Log in
Chemistry
1
answer
0
watching
257
views
10 Nov 2019

Given the following at 25 C:



AgBr(s) <---> Ag+(aq) + Br-(aq) Ksp = 5.0 x 10^-13


Ag+(aq) + 2S2O3^2-(aq) <---> Ag(S2O3)2^3-(aq) Kf = 2.9 x10^13



and



AgBr(s) + 2S2O3^2-(aq) <---> Ag(S2O3)2^3-(aq) + Br-(aq) Kc= 14.5



1. Calculate the solubility (in mol/L) of AgBr in 0.50 M Na2S2O3solution.



2. How many grams of AgBr can dissolve in 500 mL 0.50 MNa2S2O3?

Watch
1
answer
0
watching
257
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Deanna Hettinger
Deanna HettingerLv2
24 Jun 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions


Show all your steps for calculation questions in order to get full points.

1. (4 pts) The solubility product (Ksp) of the insoluble salt AgBr is 5.0 x 10-13. Calculate the equilibrium constant for the following reaction: Ag+(aq) + Br-(aq) AgBr(s).

2. (6 pts) A solution is prepared by adding 50.0 mL of 0.050 M HCl to 150.0 mL of 0.10 M HNO3.

a. Calculate the pH of the solution.

b. Calculate the concentrations of all species in this solution.

3. (4 pts) Calculate the volume of concentrated (12 M) HCl needed to prepare 1-L of a pH = 1.50 solution?

4. (5 pts) Arrange the following 0.10 M solutions in order of most acidic to most basic.

KOH, KCl, KCN, NH4Cl, HCl

5. (6 pts) Calculate the pH of an aqueous solution containing 1.0 x 10-2 M HCl and 1.0 x 10-2 M HCN.

6. (5pts) Carbonate buffers are important in regulating the pH of blood at 7.40. What is the concentration ratio of CO2 (usually written H2CO3) to HCO3- in blood at pH=7.40?

H2CO3(aq) HCO3-(aq) + H+(aq) Ka = 4.3 x 10-7

7. (10 pts) HCN gas, a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka = 6.2 x 10-10) when dissolved in water. If a 50.00-mL sample of 0.100 M HCN is titrated with 0.100 M NaOH, calculate the pH of the solution:

a. before the titration starts.

b. after 8.00 mL of 0.100 M NaOH has been added.

c. at the half-way point of the titration.

d. at the equivalence point of the titration.

Show all your steps for calculation questions in order to get full points.

1. (4 pts) The solubility product (Ksp) of the insoluble salt AgBr is 5.0 x 10-13. Calculate the equilibrium constant for the following reaction: Ag+(aq) + Br-(aq) AgBr(s).

2. (6 pts) A solution is prepared by adding 50.0 mL of 0.050 M HCl to 150.0 mL of 0.10 M HNO3.

a. Calculate the pH of the solution.

b. Calculate the concentrations of all species in this solution.

3. (4 pts) Calculate the volume of concentrated (12 M) HCl needed to prepare 1-L of a pH = 1.50 solution?

4. (5 pts) Arrange the following 0.10 M solutions in order of most acidic to most basic.

KOH, KCl, KCN, NH4Cl, HCl

5. (6 pts) Calculate the pH of an aqueous solution containing 1.0 x 10-2 M HCl and 1.0 x 10-2 M HCN.

6. (5pts) Carbonate buffers are important in regulating the pH of blood at 7.40. What is the concentration ratio of CO2 (usually written H2CO3) to HCO3- in blood at pH=7.40?

H2CO3(aq) HCO3-(aq) + H+(aq) Ka = 4.3 x 10-7

7. (10 pts) HCN gas, a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka = 6.2 x 10-10) when dissolved in water. If a 50.00-mL sample of 0.100 M HCN is titrated with 0.100 M NaOH, calculate the pH of the solution:

a. before the titration starts.

b. after 8.00 mL of 0.100 M NaOH has been added.

c. at the half-way point of the titration.

d. at the equivalence point of the titration.

e. after 52.00 mL of 0.100 M NaOH has been added.

8. (5 pts) Calculate the Ksp value. For bismuth sulfide (Bi2S3), which has a solubility of 1.0 x 10-15 mol/L at 25⁰C.

9. (5 pts) Arrange the following group of salts: in order of most soluble to most insoluble.

AgI (Ksp= 1.5 x 10-16), CuI (Ksp= 5.0 x 10-16) and CaSO4 (Ksp= 6.1x 10-5)

e. after 52.00 mL of 0.100 M NaOH has been added.

8. (5 pts) Calculate the Ksp value. For bismuth sulfide (Bi2S3), which has a solubility of 1.0 x 10-15 mol/L at 25⁰C.

9. (5 pts) Arrange the following group of salts: in order of most soluble to most insoluble.

AgI (Ksp= 1.5 x 10-16), CuI (Ksp= 5.0 x 10-16) and CaSO4 (Ksp= 6.1x 10-5)

6 What is the molar solubility of cadmium hydroxide,Cd(OH)2 in pure water at 25 oC? Note thatKSP for Cd(OH)2 is 5.3 x 10-15 at25 oC

IMPORTANT: Enter your answer in scientific notation to 2significant figures. For example, if your answer is 9.8765432 x10-1, you should enter 9.9E-1. Failure to adhere to thisformat may cause WebCT to mark your answer as incorrect.

7 In the previous problem, you calculated the solubility ofCd(OH)2 in mol/L. What is this solubility in mg/L? Notethe following atomic weights: Cd 112.411 O 15.9994 H 1.0079

IMPORTANT: Enter your answer in floating point to 1 decimal place.For example, if your answer is 9.876543210, you should enter 9.9.Failure to adhere to this format may cause WebCT to mark youranswer as incorrect <?xml:namespace prefix = o ns ="urn:schemas-microsoft-com:office:office" /?>

8 In the previous two problems, you looked at the solubility ofCd(OH)2 in pure water. Now consider a 0.50 MCd(NO3)2. Cadmium nitrate,Cd(NO3)2 is a freely soluble salt. When a0.50 M Cd(NO3)2 is prepared, the cadmiumnitrate dissolves without establishing an equilibrium:

Cd(NO3)2(s) ==========>Cd2+(aq) + 2NO3-(aq)

In a 0.50 M Cd(NO3)2 solution, theconcentration of Cd2+ will be 0.50 mol/L. When theCd(OH)2 is dissolved in this solution, it establishesits usual equilibrium between the solid and the ions insolution:

Cd(OH)2(s) <----------> Cd2+(aq) +2OH-(aq)

However, the presence of Cd(NO3)2 in thissolution means there will be Cd2+ ions in solution evenbefore the Cd(OH)2 dissolves. What is the molarsolubility of Cd(OH)2 in a 0.50 MCd(NO3)2 solutioN

9. In problem 6, you calculated the molar solubility ofCd(OH)2 in distilled water, and in problem 8, youcalculated the molar solubility of Cd(OH)2 in a 0.50 MCd(NO3)2 solution. Now consider a 0.50 M NaClsolution. Sodium chloride, NaCl is a freely soluble salt. When a0.50 M NaCl solution is prepared, the NaCl dissolves withoutestablishing an equilibrium:

NaCl(s) ==========> Na+(aq) +Cl-(aq)

In a 0.50 M NaCl solution, the concentration of Cl- willbe 0.50 mol/L. When the Cd(OH)2 is dissolved in thissolution, it establishes its usual equilibrium between the solidand the ions in solution:

Cd(OH)2(s) <----------> Cd2+(aq) +2OH-(aq)

The Cd2+ ions then react with the Cl- ionsfrom NaCl to form a complex ion:

Cd2+(aq) + 4Cl-(aq) <---------->[CdCl4]2-(aq)

Note that the formation constant for[CdCl4]2-, Kf is 1.0 x104.

IMPORTANT: Enter your answer in scientific notation to 2significant figures. For example, if your answer is 9.8765432 x10-1, you should enter 9.9E-1.

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in