what happens when barium chloride is mixed with copper sulfate. i need this for a lab?
97980
Barium sulfate will precipitate. The reaction is\n\nCuSO4(aq)+ BaCl2(aq)---> 2CuCl(aq)+ BaSO4(s)
806586
Usually the salts of Cu2+ - like CuSO4 - forms blue colored solutions. But it is not the only. Some cobalt salts also form blue colored solutions.
903862
Sorry Voyager. Copper is not so reactive a metal that it will react with sulphuric acid.\nYou need either solid copper (II) carbonate or solid copper (II) oxide for the salt.\nSince it is a sulphate, sulphuric acid is used together with the solid.\nHeat the acid so that the reaction can proceed at a faster rate. Add solid till no more will react (no bubbles of gas produced, and the solid remains insoluble). This is to ensure that all the acid is used up. Filter to remove unreacted solid and heat the filtrate, which is the copper (II) sulphate solution, till saturated (approximately 1/3 to half the original volume left would be a good gauge). Let the hot saturated copper (II) sulphate solution cool and after some days, when the excess water evaporates off, you should get hydrated copper (II) sulphate crystals.\nDo not heat till dryness as this will evaporate off the water of crystallization needed for the blue copper (II) sulphate crystals to form. Without the water of crystallization, you would get anhydrous copper (II) sulphate powder (white) and not the blue crystals.\n\nHope this helps :)
1086041
all the information you need is in the handy periodic table.   First, think about the charges of the molecules....\n\n In the molecule CuSO4, copper has two electrons to give.  The SO4 molecule wants TWO more electrons to acheive noble gas configuration (a stable electron state).   This appears to be a match in heaven.  \n\nWell all is fine until Zinc comes along.  If you look at the periodic table, Zinc is just to the right of copper.  It too has 2 electrons to donate......but, it is more electronegative than copper. (remember, electronegativity  is the lowest in the bottom left corner of the table(Fr) and increases on  a diagonal path  with F being the most electronegarive.)  \n\nSince Zinc is more reactive than Copper,  a replacement reaction occurs.  Zinc bumps Copper off of the SO4 molucule.  Zinc can be whitiish to yellowish in solution.  As all the Zinc is coming off the rod, it bumps the copper off the SO4 and also disperses the colour of the copper.  If you had one drop of blue dye (the copper), but added a cup of milk. ( the Zinc)...... you would barely see the blue color.
387822
Barium is a group II metal, therfore the most stable ion is Ba2+
200130
definitely sulphate... lol...ne ways, u gotta mix those stuff n leave it over nite to crystalise..then break it to pieces..or, u can jus ask ur chemistry teacher..haha.. all i did in sch was crystalizing copper sulphate usin the solution itself..
66513
http://en.wikipedia.org/wiki/Copper%28I%29_chloride
159504
You know, I answered exactly the same question not 2 days ago.\n\nAnhydrous copper sulfate and water would be the easiest two. \n\nYou can buy copper sulfate at any good garden supply shop and most larger hardware stores. The copper sulfate usually sold is hydrated, and is already blue in colour.\n\nYou can make it anhydrous by putting it the oven, uncovered on a sheet of tin foil at 160oC or hotter. You will know when it has become anhydrous beause it goes white. This is quite safe to do in your kitchen oven, all you are doing is driving off the water. No nasty fumes or residues are produced.\n\nStore the crystals in an airtight jar to stop them absorbing water from the air. When you are ready add some water to a few crystals they will retrun to their original blue colour.\n\nThe other possibility is to manufacture your own cabbage indicator. That will make a bluish purple colour when mixed with baking soda. I've included a link with instruction on how to do this.
277199
CuSO4 . 5H20 -> CuSO4 + 5H2O\n\nIt is just a hydrate so basically you are just getting water out of the salt. Copper(II) sulfate pentahydrate is blue while CuSO4 is a white salt.
242316
Add up the charges in the molecule. Like, in ClO4-,\n\nOxygen has an oxidation state of -2 by default. Therefore, Cl must have an oxidation state of +7 to balance out the oxygens. Notice that 7 + (-2)*4 = -1, which is the charge of the ion.\n\nThe oxidation state of Pb in PbSO4 is +2, because the sulfate ion has an charge of -2. To balance this out, the Pb must be +2, as there is no charge on the molecule.\n\nHope this helped.
174475
mix it...let NaCl dissolve in water...then let the mmixture evaporate or perhaps bring the mixture into a boil 'til you can see the formation of crystals...   try it... i've encountered such experiment in my chemistry class... im not quite certain of the procedures though...it's two years ago...cant remember it well...^_^
413983
Copper sulphate as I recall.
566694
i would imagine you'd have issues with electrochemical reactions between the copper and the various heavy metals in the tailings.  This of course is completley dependant on what is contained in your specific tailings, and what the concentrations of these metals are.  Overall, talk to an engineer familiar with the site for more details
750179
NaCl2 + NaCO3 ==> NaCO3 + NaCl2 NOTE: these two reactants will not react because the reactants and the products are identical\n\nCu + O2 ==> CuO2   This is already balenced\nCuSO3 + Fe ==> FeSO3 + Cu   The charge is not given so procuts could be different\n\n2HCl + 2Zn ==> 2ZnCl + H2\nMnO2 + H2O2 ==> No reaction: similar to NaCl2+NaCo3\n\nGood luck
471546
A.  Iodine is being reduced from +5 in HIO3 to 0 in I2; oxygen is being oxidized from -1 in H2O2 to 0 in O2.\n\nB.  There is no oxidation/reduction going on; this is simple metathesis, producing the barium sulfate precipitate.
1153335
barium acetate and carbon dioxide and water
748872
Cu2+ (aq)  +  Zn (s) -->  Cu (s) + Zn2+ (aq)