Question

A solution contains 0.018 mol each of I– , Br– , and Cl– . Use the...

A solution contains 0.018 mol each of I– , Br– , and Cl– . Use the Ksp values given below to determine how much AgCl(s) precipitates out when this solution is mixed with 200 mL of 0.24 M AgNO3. Ksp AgI = 1.5 x 10–16 Ksp AgBr = 5.0 x 10–13 Ksp AgCl = 1.6 x 10–10

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
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...
an aqueous solution contains 0.010M br and 0.010 M I. If AG+ is added until agbr(s)...
an aqueous solution contains 0.010M br and 0.010 M I. If AG+ is added until agbr(s) just begins to precipitate. what are the concentrations of ag and I? ksp of agbr = 5.4E-13, ksp of agi = 8.5E-17?
Determine if AgCl precipitates out of solution when 200 mL of 1.0x10x-4 M AgNO3(aq) is mixed...
Determine if AgCl precipitates out of solution when 200 mL of 1.0x10x-4 M AgNO3(aq) is mixed with 900 mL of 1.0x10-6M KCl(aq). Ksp AgCl = 1.6x10-10
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...)
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.
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.
Given the Ksp values for the following salts, determine the order that they would precipitate as...
Given the Ksp values for the following salts, determine the order that they would precipitate as AgNO3 is gradually added to a solution containing 0.01 M each of NaBr, Na2CrO4 and Na3PO4. Salt                              Ksp AgBr                     5.0 x 10-13 Ag2CrO4                9.0 x 10-12 Ag3PO4                 1.8 x 10-18 First: Second: Last:
Silver chloride has Ksp = 1.6 x 10-10 and silver chromate has Ksp = 9.0 x...
Silver chloride has Ksp = 1.6 x 10-10 and silver chromate has Ksp = 9.0 x 10-12. We have 1.00 liter of a solution which contains both NaCl (0.10 M) and Na2CrO4 (0.10 M). Solid AgNO3 is added slowly and the solution is stirred well. a) Which salt precipitates first, AgCl or Ag2CrO4? (Show your work!) b) What are the concentrations of [Ag+], [Cl-], and [CrO42-] at the point when the second salt just begins to precipitate? c) Is this...
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...
Can you please check my answers and tell me if they are correct? thanks 8. Write...
Can you please check my answers and tell me if they are correct? thanks 8. Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds: (a) PbCl2       PbCl2(s) --> Pb2+(aq) + 2Cl-(aq)                           Ksp = [Pb2+][Cl-]2   (b) Ag2S        Ag2S(s) --> 2Ag+(aq) + S2-(aq)                             Ksp =[Ag+]2[S2-] (c) Sr3(PO4)2 Sr3(PO4)2(s) --> 3Sr2+(aq) + 2PO43-(aq)         Ksp =[Sr2+]3[PO43-]2 (d) SrSO4       SrSO4(s) --> Sr2+(aq) + SO42-(aq)                       Ksp =[Sr2+][SO42-] 14. Assuming that no equilibria other than dissolution are involved,...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT