Four-part question set: A chemist dissolves 30.0 g of potassium phosphate in one

Question

Four-part question set: A chemist dissolves 30.0 g of potassium phosphate in one beaker of water and 30.0 g of silver(l) nitrate in a second beaker of water. When the two solutions are poured together, a solid precipitate forms. Write a balanced molecular equation, determine the identity of the limiting reactant, and predict the expected mass of solid product. (Ignore equilibrium.) What is the identity of the solid product? Add together all the coefficients in the balanced equation. What is the total? What is the identity of the limiting reactant? What is the predicted mass of the solid product?

Explanation / Answer

K3PO4(s) + AgNO3(s) --> in water

K3PO4(aq) + 3AgNO3(aq) --> Ag3PO4(s) + 3KNO3(aq)

mol of K3PO4 = mass/MW = 30/212.27 = 0.1413

mol of AgNO3 = mass/MW = 30/169.87 = 0.1766

Ratio is 1:3 so

0.1413 mol of K3PO4 --> 3*0.1413 = 0.4239 AgNO3

clearly, AgNO3 is limiting

Q28.

Identity of solid is Silver Phosphate

Q29

total balance:

1+3 = 3+1 ---> 8

Q30

clearly, AgNO3 is limiting

Q31

mass of precipitate formed

0.1766 mol of AgNO3 --> 1/3 mol of Ag3PO4

0.1766 mol --> 0.05886 mol of Ag3PO4

mass = mol*MW = 0.05886 *418.5760 = 24.6373 g of Ag3PO4 will be produced

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