## Chemistry: The Central Science (13th Edition)

Published by Prentice Hall

# Chapter 17 - Additional Aspects of Aqueous Equilibria - Exercises - Page 770: 17.69b

#### Answer

No precipitation will occur.

#### Work Step by Step

1. Find $[Ag^+]$ $[Ag^+] = [AgNO_3] = C_f$ $C_i * V_i = C_f * V_f$ $* V_f = 10ml + 100ml = 110ml$ $0.05 * 0.10 = C_f * 0.11$ $C_f = 0.0455 = [Ag^+]$ 2. Find $[SO_4^{2-}]$: $[SO_4^{2-}] = [Na_2SO_4] = C_f$ $0.05 * 0.01 = C_f * 0.11$ $C_f = 0.00455 M = [SO_4^2-]$ 3. Calculate the product of the concentrations for $Ag_2SO_4$: $P = [SO_4^{2-}][Ag^+]^2$ $P = 4.55 \times 10^{-3} * (4.55 \times 10^{-2})^2$ $P = 4.55 \times 10 ^{-3} * 2.070 \times 10^{-3}$ $P = 9.419 \times 10^{-6}$ 4. Compare this product with the Ksp: $Ksp (Ag_2SO_4)= 1.3 \times 10^{-5}$ $P = 9.419 \times 10^{-6}$ Since the Ksp value is higher, there will be no precipitations.

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.