when does a solid compound form when you are writing ionic equations of a molecular equation?

Question

1)Li3PO4(aq) + Sr(OH)2(aq)

net ionic> Li3PO4(aq) + Sr(OH)2 > Li3(OH)2(s) +PO4Sr (aq)

was Li3(OH)2 the right solid and why or why not?
thanks

Answer 1

I think you meant to say "Ironic". You're stupid.

Answer 2

See the solubilty table for help:

http://intro.chem.okstate.edu/1515SP01/Database/Solub.html

Net ionic needs to be broken down into ions, but first you need to write out your double-replacement reaction and then balance the equation!

You also need to balance your charges...do this first, or else balancing will be hell.

Charges are easy...charges are assigned for metals according to column #: Li = +1, Sr= +2

Polyatomic ions you need to learn, but you can deduce from subscript of metal (PO4 must be -3 since Li has 3)

Hydroxide (OH)= -1

This means the products are: Li(OH) + Sr3(PO4)2

Now you need to balance.

Using solubility table, you see that all hydroxides are insoluble except for Group 1A etc. Li is in column 1A (group 1), so it would be dissolved in solution. Phosphates are insoluble except for group 1A and ammonia. Since Sr is in group 2A, this is your solid.

Lastlt, be sure you always write the positive ion first (PO4Sr is incorrect).

Good luck!

Answer 3

You're welcome!!