Answer to Question #113878 in General Chemistry for Jose

Question

Identify the products for the following reaction and whether they would be (aq) or (s): CaBr (aq) + AgNO3 (aq) —> *

CaAg (aq) + BrNO3 (s)
Ca(NO3)2 (s) + BrNO3 (s)
Ca(NO3)2 (aq) + AgBr (s)
CaAg (s) + BrNO3 (aq)

What volume of water would be required to make a 0.25 M solution with 2 moles of Ba(OH)2?

0.625 L
0.10 L
1.0 L
10 L

Answer 1

Solution (1):

Equation: 2AgNO₃(aq) + CaBr₂(aq) →  Ca(NO₃)₂(aq) + 2AgBr(s)

Ionic Equation:

2Ag⁺(aq) + 2NO₃^-(aq) + Ca²⁺(aq) + 2Br^-(aq) → Ca²⁺(aq) + 2NO₃^-(aq) + 2AgBr(s)

Net Ionic Equation: 2Ag⁺(aq) + 2Br^-(aq) → 2AgBr(s)

Or: Ag⁺(aq) + Br^-(aq) → AgBr(s)

Answer (1): Ca(NO₃)₂(aq) + AgBr(s).

Solution (2):

Molarity of Ba(OH)₂ = Moles of Ba(OH)₂ / Volume of solution

Volume of solution = Moles / Molarity

Volume of solution = (2 mol) / (0.25 M) = 8 L.

The actual volume of water will be somewhat less than that since the 2 moles of Ba(OH)₂ will occupy some volume.

However, suppose that:

Volume of solution = m(H₂O) = 8 L.

Answer (2): 8 Liters of water.