# Problem: How many grams of barium phosphate (molar mass= 601.93 g ) are produced by mixing 209.28 mL of 0.182 M barium nitrate with 127.80 mL of 0.173 M sodium phosphate?  3Ba(NO3)2 + 2Na 3PO4 → Ba3(PO4)2 + 6NaNO3A) 7.64 gramsB) 13.3 gramsC) 6.65 gramsD) 4.44 gramsE) 22.9 grams

###### FREE Expert Solution
82% (107 ratings)
###### Problem Details

How many grams of barium phosphate (molar mass= 601.93 g ) are produced by mixing 209.28 mL of 0.182 M barium nitrate with 127.80 mL of 0.173 M sodium phosphate?

3Ba(NO3)2 + 2Na 3PO→ Ba3(PO4)2 + 6NaNO3

A) 7.64 grams

B) 13.3 grams

C) 6.65 grams

D) 4.44 grams

E) 22.9 grams

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofHow many grams of barium phosphate (molar mass= 601.93 g ) a...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Sabrina took 7 minutes and 38 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Costanza's class at USF.