Question

What is the I– concentration just as AgCl begins to precipitate when 1.0 M AgNO3 is...

What is the I– concentration just as AgCl begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.0500 M Cl– and 0.0500 M I– ? (Ksp values: AgCl = 1.8×10−10 ; AgI = 1×10−16 ) (the halide ions could come from sodium salts...)

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
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 solution is 0.0010 M in both Ag+ and Au+. Some solid NaCl is added slowly...
A solution is 0.0010 M in both Ag+ and Au+. Some solid NaCl is added slowly until the second solid compound just begins to precipitate. What is the concentration of Au+ ions at this point? Ksp for AgCl = 1.8 x 10-10 and for AuCl is 2.0 x 10-13
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...
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.
Calculate the concentration (in M) of Ag+ when AgIO3 just begins to precipitate from a solution...
Calculate the concentration (in M) of Ag+ when AgIO3 just begins to precipitate from a solution that is 0.0275 M in IO3−. (Ksp = 3.17 ✕ 10−8)
. (8) A 10.00-mL portion of a 0.50 M AgNO3 (aq) solution is added to 100.0...
. (8) A 10.00-mL portion of a 0.50 M AgNO3 (aq) solution is added to 100.0 mL of a solution that is 0.010 M in Cl- a) Will AgCl (s) (Ksp = 1.8X10-10) precipitate from this solution? If so, how many moles will precipitate and what will be the concentrations of the ions after precipitation?
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) 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
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0220 M...
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0220 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants. (can be found here: https://sites.google.com/site/chempendix/Ksp ) [Ca^2+] = __________ M
What is the equilibrium constant for the dissolution of lead(II) chromate in Na2S2O3? For PbCrO4, Ksp...
What is the equilibrium constant for the dissolution of lead(II) chromate in Na2S2O3? For PbCrO4, Ksp = 2.0 x 10–16; for Pb(S2O3)34–, Kf = 2.2 x 106. (Use E for the power of 10) Solid AgNO3 is slowly added to a solution that contains 0.24 M of Cl− and 0.10 M of Br− (assume volume does not change). What is [Br−] (in M) when AgCl(s) starts to precipitate? Ksp of AgCl is 1.8 x 10−10. Ksp for AgBr is 5.0...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT