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Question
(i) What is observed when a solution of potassium iodide is added to a solution of lead nitrate taken in a test tube?
(ii) What type of reaction is this?
(iii) Write a balanced chemical equation to represent the above reaction.
Solution
i) When a solution of potassium iodide is added to a solution of lead nitrate taken in a test tube, the precipitation of a yellowish solid is observed. This yellowish solid is lead iodide. Potassium nitrate is formed along with lead iodide.
(ii) This is a double displacement reaction.
(iii) The balanced chemical equation for the above reaction is:
2KI(aq) + Pb(NO3)2(aq) —→ 2KNO3(aq) + PbI2(s)↓
Potassium Lead Potassium Lead
iodide nitrate nitrate iodide
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When a potassium iodide solution is added to a solution of lead (II) nitrate in a test tube, a precipitate is formed.
List two types of reactions in which this reaction can be placed.
Which option denotes a double displacement reaction?
Write balanced chemical equation for the following word equation.
Lead nitrate + Potassium iodide → Lead iodide + Potassium nitrate
Is this a double displacement reaction? Justify your answer. Name the compound precipitated and write the ions present in it.
Give an example of a double displacement reaction.
