Log in
Chemistry
1
answer
0
watching
1,418
views
18 Nov 2019

Below is a chemical reaction in which two solutions are combined: CdSO4 (aq) + K2S (aq) → CdS(s) + K2SO4 (aq)

a) What does the subscript (s) mean?

b) For cadmium sulfate, write a chemical equation similar to problem 2 showing that cadmium sulfate dissolves in water. Do the same for potassium sulfide. How many ions are present in this solution?

c) Some of these ions react with one another to produce cadmium sulfide. Look up the physical properties of cadmium sulfide. What would you expect to see when you mix cadmium sulfate and potassium sulfide?

d) What is the name for this type of reaction?

e) Potassium sulfate is shown as a soluble product. What ions are still present in solution after the reaction?

Watch
1
answer
0
watching
1,418
views

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

Hubert Koch
Hubert KochLv2
6 Mar 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

1. Write the net ionic equation for the precipitation of aluminum carbonate from aqueous solution:

2. Write the net ionic equation for the precipitation of aluminum sulfide from aqueous solution:

3. Consider the reaction when aqueous solutions of silver(I) nitrate and chromium(II) bromide are combined.

The net ionic equation for this reaction is:

4. Consider the reaction when aqueous solutions of aluminum chloride and iron(III) nitrate are combined.

The net ionic equation for this reaction is:

5. Consider the reaction when aqueous solutions of barium chloride and chromium(III) sulfate are combined.

The net ionic equation for this reaction is:

6. Consider the reaction when aqueous solutions of copper(II) sulfate and sodium nitrate are combined.

The net ionic equation for this reaction is:

7. Consider the reaction when aqueous solutions of silver(I) nitrate and potassium hydroxide are combined.

The net ionic equation for this reaction is:

8. Consider the reaction when aqueous solutions of potassium hydroxide and sodium nitrate are combined.

The net ionic equation for this reaction is:

9. Consider the reaction when aqueous solutions of iron(II) sulfate and ammonium phosphate are combined.

The net ionic equation for this reaction is:

10. Consider the reaction when aqueous solutions of potassium carbonate and sodium iodide are combined.

The net ionic equation for this reaction is:

11. Consider the reaction when aqueous solutions of aluminum sulfate and ammonium sulfide are combined.

The net ionic equation for this reaction is:

12. Consider the reaction when aqueous solutions of sodium sulfide and potassium nitrate are combined.

The net ionic equation for this reaction is:

13. Consider the reaction when aqueous solutions of silver(I) nitrate and potassium hydroxide are combined.

The net ionic equation for this reaction is:

14. Consider the reaction when aqueous solutions of ammonium sulfide and silver(I) sulfate are combined.

The net ionic equation for this reaction is:

15. In the laboratory you are given the task of separating Ag+ and Ba2+ ions in aqueous solution.

For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No"

Y or N Reagent Formula of Precipitate if YES
1. KBr
2. Na2CO3
3. K2SO4

16. In the laboratory you are given the task of separating Ba2+ and Co2+ ions in aqueous solution.

For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No"

Y or N Reagent Formula of Precipitate if YES
1. K2S
2. HBr
3. KOH

Can I get all of the question answered in a way that I know under which sub question the answer goes please.

Can I get all of the questions answered in a way that I know how it fits in the question. Some parts are explanations. Thank you.

Q. When a pink aqueous solution of potassium permanganate, faintly acidified with dilute sulfuric acid was treated with 10% aq. hydrogen peroxide, the reaction took place with the evolution of gas bubbles, and the pink solution was turned colorless. Further chemical analysis revealed that the evolved gas was oxygen, and the resulting solution contains potassium sulfate and manganese (II) sulfate; water was also formed during the same reaction. Please answer the followings:

1) Write down the balanced chemical equation for this reaction.

2) Define the type/types of the reaction; assign the oxidation number of Manganese in potassium permanganate and manganese (II) sulfate. Also, offer an explanation for the color change.

3) Write down the ions present in the solution before & after the reaction. If 100 mL 0.5 M potassium permanganate was mixed with 50 mL 2 M sulfuric acid, what will be the final pH (>7 or <7) of the solution?

4) After the completion of reaction, when evolution of gas-bubbles ceased, what will happen if an aqueous solution of sodium carbonate was added to the reaction mixture? Please write down the net ionic equation.

5) If initially 5.65 g of potassium permanganate was taken for the reaction, calculate the total mass of manganese (II) sulfate present in the solution after the completion of the reaction. What is the Manganese ion concentration of the solution (assume that the total volume of the final reaction mixture is 500 mL)?

Useful hints: hydrogen peroxide is a strong oxidizing agent and considered to be a molecular compound.

1. (10)What ions and/or molecules are present in relatively largeproportions in a solution of a weak acid HCN (aq)?

H+
CN-
HCN
HC+
N+
CN
CN-
N3-

2. What ions and/or molecules are present in relatively largeproportions in a solution of a strong base KOH (aq)?

KOH
K2+
OH-
OH2-
KO+
OH+
K
OH
K+
None of these choices is correct

3. What ions and/or molecules are present in relatively largeproportions in a solution of a strong acid H2SO4 (aq)? (NOTE:Remember that only the first ionization is strong.)

HSO4-
H2SO4
SO42-
HS-
O42-
O22-
H2S2-
H+
S
O4

4. What ions and/or molecules are present in relatively largeproportions in a solution of a soluble ionic compound K2CO3(aq)?

K2CO3
K2+
K22+
K+
O32-
CO3-
C
CO32-
K2
CO3

5. Which of the following equations represents the proper net ionicequation for the precipitation of an insoluble phosphate compoundfrom K3PO4 (aq) and Al(NO3)3(aq)?

K3PO4 (aq) + Al(NO3)3(aq) ----> 3 KNO3 (aq) + AlPO4 (s)
K3PO4 (aq) + 3 NO3- (aq) ----> 3 KNO3 (s) + PO43- (aq)
NO3- (aq) + K+ (aq) ----> KNO3 (s)
PO43- (aq) + Al(NO3)3(aq) ----> AlPO4 (s) + 3 NO3 (aq)
2 PO43- (aq) + 3 Al2+ (aq) ----> Al3(PO4)2 (s)
Al3+ (aq) + PO43- (aq) ----> AlPO4 (s)
K3+ (aq) + (NO3)3- (aq) ----> K3(NO3)3(s)
K3PO4 (aq) + Al(NO3)3(aq) ----> K3(NO3)3 (aq) + AlPO4 (s)
Al+ (aq) + PO4- (aq) ----> AlPO4 (s)

6. Which of the following equations represents the proper net ionicequation for the complete neutralization reaction between the weakacid H2S (aq) and the strong base KOH (aq) ?

H2S (aq) + 2 KOH (aq) ----> 2 H2O (l) + K2S (aq)
S2- (aq) + 2 K+ (aq) ----> K2S (aq)
H2+ (aq) + 2 OH- (aq) ----> 2 H2O (l)
H+ (aq) + OH- (aq) ----> H2O (l)
H+ (aq) + KOH (aq) ----> H2O (l) + K+ (aq)
H2S (aq) + 2 OH- (aq) ----> 2 H2O (l) + S2- (aq)
H+ (aq) + K+ (aq) ----> HK (aq)
S2- (aq) + OH- (aq) ----> SOH (aq)

7. What are the spectator ions in the solution after completelyprecipitating an insoluble sulfide compound when mixing Ag2SO4 (aq)and K2S (aq)?

Ag+ , SO42- , K+ , and S2-
S2- and Ag+
SO42- and S2-
S2- and K+
K+ and Ag+
SO42- and Ag+
Ag+
K+ and SO42-

8. What are the spectator ions in the solution after the completeneutralization reaction occurs when mixing the weak acid H2S (aq)and the strong base KOH (aq)?

H+ , S2- , K+ , and OH-
OH- and K+
H+ and OH-
OH- and S2-
K+ and S2-
K+ and H+
S2- and H+
K+
S2-
SO42-
K+

Weekly leaderboard

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