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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Textbook Question
Chapter 16, Problem 103CWP
A 50.0-mL sample of 0.0413 M AgNO3(aq) is added to 50.0 mL of 0.100 M NaIO3(aq). Calculate the [Ag+] at equilibrium in the resulting solution. [Ksp for AgIO3(s) = 3.17 × 10−8.]
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Given the equation:
Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq) ?f=2.00×10^7
determine the concentration of NH3(aq) that is required to dissolve 295 mg of AgCl(s) in 100.0 mL of solution. The ?sp of AgCl is 1.77×10^−10.
I've worked this through several times, but I am just not coming up with the right answer! Thanks :)
11.An acid-base equilibrium system is created by dissolving 0.15 mol HNO2 in
water and diluting the resulting solution to a volume of 1.0 L. What is the effect
of adding 0.020 mol NO2 (aq) to this solution? How will pH change (calculate pH
before and after the addition. For HNO2 Ka = 4.5 x 104)? How will
concentrations of HNO2 and NO2 at equilibrium change?
Write the equilibrium expression for the reaction:
Zn2+(aq) + 2NH3 (aq) = Zn(NH3)2+(aq)
Chapter 16 Solutions
Chemistry
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