1. Describe the process by which Ag + ions are precipitated out of solution. 2.

Question

1.   Describe the process by which Ag+ ions are precipitated out of solution.

2.   A disproportion reaction occurs when NH3 solution reacts with Hg2Cl2. Write a balanced reaction equation for this event.

3.   Write half-reactions that show how H2O2 can act as either an oxidizing agent or a reducing agent, and describe where each of these situations occurred in your testing.

4.   When Mn2+ ions are separated from the mixture, they go through a series of oxidizing and reducing steps. Write the reaction equations that describe this process.

5.   Al3+ and Zn2+ ions are amphoteric. Describe how the amphoteric nature of these ions is shown in your testing.

Explanation / Answer

Q1.

Typically, we will preciptiate Ag+ ions with Cl- ions from HCl (acidic media)

Ag+ and Cl- ions will satureate therefore, they will form AgCl(s)

Q2.

Hg2Cl(s) + NH3 = Cl(NH2)Hg(s) + Hg0 + Cl-(aq) + NH4+

Q3.

H2O2(aq) + 2 H+ + 2 e 2 H2O +1.78

O2(g) + 2 H+ + 2 e H2O2(aq) +0.70

Q4.

Mn(NO3)2 + 2 (NH4)2S ---> MnS(s) + NH4NO3

2 Mn(NO3)2 + 5 NaBiO3 + 16 HNO3 ---> 2 HMnO4 + 5 Bi(NO3)3 + 5 NaNO3 + 7 H2O

Mn(NO3)2 + 2 NaOH ---> Mn(OH)2(s) + 2 NaNO3

Mn(OH)2 + H2O2 --->MnO(OH)2(s) + H2O

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.