Question

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?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
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.
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.
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) 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
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...
At 25 °C, you conduct a titration of 15.00 mL of a 0.0460 M AgNO3 solution...
At 25 °C, you conduct a titration of 15.00 mL of a 0.0460 M AgNO3 solution with a 0.0230 M NaI solution within the following cell: Saturated Calomel Electrode || Titration Solution | Ag (s) For the cell as written, what is the voltage after the addition of the following volume of NaI solution? The reduction potential for the saturated calomel electrode is E = 0.241 V. The standard reduction potential for the reaction Ag+ + e- --> Ag(s) is...
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.
Find the concentration of I– in 0.050 M AgNO3 saturated with AgI. Include activity coefficients in...
Find the concentration of I– in 0.050 M AgNO3 saturated with AgI. Include activity coefficients in your solubility-product expression. The Ksp of AgI is 8.3× 10–17. A table of activity coefficients at various ionic strengths can be found here.(https://sites.google.com/site/chempendix/activity-coefficients-for-aqueous-solutions-at-25-c)
Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH. 1.What...
Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH. 1.What is the pH of the titration medium after the addition of the following volumes of NaOH titrant: F. 50.00 mL: G. 60.00 mL: H. 62.50 mL: I. 75.00 mL: J. 85.00 mL Can writer should how to find Ka1,Ka2, and Ka3?
Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH. A....
Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH. A. Write the net ionic equation for the reaction of phosphoric acid with NaOH to form sodium phosphate and water:
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT