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# the question reads: a) balance the equation: H3PO4 + Ca(OH)2 --> Ca3(PO4)2 + H2O b)what mass of each product results if 750 mL of 6.00 M H3PO4 reacts...

a) balance the equation:
H3PO4 + Ca(OH)2 --> Ca3(PO4)2 + H2O
b)what mass of each product results if 750 mL of 6.00 M H3PO4 reacts according to the equation?
i balanced it with:
2H3PO4 + 3Ca(OH)2 --> Ca3(PO4)2 + 6H2O
but i'm not sure where to go from there
also,
A solution is made by dissolving 26.42 g of (NH4)2SO4 in enough H2O to make 50.00 mL of solution.
a) what is the molar mass of (NH4)2SO4?
b) what are the products of the solution?
c) how many milliliters of solution are needed?
i got:
a) 196g/mol
b) (NH4)2SO4 + H2O --> NH4O + SO4H
c) 2.7 M
i'm sure a and c is right.. just unsure about b
sorry for the long post, thanks !

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