![]() Pb(NO3)2 and Na2CO3When Lead (II) Nitrate and Sodium Carbonate it produced Sodium Nitrate and Lead Carbonate as a precipitate.Pb(NO3)2 + Na2CO3 -> Na2NO3 + PbCO3The precipitate has got Whitecolour. ![]() Pb(NO3)2 + KNO3 -> KNO3 + PbNO3The precipitate’s colour is transparent white. Pb(NO3)2 and KNO3When Lead (II) Nitrate and Potassium Nitrate react with each other it produced equal products as reactants because Potassium take place of Lead and Lead takes place of Potassium so it produced same. Pb(NO3)2 and NaClWhen Lead (II) Nitrate react with Sodium Chloride it produced Sodium Nitrate and Lead (II) chloride.Pb(NO3) + 2NaCl ->2NaNO3 + PbCl2The precipitation has got white colour. The precipitation is Lead Iodide.Pb(NO3)2 + 2KI -> 2KNO3 + PbI2The precipitation’s colour is Yellow. Reactions with Lead (II) NitratePotassium nitrate and Lead Iodide are formed when Lead (II) Nitrate react with Potassium Iodide. AgNO3 + FeCl3-> Fe(NO39 + AgCl3↓The precipitate colour was light Yellow. ĪgNO3 and FeCl3Iron Nitrate and Silver Chloride are produced when Silver Nitrate reacts with Iron(III) Chloride. AgNO3 + Na2CO3 -> Na2CO3 + Ag2CO3↓Precipitate’s colour is light Green. The precipitate is Silver Sulphate.AgNO3 + CuSO4-> Cu(NO3)2 + Ag2SO4The colour of precipitate is light blue.ĪgNO3 and Na2CO3Silver Nitrate and Sodium Carbonate react to form Sodium Nitrate and Silver Carbonate. ĪgNO3 and CuSO4Copper nitrate and Silver Sulphate are formed when Silver Nitrate and Copper Sulphate react with each other. ĪgNO3 and NaClWhen we add a small quantity of Sodium Chloride solution to Silver Nitrate solution it produce Sodium Nitrate and a precipitate of Silver Chloride.AgNO3 + NaCl-> NaNO3 + AgCl↓ Precipitate has got white colour. AgNO3 + KI -> KNO3 + AgI↓Precipitate has got a Yellow colour. Reactionswith AgNo3When we add a small quantity of Potassium Iodide to Silver Nitrate two compounds are produced Potassium Nitrate and a precipitate of Silver Iodide. We clean the test tubes and dispose of the wastes in the waste container.And finally we write correctly equations for all of the reactions where a precipitate is formed. We do the same with Pb(NO3)2 and with CaCl2. We add 6 drops of AgNO3 solution to every test tube.We have to observe and record information and colour of any precipitate formed. Procedure of these reactionsWe put 21 clean test tubes in a test tube rack.We add 6 drops of the solutions indicated which are: KI,NaCl, NaOH, FeCl3, KNO3, Na2CO3, CuSO4 to 7 clean test tube. MaterialsThe material which we need are following: Pb(NO3)2 CaCl2KI NaClNaOH FeCl3Na2CO3 CuSO4AgNO3 Test tubesKNO3 Test tubes rack PurposePurposeThe purposes of this experiment are:To observeprecipitationreactionsbymixingaqueoussolutions of cations and anions.To write and balancecompletechemicalequations for precipitationreactions In effect, the compounds change partners with each other. Introduction Double Replacement ReactionsA double displacement reaction involves the reaction of two compounds to form two new compounds. ![]() Instead, you must begin by identifying the various reactions that could occur and then assessing which is the most probable (or least improbable) outcome.Precipitation in Double Displacement ReactionsPIERRE COMASCRISTINA RÍOS Nothing could be further from the truth: an infinite number of chemical reactions is possible, and neither you nor anyone else could possibly memorize them all. ![]() Students tend to think that this means they are supposed to “just know” what will happen when two substances are mixed. As you advance in chemistry, however, you will need to predict the results of mixing solutions of compounds, anticipate what kind of reaction (if any) will occur, and predict the identities of the products. So far, we have always indicated whether a reaction will occur when solutions are mixed and, if so, what products will form.
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