This question is about Preparation of Salts that was sent to me by one of my Sec 4 Pure Chemistry student.
Before we take a look at the question, let’s recap that there are 3 main methods to prepare salts in the laboratory:
- Titration
- Acids + Excess Insoluble Substances
- Precipitation
If you need more information on Preparation of Salts, you can go to my earlier blogposts under archives.
Let’s take a look at the question.
Question:
A student was given two beakers, one containing an aqueous solution of sodium chloride and the other aqueous lead (II) nitrate. He was told to prepare lead (II) chloride using those reagents.
(i) What is the name of the method that he used to prepare the salt?
(ii) Name the other? product made, besides lead (II) chloride
(iii) Write an ionic equation for the preparation.
In the process of doing the experiment, he accidentally spilled some of the salt solutions. Since he could not obtain sufficient lead (II) chloride, he tried to prepare more lead (II) chloride by adding solid lead (II) carbonate to dilute hydrochloric acid. Effervescence was seen but the reaction stopped in a short while.
(iv) Why was there effervescence?
(v) Why was he unsuccessful in preparing lead (II) chloride from the process of adding dilute hydrochloric acid to lead (II) carbonate?
Go try it out and leave your answers (and workings) in the Comment Section below.
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