Question

Calculate the equilibrium concentration of Ag+(aq ) in a solution that is initially 0.200 M AgNO3...

Calculate the equilibrium concentration of Ag+(aq ) in a solution that is initially 0.200 M AgNO3 and 0.710 M NH3, and in which the following reaction takes place: $$ (Kf = 1.70x107)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

[Ag+] = 1.2241E-7

If you have any doubts about the answer please mention in the comments please do rate the answer.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.200 M AgNO3...
Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.200 M AgNO3 and 0.800 M KCN. The formation constant for [Ag(CN)2]- (aq) is Kf = 1.0 x 10^21 *PLEASE SHOW ICE TABLE AS WELL, THANKS!!!*
Calculate The concentration of Ag+  present in solution at equilibrium when equilibrium concentration of [NH3] =0.20 M....
Calculate The concentration of Ag+  present in solution at equilibrium when equilibrium concentration of [NH3] =0.20 M. The initial Ag(NH3)2+ concentration is 0.010M. The Kf of Ag(NH3)2+ is 1.7 x 107. Ag+(aq)+ 2NH3(aq)--- >Ag(NH3)2+(aq)
Calculate the concentration of Ag+ present in solution at equilibrium when concentrated ammonia is added to...
Calculate the concentration of Ag+ present in solution at equilibrium when concentrated ammonia is added to a 0.013 M solution of AgNO3 to give an equilibrium concentration of [NH3] = 0.17 M. The formation constant for Ag(NH3)2+ at this temperature is 1.7 × 107. How do you solve a problem like this? Thanks!
Calculate the equilibrium constant Kc for the net reaction show below AgI(s) + 2NH3(aq) <> Ag(NH3)2+(aq)...
Calculate the equilibrium constant Kc for the net reaction show below AgI(s) + 2NH3(aq) <> Ag(NH3)2+(aq) + I-(aq) For AgI, Ksp=8.3*10^-17 For Ag(NH3)2+ , Kf=1.5*10^7
Question 1   : We have a solution that has a concentration of 0.321 M for A(aq)...
Question 1   : We have a solution that has a concentration of 0.321 M for A(aq) and 0.618 M for B(aq). There are no other solutes initially. The reaction 2 A(aq) + B(aq) <---> 2 C(aq) + D(aq) takes place. At equilibrium, the concentration of C(aq) is 0.158 M. What is the equilibrium constant of this reaction?
For the following cell at 25 Celsius: Ag+ +e—>Ag(s)=0.80V Cu2+ +2e—>Cu(s)=0.34V (Cu(s)|CuCl2(aq)||AgNO3(aq)|Ag(s)) 1) what is the...
For the following cell at 25 Celsius: Ag+ +e—>Ag(s)=0.80V Cu2+ +2e—>Cu(s)=0.34V (Cu(s)|CuCl2(aq)||AgNO3(aq)|Ag(s)) 1) what is the equilibrium constant under standard conditions? 2)what is the cell potential if the concentration of the AgNO3 solution was changed to 0.500 M, and all other conditions remained the same? 3)Calculate delta Grxn for part 2
Given the following equilibria at 25oC: AgCl(s) <----> Ag+(aq) + Cl-(aq); Ksp = 1.6 x 10-10...
Given the following equilibria at 25oC: AgCl(s) <----> Ag+(aq) + Cl-(aq); Ksp = 1.6 x 10-10 Ag+(aq) + 2NH3(aq) <----> Ag(NH3)2(aq); Kf = 1.7 x 107 What are the equilibrium concentration of Ag+ in the saturated solution?
You mix 5.00 mL of 1.0x10^-5 M AgNO3 with 10.00 mL of 2.00 M NH3 solution...
You mix 5.00 mL of 1.0x10^-5 M AgNO3 with 10.00 mL of 2.00 M NH3 solution resulting in the formation of diamminesiler(I) complex ion, [Ag(NH3)2]. (Assume volumes are additive). a. Write the net-ionic equilibrium equation for the formation of this complex ion. b. Calculate the concentration of the complex ion in the reaction mixture, assuming the reaction goes to completion.
Calculate the equilbrium concentration of Zn2 (aq) in a solution that is initially 0.150 M Zn(NO3)2...
Calculate the equilbrium concentration of Zn2 (aq) in a solution that is initially 0.150 M Zn(NO3)2 and 0.800 M NaCN. The formation constant for [Zn(CN)4]2- (aq) is Kf = 2.1 x 1019. Please show all of your work and include any formulas you use! Thank you!
Calculate the Kf for the following reaction. 1) Ag+ (20 mL of aqueous 0.02 M solution...
Calculate the Kf for the following reaction. 1) Ag+ (20 mL of aqueous 0.02 M solution as the nitrate salt). 2) Na2CO3 (1 mL of aqueous 1 M solution). Once the precipitate is formed, add NH3 (1 mL of aqueous 3 M solution) to form the complex ion Ag(NH3)2 +
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT