The following results, in the table below, were obtained through a series of two

Question

The following results, in the table below, were obtained through a series of two experiments:

Write the total net ionic equations that describe all of the results noted from Experiment 1 and Experiment 2.

Explain the color change observed in Experiment 2 (replacement reactions).

Briefly discuss the relative activities of silver and chromium.

Experiment 1: Reactions w/ acids

Experiment 2: Replacement reactions

Cr2+ + Ag metal: no apparent reaction, silver metal did not change, solution stayed green.

Ag+ + Cr metal: silvery solid formed on piece of Cr metal: Solution went from colorless to bluish green.

Cr(s) Ag(s) HCl metal dissolves, bubbles, green solution no apparent reaction H2SO4 metal dissolves, bubbles, bluish purple solution no apparent reaction

Explanation / Answer

1 )

Cr (s) + 2HCl (aq) ---------------------> CrCl2 (aq) + H2 (g)

total net ionic equation: Cr(s) + 2H+   --------------------> Cr+2 (aq) + H2 (g)

Cr (s) + H2SO4 (aq) -------------------> CrSO4 (aq) + H2 (g)

total net ionic equation: Cr(s) + 2H+   --------------------> Cr+2 (aq) + H2 (g)

2)

Ag (s) + HCl ------------------> no reaction

Ag(s) + H2SO4 ---------------> no reaction

3)

Cr+2 + Ag --------------------->no reaction

Ag+ (aq) + Cr (s) ------------------------------> Cr+2 (aq)+ Ag (s)

note : Cr is nore active metal than Ag . so it can replace Ag+ from its solution

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