Asked by Boo Boo
Determine whether a solid forms when solutions containing the follow salts are mixed. If so, write the ionic equation and the net ionic equation.
a: Na3PO4 and AgNO3
b: K2SO4 and Na2CO3
C: Pb(NO3)2 and Na2CO3
d: BaCl2 and KOH
a: Na3PO4 and AgNO3
b: K2SO4 and Na2CO3
C: Pb(NO3)2 and Na2CO3
d: BaCl2 and KOH
Answers
Answered by
DrBob222
You need to learn (read that memorize) the solubility rules. Here is a simplified set.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
For a I know that Ag3PO4 is insoluble.
The net ionic equation is
3Ag^+(aq) + PO4^-(aq) ==> Ag3PO4(s)
For b I know that K2CO3 and Na2SO4 are soluble.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
For a I know that Ag3PO4 is insoluble.
The net ionic equation is
3Ag^+(aq) + PO4^-(aq) ==> Ag3PO4(s)
For b I know that K2CO3 and Na2SO4 are soluble.
Answered by
Kaitlyn
Determine whether a solid forms when solutions containing the following salts are mixed. If so, write the ionic equation and the net ionic equation.
KCl and Na2S
KCl and Na2S
Answered by
Brandi
no
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