One of the questions I have to answer is: "Characterize the following compounds as soluble or insoluble in water: (a) CaCO3, (b) ZnSO4, (c) Hg(NO3)2, (d) HgSO4, (e) NH4ClO4"
What I don't understand is how to recognize soluble and insoluble compounds. Please help!
2006-09-04 08:44:15 · 13 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
It is simple how to recognise soluble and insoluble compounds.
U must memorise the SOLUBILITY RULES.They are:
1.All salts of trioxonitrate(v) (NO3-) are soluble.
2.All salts of Na+,K+ and NH4+ are soluble
3.All tetraoxosulphate(vi)salts are soluble except those of Ca2+,Pb2+ and Ba2+.
4.All chlorides,bromides and iodides are soluble except those of Pb2+ and Ag+
5.All trioxosulphate(iv) salts are insoluble except those of Na+,K+ and NH4+.
6.All sulphides are insoluble except those of Na+,K+ and NH4+.CaS is sparingly soluble.
7.All oxides and Hydroxides are are insoluble except those of Na+,K+ and NH4+.Ca(OH)2 is slightly soluble.
8.All trioxocarbonate(IV) salts are insoluble except those of NH4+,Na+ and K+.
Therefore from the salts listed above
(a)CaCO3 is insoluble
(b)ZnSO4 is soluble
(c)Hg(NO3)2 is soluble
(d)HgSO4 is soluble
(e)NH4ClO4 is soluble
2006-09-04 09:31:15 · answer #1 · answered by Albert F 2 · 1⤊ 1⤋
First, I would tell you to go to the library and look in Lange's Handbook of Chemistry (15th Edition), a classic reference that covers the entire field of chemistry including solubilities.
Second, compounds may be soluble in solvents other than water.
Third, compounds differ to the extent they are soluble and there are solubility constants for every compound. That is, a compound may be slightly soluble in water while part of it remains a precipitate.
Lastly, it is very difficult to "recognize" which compounds may be soluble in water or not, although ionic compounds are more likely and this can be predicted based on their ionization potential, another characteristic that can be found in the Handbook.
2006-09-04 08:58:03 · answer #2 · answered by Skyeman 2 · 0⤊ 0⤋
Solubility in water will depend largely on the type of chemical bonding the molecule has. Certain factors like temperature and the size of the molecule will also have an influence.
For example, chemicals with ionic bonds are mostly soluble in water, whilst those of metallic bonds will have no solubility in water.
CaCO3, like most carbonates, is very insoluble in water (that's the stuff your bones are mostly made of, imagine if they were soluble in water! You're almost 80% water!)
ZnSO4 is very soluble in water, like most sulphates are.
Hg(NO3)2 is soluble in water, like most nitrates are.
HgSO4 has a very unstable bond, thus it decomposes in water and is not considered soluble.
NH4ClO4 is a tricky one, while NH4Cl will dissolve easily in water, but when those oxigen ions get in the way it makes it only partially soluble in water, to 200g per litre.
Here's a bit of reference in regards to this matter.
http://en.wikipedia.org/wiki/Solubility
http://en.wikipedia.org/wiki/Solubility_chart
And here's the most comprehensive:
http://www.chem.lsu.edu/lucid/tutorials/solubility/Solubility.html
2006-09-04 09:08:07 · answer #3 · answered by flammable 5 · 0⤊ 1⤋
-All phosphate salts are insoluble except for ammonium salts and group IA compounds therefore it is soluble -All nitrate salts are soluble -All metal hydroxides are insoluble -All potassium salts are soluble The only ones insoluble in water are Calcium Phosphate and Zinc hydroxide
2016-03-26 22:00:13 · answer #4 · answered by Anonymous · 0⤊ 0⤋
All things are soluble, it just depends on in what solvent!
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2006-09-04 08:46:40 · answer #5 · answered by Anonymous · 0⤊ 1⤋
Soluble dissolves
2006-09-04 08:49:51 · answer #6 · answered by Jet 6 · 0⤊ 0⤋
All sodium, potassium and ammonium salts are soluble.
All chlorides are soluble except lead and silver.
All nitrates are soluble.
All Sulphates are soluble except lead, barium and calcium.
All carbonates are insoluble except sodium, potassium and ammonium.
2006-09-08 07:01:20 · answer #7 · answered by carbon dioxide 2 · 0⤊ 0⤋
FeO, CuCo3, Mq3(Po4)2, NaHCO3
2016-02-27 15:49:55 · answer #8 · answered by ? 1 · 0⤊ 0⤋
Combine
Shake
Observe
2006-09-04 08:49:49 · answer #9 · answered by da_hammerhead 6 · 0⤊ 1⤋
I suppose it would be too easy to just drop some in water, huh?
2006-09-04 08:50:00 · answer #10 · answered by auntb93again 7 · 0⤊ 0⤋