what is the solubility of copper 2 nitrate?
108866
the solubility of copper (II) nitrate is 138 g/100 ml of water at 0oC.
801118
CuCl2 + 2NH4OH --> Cu(OH)2 + 2NH4Cl\n\nCu(OH)2 (s) + 4NH3 (aq)     ----->     Cu(NH3)4^2+
945429
Equation becomes CuCl2 + 2KI --> CuI2 + 2KCI\n\nProducts are Cuprous Iodide and Potassium Chloride
712818
more soluble in what solution?
721562
Beryllium sulfate, in the anhydrous form, absorbs water to become the tetrahydrate immediately upon contact.\n\nThe solubility of the tetrahydrate form in cold water is 42.5 grams/100 mL of water at 25°C.  The solubility in boiling water (100°C) is 100 grams/100 mL water.
187439
the first answer is wrong, all nitrates are soluble, you learn that in first year chemistry. Therefore the precipitate cannot be ammonium nitrate. Althought i have no answer yet myself for the question, i do know the 1st answer cannot be correct.
513514
Crystallization of solution of CuSO4.
726370
There should be no reaction.  Provided there is enough water to dissolve the CuCl, the Compounds would separate into their Ion counterparts.\n\nSo, youd end up with Cu+, K+, and Cl- in solution
793636
shawty's NOT good at stoichiometry...has made a fundamental error in the final line so end result is rubbish...\nhow can you end up with MORE Cu than you started with when it's 2 moles : 2moles? \n\n(8/159)x 127 = 6.4 g
748872
Cu2+ (aq)  +  Zn (s) -->  Cu (s) + Zn2+ (aq)
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.
916529
d) Cu I\n\nChromic and phosphoric acid are polyprotic acids and the salts will show a decreasing solubility with increasing pH as the higher pH favours the formation of chromate and phosphate.\n\nHydroIodic acid is a strong acid and is fully dissociated and the the amount of iodide formed depends on concentration and not pH. Thus CuI solubility will show no dependence on pH.
964608
There's quite a few. Just google solubility chart. Here's one I found.
606075
Cu(s) + 4HNO3 (aq)--> Cu(NO3)2(aq) + 2H2O(l) +2NO2(g)
24810
Cu + 2H2SO4 --> 2H2O + SO2 + CuSO4\nDouble the H2SO4 and the H2O.
387399
Pb2+ + Cl- ---> PbCl2\n\nWe know that the lead in Pb(NO3)2 has to have a 2+ charge because a nitrate ion has a 1- charge, so two of them is a 2- charge.  The entire compound must have no charge, so a 2+ charge is assigned to the lead. \n\nBoth compounds Pb(NO3)2 and NaCl dissociate (they are both soluble), and because nitrate and Na+ ions are always soluble, they can be ignored in a net ionic equation.
64690
NA2SO4,KOH,AGCL,CA(NO3)2 ARE SOLUBLE.AND HG2BR2 AND CDS IS INSOLUBLE.