Question

If 0.040 mol AgNO3 and 0.10 mol KI are added to 200.0 mL of water, what...

If 0.040 mol AgNO3 and 0.10 mol KI are added to 200.0 mL of water, what concentration of Ag+ remains in the solution once equilibrium is established? The Ksp of AgI is 8.5 X 10-17.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to...
A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10) A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10)
a) A 0.1500 M of AgNO3 solution was employed to titrate a 25.00 mL of 0.1250...
a) A 0.1500 M of AgNO3 solution was employed to titrate a 25.00 mL of 0.1250 M of NaI and 0.2500 M NaCl. Given that Ksp, AgI(s) = 8.3*10-17, and Ksp, AgCl(s) = 1.8*10-10, please calculate the concentration of Ag+ ion after 6.00 mL of AgNO3 was added. b) please calculate the pAg after 100.00 mL of AgNO3 was added
a) A 0.1500 M of AgNO3 solution was employed to titrate a 25.00 mL of 0.1250...
a) A 0.1500 M of AgNO3 solution was employed to titrate a 25.00 mL of 0.1250 M of NaI and 0.2500 M NaCl. Given that Ksp, AgI(s) = 8.3*10-17, and Ksp, AgCl(s) = 1.8*10-10, please calculate the concentration of Ag+ ion after 6.00 mL of AgNO3 was added. Answer: 1.2 x 10-15 M b) please calculate the pAg after 100.00 mL of AgNO3 was added Answer: 1.35 I just want to see how they got that.
A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to...
A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10)
Consider the titration of 25.00 mL of 0.1250 M AgNO3 with 0.05012 M KI. ksp =...
Consider the titration of 25.00 mL of 0.1250 M AgNO3 with 0.05012 M KI. ksp = AgI(s) = 8.3*10-17. 1)  For the same titration as shown in Question 2, please calculate the pAg value after 90.00 mL of KI is added. 2)  For the same titration as shown in Question 2, please calculate the volume of KI that is required to reach a pAg of 2.00.
Consider the titration of 25.00 mL of 0.1250 M AgNO3 with 0.05012 M KI. Ksp, AgI(s)...
Consider the titration of 25.00 mL of 0.1250 M AgNO3 with 0.05012 M KI. Ksp, AgI(s) = 8.3*10-17. please calculate the volume of KI that is required to reach a pAg of 2.00. Answer is 47.82 mL. How they got that?
1. a. 0.0500 M of AgNO3 is used to titrate a 25.00-mL containing 0.1000 M sodium...
1. a. 0.0500 M of AgNO3 is used to titrate a 25.00-mL containing 0.1000 M sodium chloride (NaCl) and 0.05000 M potassium iodide (KI), what is the pAg of the solution after 15.00 mL of AgNO3 is added to the solution? Ksp, AgCl (s) = 1.82 x 10-10; Ksp, AgI(s) = 8.3*10-17. b. Same titration as in (a), what is the pAg of the solution after 25.00 mL of AgNO3 is added to the above solution? c. Same titration as...
Consider the titration of 25.00 mL of 0.1250 M AgNO3 with 0.05012 M KI. Ksp, AgI(s)...
Consider the titration of 25.00 mL of 0.1250 M AgNO3 with 0.05012 M KI. Ksp, AgI(s) = 8.3*10-17. For the same titration as shown in Question 2, please calculate the volume of KI that is required to reach a pAg of 2.00.
A 125.0 −mL sample of a solution that is 2.9×10−3 M in AgNO3 is mixed with...
A 125.0 −mL sample of a solution that is 2.9×10−3 M in AgNO3 is mixed with a 230.0 −mL sample of a solution that is 0.12 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?
A 125.0 −mL sample of a solution that is 2.9×10−3 M in AgNO3 is mixed with...
A 125.0 −mL sample of a solution that is 2.9×10−3 M in AgNO3 is mixed with a 225.0 −mL sample of a solution that is 0.12 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?