is CaSO4 soluble in water at the .1-M level?
349631
CaSO4 (Calcium Sulfate) is soluable in everything exept for Ag2+, Ca2+, Sr2+, Ba2+, and Pb2+. i am not going to lie to you and tell u that i know y this occurs but if i were to guess i would say that it was because CaSO4 is an ionic compound.
141058
sodium sulfte is soluble, but barium sulfate would form as a precipitate. Thus\n\nBaNO3 + Na2SO4 -> BaSO4 + 2 NaNO3, or simply\n\nBa(2+) + SO4(2-) -> BaSO4
874827
It could be, but it generally is not.\n\nA solution is a homogeneous mixture of a solute (in this case (NH4)2SO4) and a solvent (unknown in this case).\nIt is possible have solutions which are solids, but generally when one refers to solutions, one means "aqueous" solutions, meaning that they are dissolved in water.\nThe above poster, "☺ Mathew ☺", is wrong in his generalization of solutions to mean aqueous solutions.\n\nAmmonium Sulfate is soluble in water.  At 25 degrees C, (NH4)2SO4 has a solubility of about 44.22 g/mL.\nhttp://www.jtbaker.com/msds/englishhtml/A6192.htm
666223
methane wouldnt really dissolve in water.  KCl would ionize in water to become K+ and Cl-.  Helium wouldn't dissolve in water.  MgSO4 would also ionize in water.  Sucrose would dissolve in water to a significant extent, because of hydrogen bonding.  Sucrose has lost of hydroxyl groups in its structure and allow it to hydrogen bond in water, therefore dissolving.  Sodium bicarb would also just ionize.
838558
Of course. Take any compound that is not very soluble in water.\nThe saturated solution will have a very low concentration of this compound. E.g a saturated solution of CaCO3 is approximately 5.8*10^-5 M
1125846
NaVO3, MW = 122 g/mol\n\n100 mM = 0.1 M, so 0.1 moles in 1 L.  Dissolve 12.2g in water, dilute to 1L.
884562
Doesn't matter how much you started with.  The final amount remaining in the water at 20 will be 0.22g/100mL of solvent.\n\nSo your system will deposit 1.53g of SA at 20C.
364233
Yes, of course "salt" (table salt) can dissolve in water.\n\nThereare, however, many types of salts.  "Salt" is a general term refering to an ionic compound formed with a metal cation (+) and a non-metal anion (-), but it has come to commonly refer to table salt [NaCl] by most common people.\nSince salts are ionic compounds, they are soluble in water.  Some salts are very soluble, others only slightly, others are almost totally insoluuble.\nSodium Chloride (NaCl) is very soluble, but other salts like Silver Chloride (AgCl) are almost totally insoluble.\n\nHave you ever heard of the "like dissolves like" rule?  It states that polar solvents (like water) can dissolve ionic or polar solutes (like salt).  Non-polar solvents will dissolve non-polar solutes.\nThe polar water molecules will surround the Ions making up the salt, breaking it up into ions and placing it in solution.\n\nWhen you dissolve table salt in water, it forms an aqueous solution of Na+ and Cl- ions.\nSince the Na+ ion has a positive charge, it is surrounded by the Oxygen end of a water molecule which has a slight negaitve charge due to the two lone pairs of electrons surrounding it and the difference in electronegativity between the Oxygen and the Hydrogen atoms.  Since the Chloride ion has a negative charge, it is surrounded by the Hydrogen side of the water molecule.\n\n\n"corrupted_bunny" doesnt know what she is talking about.  Table salt very much so dissolves in water.  Melting is a completely different process than dissolving.
560067
According to the solubility rules, it is insoluble.\n\nHere are the solubility rules\n1. All common compounds of Group I and ammonium ions are soluble. \n\n2. All nitrates, acetates, and chlorates are soluble. \n\n3. All binary compounds of the halogens (other than F) with metals are soluble, except those of Ag, Hg(I), and Pb. Pb halides are soluble in hot water.) \n\n4. All sulfates are soluble, except those of barium, strontium, calcium, lead, silver, and mercury (I). The latter three are slightly soluble. \n\n5. Except for rule 1, carbonates, hydroxides, oxides, silicates, and phosphates are insoluble. \n\n6.Sulfides are insoluble except for calcium, barium, strontium, magnesium, sodium, potassium, and ammonium.
76843
Yes, these are both very water soluble.  All ammonium salts and group one salts (like sodium) are water soluble.  I have personally worked with both of them.  I can tell you that ammonium chloride dissolves very endothermically; it's so cold that it's hard for me to hold when I'm dissolving a lot of it in a test tube of water.  \nAmmonium chloride: 29.7g/100g water @ 0°C\nSodium carbonate: 30 g/100 ml (20 °C)
36586
Ag+ + SO4(2-) ---> Ag2SO4\nYeah, it's double replacement, and according to my solubility rules, AgSO4 is insoluble.
1075365
Dinitrogen oxide is somewhat soluble in water and it will simultaneously also get oxidized to give NO2 as brown fumes. NO2 will further dissolve in water to give nitric and nitrous acid. \n\nN2O (g) --------> NO2(g)  (in water)\nNO2(g) + H2O(l) ------> HNO3(aq) + HNO2(aq)\n\nIndustrially, CuSO4 is made by first heating scrap Cu with sulphur:\n\nCu(s) + S(s) -----> CuS(s)\n\nThe sulphide is then oxidized by heating it in excess air:\n\nCuS(s) + O2(g) ---------> CuSO4(s)\n\nIn the lab, you can heat some dilute H2SO4 in a beaker and then add excess of copper(II) oxide a little at a time and stir. You'll get a blue solution of CuSO4 and a black precipitate of the excess CuO which didn't react with the acid. By filteration, you'll separate the precipitate and get CuSO4 solution as a filterate which you can heat gently and then cool to obtain crystals.
479476
You need to know concentrations to determine the amount of substance that precipitates out by using solubility products. In this case the precipitate will be CaSO4, so the solubility product will be given by:\n\nk=[Ca(+2)]*[SO4(-2)]\n\nWhere k is the equilibrium constant (probably a given), and [Ca(+2)] & [SO4(-2)] are the concentrations of Ca(+2) and SO4(-2) in the solution. Any amounts greater than the equilbrium concentration will precipitate out as a solid.
903130
Na2SO4(aq)+ 2 AgNO3(aq)-->Ag2SO4(s)+ 2 NaNO3(aq).
663838
I agree with Thinkstoomuch's Answers in most part.  \n\nSolid Cu, C will not be soluble in water.  However glucose and  CuBr2 will be soluble in water.  At STP solubility of glucose (C6H12O6) is about 90g/ml.  That eliminates choice 1 and 3.\n\nWhen a compound ionizes in soln it makes electrolyte.  Glucose will not ionize but CuBr2 will ionize to Cu++ and 2Br-, choice 4 can be eliminated.\n\nThe third clue is just there to confirm your answer and CuBr2 being an ionic compound will indeed have a relatively high melting point.  498°C to be exact.  \n\nClearly, Cupric Bromide should be your Answer.\n\nI hope this helps.
83196
I've usually made up a concentrated stock of various buffers and dilute it to the concentration I need.  From a 1M Tris stock it's a 1/100 dilution to 10mM and from a 1M MgCLs it's a 1/1000 dilution.  I would decide how many milliters I wanted to make, measure out the cesium powder then pipette out the amount of each Tris (1/100 of the total solution vulume) and Mg (1/1000 of the volume) then bring to the final volume with distilled water.  This works fine if the concentrated solutions don't interact and cause precipitates or something else like being nearly a saturated solution.
712912
BaI2(aq) + MgSO4(aq)  --> BaSO4(s) + MgI2(aq)\n\nSo BaSO4 will precipitate.