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Solubility Rules. Soluble: Group 1 and + NH4 compounds. Acetate (CH3COO-), Nitrate (NO3 Perchlorate (ClO4 -) compounds. Halide compounds (Cl-, Br-, I-) [except: Ag+, Pb2+, Hg2 2+] Sulfate compounds (SO4 2-) [except: Ag+, Pb2+, Hg2 2+, Mg2+, Ca2+, Sr2+, Ba2+] Insoluble: 5. Sulfide compounds (S2-) [except: Ca2+, Sr2+, Ba2+] 6.
The Solubility Rules 1. The nitrates, chlorates, and acetates of all metals are soluble in water. Silver acetate is sparingly soluble. 2. All sodium, potassium, and ammonium salts are soluble in water. 3. The chlorides, bromides, and iodides of all metals except lead, silver, and mercury(I) are soluble in water. HgI2 is insoluble in
30 Ιαν 2023 · When a substance is mixed with a solvent, there are several possible results. The determining factor for the result is the solubility of the substance, which is defined as the maximum possible concentration of the solute. The solubility rules help determine which substances are soluble, and to what extent.
GROUP I ALKALI METALS GROUP II ALKALINE EARTH METALS TRANSITION METALS POST-TRANSITION METALS Ammonium (NH 4 +) Lithium (Li+) Sodium (Na+) Potassium (K+) Magnesium
General Rules for Water Solubility of Simple Ionic Compounds1. Soluble Compounds. All nitrates and acetates. All compounds with alkali-metal (Li+, Na+, K+, etc.) and ammonium (NH +) cations. 4. The halides Cl–, Br–, and I–, except those of Pb2+, Ag+, Hg2 2+, which are insoluble.
In this experiment, aqueous solutions of several different ionic compounds will be used. Different combinations of solutions will be mixed and the results observed. For those mixtures in which precipitates form, the identity of the precipitate will be determined from the balanced chemical equation.
Zeros between non-zeros are significant. Zeros after non-zeros are significant if a decimal point is written. Exact numbers have infinite significant figures. Add/Sub: Lowest # of significant decimal places. Mult/Div: Lowest # of total significant figures.
