Question

A solution is made from 25 mL of 2.00x10^-2 M AgNO3 and 10mL of 6.00 x10^-2...

A solution is made from 25 mL of 2.00x10^-2 M AgNO3 and 10mL of 6.00 x10^-2 M Na3AsO4. The Ksp of Ag3AsO4 is 1.00 x10^-22. Does a precipitate form? Show all calculations.
Ag3AsO4 (s) <----> 3 Ag+(aq) + AsO4^3- (aq)

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) 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.
. (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?
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...
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 130.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with...
A 130.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with a 220.0 −mL sample of a solution that is 0.13 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains? Answer with 2 sig. figures.
A 130.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with...
A 130.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with a 220.0 −mL sample of a solution that is 0.13 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains? Answer with 2 sig. figures.
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?
A 115.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with...
A 115.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with a 230.0 −mL sample of a solution that is 0.14 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT