reduction I can explain that carbon would not be able to displace metals more reactive than carbon. 57 Lesson 9-10 - Rates of reaction Learning Intention To be able to explain how a reaction occurs based on collision theory To be able to explain what factors can change the rate of reaction 58  Rates of Reaction Reactions can be very fast, like fireworks or explosives, but they can also be slow – such as an apple turning brown. 59  Rates of Reaction Apples go brown when their flesh reacts with air. Which apple will go brown the quickest? Why? Where does the reaction take place? The reaction can only take place at the surface of solids, as this is where the reactants meet. 60 Rates of reaction What does rate of reaction mean? How can we measure it? What could we do to speed up rate of reaction? Why do these speed up the rate? Video below is for reference and can be viewed before the practical to help with understanding or after the practical to help with writeup. https://www.youtube.com/watch?v=f5IGpcuQNxo&t=922s (16min) This video from the portal page shows an example of how a rates 61 practical can be carried out. What makes a reaction happen? https://www.youtube.com/watch?v=SbapBWjDA74 62 Fruitful collisions Particles must collide with sufficient energy Particles must collide in the correct orientation 63 Changing rate of reaction Change the temperature Change the surface area Change the concentration These change the number of successful collisions of particles that lead to a reaction Add a catalyst Increases reaction rate and doesn’t get used up https://www.youtube.com/watch?v=ExHV_cFWYSM 64  Rate of Reaction Rate = change in reaction time e.g. Change in volume gas made time If the amount of product made is constant then the change in the reaction is a constant and is given the value 1, so rate = __1__ time 65  Calculating rate at regular intervals A student running 100m in 12.5 seconds has an average speed (rate) of 8 m/s. This is their rate, however it does not provide enough information to determine if they were faster at the start or the end of the race. If you had times for the first 50 m and the second 50 m, their rate at the start and end could be compared. Even better would be if you had their rate for each 10 m. We know that reactions slow over time, so it would be beneficial to calculate rate at intervals, rather than average rate for the whole reaction.  Rate of Reaction Graphs These show the increasing amount of product or the decreasing amount of reactant. The graph can indicate when the reaction was occurring most quickly. Shallow gradient Slow reaction 67  Finding the Rate of reaction from a curved graph YouTube video - how to get the ‘Rate of Reaction’ from the curve of a graph. https://youtu.be/GCR5xeduq2o?feature=shared&t=171 68 From the booklet - find the rate of reaction at 40seconds 69 Rate of Reaction Practical – see Portal page for the chosen prac sheet 70 Post Practical – Worksheet/Homework 5.8 – Calculating rates of reaction using the gradient of the graph 71 Success Criteria I can state that the rate of reaction can be measured by change of product or change of reactant over time I can state the factors that can affect rate of reaction I can explain why these factors can change rate of reaction based on particles colliding I can calculate the rate of reaction from a curved graph The SIS task will include content on rates and calculating rates of reaction. 72  Lesson 11 - Combustion reactions Lesson starter: calculate the rate of reaction for this graph at the time point of approximately 30seconds. Answers next: Change in g= 3.7-2.2 = 1.5 73 Change in time: 52- 12 = 40 Lesson 11 - Combustion reactions Learning Intention To be able to recognise combustion reactions and work out what the products of these will be. 74  Combustion Reactions Combustion requires 3 essential things: - Fuel - Oxygen supply - An ignitions source When a fuel burns in oxygen, it releases energy in the form of heat, light and sound. Fuels are organic compounds, such as wood, coal, natural gas and petrol (derived from oil). Spirit burners use alcohol as the fuel If there is enough oxygen present, complete Your teacher will now demo 75 combustion takes place. combustion for you. Combustion reactions The products of complete combustion are always carbon dioxide gas and water vapour. Incomplete combustion can produce solid carbon (soot), for example using the safety flame, and sometimes it can produce carbon monoxide if appliances are not working correctly or if areas are not ventilated correctly. Here is the combustion equation for propane gas in sufficient oxygen supply: Propane + oxygen  carbon dioxide + water vapour C3H8 (g) + O2 (g) CO2 (g) + H2O (g) 76 The equation is unbalanced. Can you balance it?? Incomplete Combustion https://www.youtube.com/watch?v=lMnaLKlVXxo (3:13) The above is an informative clip aimed at highlighting the dangers of incomplete combustions in homes, which you have just learnt about through in the demo. 77 Corrosion and Combustion Complete Worksheet 1 – Lesson 11 – Worksheet 5.6 Corrosion and Combustion 78 Success Criteria I can state the products of complete combustion I can state the products of incomplete combustion I can write chemical equations for combustion reactions 79 Lesson 12-13 - Neutralisation Reactions Learning Intention To be able to recognise neutralisation reactions and work out what the products will be. 80 Acids & Bases Acids are chemicals that taste sour, are corrosive, react with bases and have a low pH. Bases are chemicals that taste bitter, are caustic, have a slippery feel, react with acids and have a high pH. Examples of acids: vinegar, citrus juice, hydrochloric acid, sulphuric acid. Uses of acids: cleaning agents, to make fertiliser, to make carbonated drinks. Examples of bases: sodium hydroxide, ammonia, sodium carbonate. Uses of bases: cleaning products, soap-making, antacids. 81  These colours are only for universal indicator. Other indicators can tell you information about pH with different colours. A substance with a low pH is a hydrogen donor, one with a high pH is a hydrogen acceptor. pH stands for ‘power of Hydrogen’. When you mix the right amounts/concentrations together, you can 82 balance acids and bases out to make a neutral substance.  Neutralisation Reactions During a neutralisation reaction between an acid and a base, the pH decreases when acid is added to alkali (alkali = a dissolved base (aq)). The solution has been neutralised when a pH of 7 is achieved. If excess acid is added, then a low pH will be produced and the solution will be acidic. When approaching the pH7 end point (colour change), the titrate (what is in the burette) should be added one drop at a time. It can take one drop to make it neutral, and one to make it go too 83 far and become acidic.  tion Titration 84 Carrying out titrations When carrying out a simple acid-base titration, the following procedure is usually followed: Add the alkali to the conical flask Add the indicator to the alkali Add the acid quickly until you approach the predicted end point Add the acid slowly (drop by drop) to the alkali until the end point is reached. The end point is reached when the indicator changes to the appropriate colour. Your indicator will be pink in alkali, colourless in acid. You’re looking for the pink colour to permanently disappear. Single colour indicators are more accurate than universal 85 indicator. Acid-Alkali titrations – The Burette A burette is used to accurately decide on the volume of solution added. The scale reads downwards, not upwards, because as you open the tap at the bottom, the liquid exits. The reading on the scale tells you how much solution you have used. Each small division is worth 0.1mL. This makes it an accurate volume measurement. You need to read the volume using the bottom of the meniscus. This is the curved shape the solution has in the tube, like a sideways crescent moon. You also need to make sure you remove the funnel before you start. You will be using a pipette you won’t have used before to fill the conical flask, I will demo this for you and you should all have a go at using it. 86 Teacher demonstration Prac 1) Fill a burette with 1 M hydrochloric acid. If it ends in –ette, rinse it with what goes in it, everything else is rinsed with deionised water 2) With a pipette, accurately measure out 20 mL of 1 M sodium hydroxide and place it in the conical flask. 3) Add a few drops of phenolphthalein indicator to the flask. 4) Slowly add the acid until the mixture in the flask is no longer pink and record the titre volume (you need to swirl the flask as you reach the end point and stop as soon as the loss of pink is permanent). 87 Neutralisation Reactions Post demonstration activity sheet – on the portal Investigation 5.3: Pass the Salt. 88 Success Criteria I can state what is in a neutralization reaction I can state the general products of a neutralization reaction I can explain how to carry out a titration 89 Lesson 14 -Products of neutralisation Learning Intention OPTIONAL/MAY HAVE BEEN DONE: Complete PART 3 of the practical to obtain the salt produced To be able to recognise different types of reactions and work out what the names of any salts produced. 90 Neutralisation – naming salts 1 The first part of the name of the salt comes from the first name of the To name the base formed in a neutralisation: salt So Ammonium hydroxide gives ammonium ………… Magnesium oxide gives magnesium …………... 2 The acid gives the last part of the name of the salt. So Sulphuric acid make sulphates Nitric acid makes nitrates Hydrochloric acid makes chlorides Eg. Sodium hydroxide + nitric acid forms: Sodium nitrate Calcium carbonate + sulphuric acid forms: calcium sulphate 91 Naming salts - click to reveal Complete the word equations for the following neutralisation reactions. If carbon is present in the reactants, carbon dioxide will be produced as a product in addition to the salt + water Sodium hydroxide + sulphuric acid  sodium sulphate + water Calcium carbonate + hydrochloric acid  calcium chloride + carbon dioxide + water Copper oxide + nitric acid  copper nitrate + water 92 Knowledge Check – click to reveal Bicarb, or bicarbonate of soda, is a compound called sodium hydrogen carbonate, with the formula NaHCO3. Bicarb can be used to neutralise hydrochloric acid. (remember what is always produced in a neutralisation reaction) 1. Write a word equation for the reaction 2. Write a symbol equation for the reaction 3. If necessary, balance the equation 4. Add state symbols. Sodium hydrogen carbonate + hydrochloric acid  sodium chloride + carbon dioxide + water NaHCO3(s) + HCl(aq)  NaCl(aq) + CO2(g) + H2O(l) 5. Rate yourself, in %, for the above task. Have you 93 improved from the last time that you did this? Success Criteria I can name salts based on the acid and alkali that react 94 Revision Activities Ensure the booklet has been completed fully Complete A3 Revision sheet Complete practice tests and revision worksheets from the portal 95