Add 2 mL each of silver nitrate [AgNO3], lead nitrate [Pb(NO3)2] and mercury(I) nitrate[Hg(NO3)2] to the test tube. The chlorides formed are: AgCl, PbCl2, Hg2Cl2.
The mixture of the 3 above compounds once precipitated is added water and then heated to to 70C to get [Pb(NO3)2] to disolve it back into solution.
PRECIPITATION BY HCl:
(a) Add 1 mL of 6M HCl to the test tube.
Continue adding HCl in 1 mL increments until all of the original compounds have either precipitated as Unknown solids or dissolved as Unknown chlorides.
2.Write the net ionic equations for the formation of the 3 chlorides formed in step 1.
3. Write the net ionic equation for the dissolving of lead chloride in hot water.
4. Why do you need hot water to dissolve the lead chloride?© BrainMass Inc. brainmass.com October 24, 2018, 10:21 pm ad1c9bdddf
Net Ionic Reactions of Metal Chlorides are discussed and shown in detail.
A Selection of Net Ionic Equation from Reaction Problems
Can you please assist me in understanding what the name of the products and the net ionic equations are for the following mixtures?
-ammonia poured into aluminum nitrate
-barium chloride poured into sodium sulfate
-copper(II) chloride poured into sodium carbonate
-lead(II) nitrate poured into potassium iodide
-mercury(II) chloride poured into potassium iodide
-mercury(II) chloride poured into sodium carbonate
-sodium carbonate poured into calcium chloride; and then add hydrochloric acid
-sodium carbonate poured into hydrochloric acid
-sodium carbonate poured into water
-sodium chloride poured into potassium chloride
-sodium chloride poured into potassium nitrateView Full Posting Details