What are some non examples of precipitate?

Answer 1

Silver Chloride (AgCl)

Silver Bromide (AgBr)

Silver Iodide (AgI)

Barium Sulfate (BaSO4)

Calcium Carbonate (CaCO3)

to list a few...

Some Others:

BaCrO4 (not molecular - ion lattice)

PbSO4

Hg2SO4

BaSO4

CaSO4

Ca3(PO4)2

Fe(OH)3

Pb(OH)2

Al(OH)3

Co(OH)2

Cu(OH)2

CuS

NiS

Co2O3

Hg2Br2

Hg2Cl2

Hg2I2

AgCrO4

Ag3PO4

FePO4

Fe2S3

Fe2(CO3)3

PbCl2

PbBr2

PbI2

PbS

Some Notes on Solubility in H2O: (if a compound IS soluble it will NOT precipitate)

1. EXCLUDING NaOH and KOH (which are very soluble), many -OH salts are only slightly soluble [i.e. some may precipitate out of solution with lowered temperatures or high concentrations, ex: Ba(OH)2, Sr(OH)2, Ca(OH)2]

2. Similarly, many salts containing the following ions are also only slightly soluble (and may precipitate out of solution depending on the experimental conditions): S2-, CrO42- (above examples of precipitates), CO32-, PO33-

3. Alkali metal salts are usually soluble (i.e. salts with Li+, Na+, K+ etc.)

4. Most halide salts are soluble (Cl-, Br-, I-) EXCEPT when combined with Ag+, Pb2+, Hg22+ (see examples above) and a few other metals (esp. towards the right of the transition metals and into the "poor" metals on the Periodic Table) à in general, silver, lead and Mercury often lead to compounds that will precipitate out of water (Fe3+ can also lead to many precipitates)

Notable exception: Pb(NO3)2 IS soluble and WILL NOT precipitate out

5. Most sulfate (SO42-) salts ARE soluble (with some common exceptions listed above)

6. NO3- and NH4 salts are usually soluble

7. There are several phosphate salts that are insoluble (see above for examples)

Answer 2

Is a sloid product, witch may form when chemicals in two liquids react.

Answer 3

mixing vinegar and milk to make chunky milk.

Answer 4

The reaction between sodium chloride and silver nitrate give the silver chloride precipitate.

Answer 5

Weather without rain or snow, etc.

Answer 6

Snow;)

Answer 7

Hail