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Sulphate

Sulfate compounds arise when cations combine with the anion SO42-. Often this combination results in an ionic compound, although sulfates can engage in covalent bonding with most elements. The metal complex PtSO4P(C6H5)32 is clearly covalent Pt-O bonding. Dialkylsulfates, such as dimethylsulfate are covalent, distillable species. Many sulfate salts are highly soluble in water. Exceptions include calcium sulfate, strontium sulfate, and barium sulfate, which are poorly soluble.

- Aluminium Sulphate
- Ammonium Sulphate
- Aluminium Sulphat Ferric
- Barium Sulphate
- Basic Chromium Sulphate
- Ferrous Ammonium Sulphate
- Ferrous Ammonium Sulphate
- Lithium Sulphate
- Glauber,S salt
- Tin Sulphate
- Sodium Sulphate
- Manganese Sulphate
- Alum
- Aluminium Sulphate Non-Ferric
- Chromium Sulphate
- Calcium Sulphate
- Copper Sulphate
- Ferrous Sulphate
- Magnesium Sulphate
- Ferric Sulphate
- Stannous Sulphate
- Zinc Sulphate
- Potassium Sulphate


  Basic Chromium Sulphate

Appearance Fine Free Flowing, Spray Dried, Dark Green Color Powder Cr203 Cont. 25% + 1%
Basicity 33% + 2% PH 3 + 0.2
Presence Of Chromate Absent. Chrome Vi Content Absent.
Moisture Cont. 6% Maximum. Insoluble 0.2% Maximum.
Chrome Vi Content Absent




  Copper Sulphate

Copper Sulphate 97% Formula CuSO4.5H2O
Appearance Blue Crystal Assay 97.00% + - 1%
Cu Content 24.50% +_ 0.50% Insoluble 1% Max
Free Moisture 1% Max




  Ferrous Ammonium Sulphate

Mohr's Salt, ammonium iron sulfate, is a double salt of iron sulfate and ammonium sulfate, with the formula [NH4]4[Fe][SO4]4·6H2O. Mohr's salt is preferred over iron(II) sulfate for titration purposes as it is much less affected by oxygen in the air than iron(II) sulfate, solutions of which tend to oxidise to iron(III). The oxidation of solutions of iron(II) is very pH dependent, occurring much more readily at high pH. The ammonium ions make solutions of Mohr's salt slightly acidic, which prevents this oxidation occurring. The relevant equation for this is:
4 Fe2+ + O2 + (4+2x) H2O 2 Fe2O3.xH2O + 8 H+
The presence of protons keeps this equilibrium to the left, the Fe(II) side.



  Ferrous Sulphate

Formula: Fe(SO4).7H2O Assay. 97.00 % Min
Fe Content: 19.50% Min Appearance: Blue green crystals.
Solubility: 48.6 g/100 g water @ 50C (122F) Density: 1.90
Boiling Point: > 300C (> 572F) Decomposes. Melting Point: 57C (135F) Loses water




  Ferrous Ammonium Sulphate

Inhalation: Ingestion:Skin Contact: Eye Contact:
Causes irritation to the respiratory tract. Symptoms may include coughing, shortness of breath.Low toxicity in small quantities but larger dosages may cause nausea, vomiting, diarrhea, and black stool. Pink urine discoloration is a strong indicator of iron poisoning. Liver damage, coma, and death from iron poisoning has been recorded.Causes irritation to skin. Symptoms include redness, itching, and pain. May cause skin discoloration with irritation.Causes irritation, redness, and pain.


  Magnesium Sulphate

Purity as MgSo4 7H2O > 99% to 99.5% Magnesium Sulphate as MgSo4 > 48.5%
Magnesium Oxide as MGO > 16% to 17% Magnesium as Mg > 9.6%
PH of 5% aqueous solution 7 + 0.5 Sulphates of K and Ca < 0.1% each
Chlorides of K and Ca < 0.1% each Chlorides of Cl < 300 ppm
Heavy metals as Pb < 2 ppm Arsenic as As2O3 < 2 ppm
Iron as Fe < 20 ppm Calcium as Ca < 300 ppm



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  Lithium Sulphate

Inhalation: No information found, but compound should be handled as a potential health hazard. Inhalation may cause irritation to the upper respiratory tract. Symptoms may include coughing, shortness of breath and chest pain. Other symptoms may parallel those from ingestion.



  Ferric Sulphate

Appearance: Grayish-white powder or rhombic crystals. Odor: Odorless.
Solubility: Soluble in water. Density: 3.097 (Anhydrous)
% Volatiles by volume @ 21C (70F): 0 Melting Point: 480C (896F)





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