Part of NCSSM CORE collection: This video shows the double displacement reaction of Pb(NO3)2 and KI. An aqueous solution of Potassium Iodide is added to an aqueous solution of Lead (II) Nitrate forming lead (II) iodide. 5. (ii) Finely divided substance is more effective as an adsorbent. Halide ions in solutions are detected using silver nitrate solutions. STATION Potassium Chlorate and Gummy bear. Gummy Station #3: Elephant toothpaste. Give reason for the following observations : (i) When Silver nitrate solution is added to Potassium iodide solution, a negatively charged colloidal solution is formed. The reaction produces a precipitate of AgBr, because it is insoluble. STATION #: INITIAL APPEARANCE: OBSERVATIONS: TYPE OF CHANGE: CLUE: BALANCE EQUATION: Station #1: Lead Nitrate and Potassium Iodide solutions. The nitric acid reacts with, and removes, other ions that might also form precipitates with silver nitrate. Video \(\PageIndex{1}\): Mixing Potassium Chromate and Silver Nitrate together to initiate a precipitation reaction (Equation \(\ref{4.2.1}\)). Note: This is an unusual reaction as the precipitate dissolves in excess iodide solution and disappears as a complex ion is formed. When dissolved they are present as a mixture of ions, Ag^(+), K(+), NO3(-), Cl(-) This means we have, in effect, 4 compounds, AgNO3, KCl, KNO3 and AgCl. Shower of yellow Station #2: Potassium Chlorate and Gummy bear. While full chemical equations show the identities of the reactants and the products and give the stoichiometries of the reactions, they are less effective at describing what is actually occurring in solution. Choose (4pts) Part : Mixing Lead(II) Nitrate with Potassium lodide (3pts) Record your observations for the mixing of lead(1nitrate with potassium iodide for each stage as prompted below Normal . Potassium iodide + silver nitrate potassium nitrate + silver iodide. The solution is acidified by adding dilute nitric acid. In this lesson, we will learn what molar heat of combustion is. The products of the reaction ... Observations Anode Cathode Potassium Iodide Sodium Chloride Copper(II) Bromide Post-Lab Questions 1. There will be no reaction under normal conditions because the potential for the reduction of magnesium ion is highly negative which means that it prefers to be oxidized rather than reduced. Lead (II) Nitrate and Potassium Iodide . Using silver nitrate solution. (iii) Lyophilic colloids are also called reversible sols. The formation of a precipitate occurs when the cations of one reactant combines with the anions of the other reactant to form an insoluble or slightly insoluble compound. The test solution is acidified using a few drops of dilute nitric acid, and then a few drops of silver nitrate solution are added. STATION #: Lead Nitrate and Potassium Iodide solutions INITIAL APPEARANCE: yellow liquid OBSERVATIONS: at first it did not dissolve and had like a lava lamp reaction TYPE OF CHANGE: chemical change CLUE: both liquids produced a different type of liquid not to a gas or solid 2. KI(aq) + AgNO 3 (aq) KNO 3 (aq) + AgI(s) A yellow white precipitate of silver iodide, AgI is produced. Elephant toothpaste Station #4: Copper and Nitric Acid. AgNO3 and KCl are ionic solids which are soluble in water. The electrolysis of aqueous silver nitrate (AgNO 3), for example, produces oxygen at the anode and silver metal at the cathode. This test is carried out in a solution of halide ions. 1. 6. Silver nitrate solution is then added, and the halide can be identified from the following products: