Question

Balance the equation and show the calculation of the number of moles and grams of Ca3(PO42 formed from 10.8 grams of Ca(OH)2. Show your answers to 3 significant figures Ca(OH)2 H3PO4-- Ca3(PO4)2 + H2O]

Answer 1

The number of moles of calcium phosphate is 0.0485 mol. The mass is 15.1 g.

Step-by-step explanation:

The balanced equation is:

`3 Ca(OH)_(2) + 2 H_(3)PO_(4) => Ca_(3)(PO_(4))_(2) + 6H_(2)O`

As we can see, 3 moles of calcium hidroxide produced 1 mol of calcium phosphate. So the quantity of moles of Calcium posphate is:

`10.8g Ca(OH)_(2)*(1 molCa(OH)_(2))/(74.093gCa(OH)_(2)) *(1mol Ca_(3)(PO_(4))_(2))/(3molCa(OH)_(2)) =0.0485 molCa_(3)(PO_(4))_(2)`

The mass of calcium phosphate in grams is:

`0.0485 molCa_(3)(PO_(4))_(2)*(310.176g)/(mol) =15.1 g`