The substance is toxic to aquatic organisms.Īll rights reserved. TLV: (as Cr(III), inhalable fraction): 0.003 mg/m 3, as TWA (DSEN) (RSEN) A4 (not classifiable as a human carcinogen).
#Solubility of chromium sulfate skin#
Repeated or prolonged contact may cause skin sensitization. The substance is irritating to the respiratory tract.Ī harmful concentration of airborne particles can be reached quickly when dispersed.Įffects of long-term or repeated exposure With the financial assistance of the European Commission.ĭecomposes on heating. Prepared by an international group of experts on behalf of ILO and WHO, If appropriate, moisten first to prevent dusting. Sweep spilled substance into covered containers. Vacuum spilled material with specialist equipment. Do NOT let this chemical enter the environment. Personal protection: particulate filter respirator adapted to the airborne concentration of the substance. Give one or two glasses of water to drink. Rinse skin with plenty of water or shower.įirst rinse with plenty of water for several minutes (remove contact lenses if easily possible), then refer for medical attention. Use local exhaust or breathing protection. We would use this molar mass just like we did above to calculate the moles of the compound in solution.In case of fire in the surroundings, use appropriate extinguishing media. In this case, if the problem stated that we were dealing with the pentahydrate, we would have to add five times the molar mass of water to our result for the anhydrous molar mass to get the total molar mass of the hydrate (148.06 g/mol + 18.02 g/mol * 5 = 238.16 g/mol for the hydrate).
Regardless, if you are ever doing one of these problems and you are dealing with a hydrate, you would take that into account during the molar mass calculation. After googling the compound, I found that the pentahydrate was soluble in water, and that chromium (III) sulfate was insoluble, but couldn't seem to find much on the anhydrous form of the compound. The problem states that the compound is dissolved and then water is added until the volume of the solution is 375 mL, but I was curious about the solubility of the compound in water. And so, by dividing by the solution volume again, we can see that the concentrations of both the chromium cation and the sulfate anion are the same as that of the overall solution, or 0.346 M. If, per se, 0.12968 moles of chromium sulfate molecules dissolved, we would expect 0.12968 moles of chromium ions and 0.12968 moles of sulfate ions to be in solution. If a dozen chromium (II) sulfate molecules dissolved, we would expect a dozen chromium ions and a dozen sulfate ions to be in solution. Therefore, when the compound dissolves, we would expect one chromium ion and one sulfate ion for every chromium (II) sulfate molecule. We already figured this out earlier when we determined the chemical formula, and so we can see that one chromium ion and one sulfate ion form the chromium (II) sulfate compound. Now, if we want to know the concentration of the individual ions, we need to know how many of each ion is in the undissolved compound. We should report this to the number of significant figures given in the question, which is 3, and so our answer is 0.346 M. To get from milliliters to liters, we divide the number of milliliters by 1000, so 375 mL is 0.375 L. To find the molarity, we divide the number of moles by the volume of the solution in liters. Now, to calculate the moles in solution, we take the mass added to the solution and divide by the molar mass: From there, we can calculate the molar mass using the molar masses of the individual elements and the number of atoms in the compound: Therefore, a neutral compound will have equal amounts of chromium and sulfate, and so we should expect a chemical formula of CrSO 4. Sulfate ions have a -2 charge, and the "(II)" in "chromium (II)" means that the chromium has a +2 charge. To do that, we will need the molar mass of the chromium (II) sulfate, and to determine the molar mass, we need to know the chemical formula. The first thing we need to do is determine the amount of chromium (II) sulfate present in the solution in moles.
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