How do you balance this reaction: #?Na_3PO_4(aq) + ?CaCl_2(aq) -> ?NaCl(aq) + ?Ca_3(PO_4)_2(s)#?

1 Answer
anor277
Jan 2, 2017

As always, we must balance mass and charge............

Explanation:

#2Na_3PO_4(aq) + 3CaCl_2(aq) rarr 6NaCl(aq) + Ca_3(PO_4)_2(s)darr#

Are charge and mass balanced here?

As a matter of fact, this is a simplified version of what occurs in solution. Phosphates in water are commonly the #"biphosphate ion"#, #HPO_4^(2-)#.

The reaction is probably better represented as:

#Na_2HPO_4(aq) + CaCl_2(aq) rarr 2NaCl(aq) + Ca(HPO_4)(s)darr#

But you have to go with what your teacher says, not what I say.

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