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Chemistry
OpenStudy (anonymous):

i have to re write each reaction as a balanced net ionic equation. Ca(s)+MgSO4(AQ)->CaSO4(aq)+Mg BaCl2(aq)+K2So4(aq)->BaSo4(s)+2KCl

OpenStudy (rogue):

Alright, you have to identify the things that will dissociate and the things that are insoluble. Sulfates are generally soluble; they are insoluble when combined with Ag+, Ca2+, Sr2+, Ba2+, and Pb2+. For your first reaction, MgSO4 dissociates and CaSO4 remains an insoluble precipitate. So your net ionic is \[Ca(s)+Mg^{2+} (aq) +SO_4^{2-}(aq) \rightarrow CaSO4(aq)+Mg (s)\]Can you do the second one on your own from this?

OpenStudy (rogue):

Also, halides (Cl-, Br-, I-) are generally soluble as well; they are insoluble when combined to Ag+, Pb2+, Hg2 2+.

OpenStudy (anonymous):

idk if im doing the second one right

OpenStudy (rogue):

For the second one, everything is soluble except BaSO4.\[Ba^{2+} (aq) + 2Cl^- (aq)+2K^+ (aq) +SO_4^{2-} (aq)\rightarrow BaSO_4(s)+2K^+ (aq)+ 2Cl^- (aq)\]Cancel out terms that appear on both sides.\[Ba^{2+} (aq)+ SO_4^{2-} (aq) \rightarrow BaSO_4 (s)\]

OpenStudy (anonymous):

you did it likes it nothing lol im reading it over and over and its like ... but thanks :D

OpenStudy (anonymous):

for Na2Co3(aq)+Ca(OH)2(aq)->2NaOH(aq)+CaCo3(s) idk if im right but is net ionic equation for it

OpenStudy (anonymous):

idk how to write the exponents the way you do but is it Na2^+ + Co3^-(aq)+Ca(OH)2(aq)->2NaOH(CaCo3(s)

OpenStudy (rogue):

The NaOH & Ca(OH)2 both dissociate. The only insoluble product is CaCO3.

OpenStudy (anonymous):

hmm im lost but i think i got it lol :X

OpenStudy (rogue):

\[Na_2CO_3(aq)+Ca(OH)_2(aq)\rightarrow2NaOH(aq)+CaCO_3(s)\]\[2Na^+ + CO_3^{2-}+Ca^{2+} + 2OH^- \rightarrow2Na^+ + 2OH^- +CaCO_3\]\[CO_3^{2-} (aq) +Ca^{2+} (aq) \rightarrow CaCO_3 (s)\]

OpenStudy (anonymous):

oooo i was almost right! but thanks

OpenStudy (rogue):

It takes some practice at first, but it'll become easy later on :)

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