Only need last three Solubility Rules:edncone ueu e cobonugWater Soluble CompoundsG Qu llae of worlofnimemer uoy1. Salts of ammonium (NH4*) and Group IA are always soluble.2. Salts containing nitrate (NO3-), acetate (C2H3O2-), or chlorate (CIO3-) ions arealways soluble.rolleo 1ol Xoo3. Salts of the halides are soluble with the following exception:JeulJon ernirtilyns pniobprirdolewof Inola. Compound containing Ag*, Hg2+, Pb²*4. Salts containing the sulfate ion (SO42-) are soluble with the exceptionelgmsx3a. Compounds containing Ag*, Hg2+, Pb2+, Ca2*, Sr2*, or Ba2+Water Insoluble Compoundsent ef1. Salts of the carbonate (CO32-), phosphate (PO43-), chromate (CrO42-), or sulfides(S2-) ions are insoluble with the exception of compound containing group 1A orammonium cations.2. Salts containing the hydroxide ion (OH-) are insoluble with the exception ofcompounds containing group 1A, ammonium cations, or Ba2+.Soluble means that it dissolves in water while insoluble means that it is not soluble inwater and will precipitate out of solution as a solid. 1. For each of the following compounds, list whether they are soluble or insoluble inwater and explain the solubility rule that tells you that. Use the solubility rules givenin the introduction of the lab.RuleCompoundSolubilityAl203NH4CICa(OH)2Na2CO3AgFH93PO4XXX

Na2CO3 is soluble in waterAgF is soluble in water Hg3PO4 is in soluble in water

Answered: Na2CO3 AgF Hg3PO4

Science

Chemistry

Na2CO3 AgF Hg3PO4

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Only need last three

Solubility Rules:
edncone ueu e cobonug
Water Soluble Compounds
G Qu llae of worl
ofni
memer uoy
1. Salts of ammonium (NH4*) and Group IA are always soluble.
2. Salts containing nitrate (NO3-), acetate (C2H3O2-), or chlorate (CIO3-) ions are
always soluble.
rolleo 1ol Xoo
3. Salts of the halides are soluble with the following exception:
Jeul
Jon er
nirtilyns pniob
prirdolew
of Inol
a. Compound containing Ag*, Hg2+, Pb²*
4. Salts containing the sulfate ion (SO42-) are soluble with the exception
elgmsx3
a. Compounds containing Ag*, Hg2+, Pb2+, Ca2*, Sr2*, or Ba2+
Water Insoluble Compounds
ent ef
1. Salts of the carbonate (CO32-), phosphate (PO43-), chromate (CrO42-), or sulfides
(S2-) ions are insoluble with the exception of compound containing group 1A or
ammonium cations.
2. Salts containing the hydroxide ion (OH-) are insoluble with the exception of
compounds containing group 1A, ammonium cations, or Ba2+.
Soluble means that it dissolves in water while insoluble means that it is not soluble in
water and will precipitate out of solution as a solid.

1. For each of the following compounds, list whether they are soluble or insoluble in
water and explain the solubility rule that tells you that. Use the solubility rules given
in the introduction of the lab.
Rule
Compound
Solubility
Al203
NH4CI
Ca(OH)2
Na2CO3
AgF
H93PO4
XXX

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