Question

. (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?

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 100.0 ml portion of 0.250 M copper (ii) chloride is combined with 100.0 ml of...
A 100.0 ml portion of 0.250 M copper (ii) chloride is combined with 100.0 ml of 0.250 M potassium phosphate, resulting in the formation of a plate blue precipitate. Part (A): what is the mass of the precipitate formed? Part (B): how many moles of the excess reagent remain after the precipitation? I need help with this question please.
Suppose that 31.3 mL of 0.487 M NaCl is added to 31.3 mL of 0.245 M...
Suppose that 31.3 mL of 0.487 M NaCl is added to 31.3 mL of 0.245 M AgNO3. Write a balanced molecular equation for the reaction. Include physical states for all reagents and products. How many moles of AgCl would precipitate? What are the concentrations of each of the ions in the reaction mixture after the reaction occurs?
13.A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2....
13.A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2. (8 points) a.Write the balanced molecular equation for the reaction. b.Write the net ionic equation for the reaction. c.How many grams of precipitate will form? What is the concentration of Ag+, NO3‒, Ca2+, and Cl‒in the final solution (assume volumes are additive)
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
When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.300 M NH4Cl,...
When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.300 M NH4Cl, how many extra mLs of excess reactant were used? AgNO3 (aq) + NH4Cl(aq) → AgCl(s) + NH4NO3 (aq)
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.
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
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)
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...)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT