Decide whether or not each of the following metals dissolves in 1 M HCl. For the

Question

Decide whether or not each of the following metals dissolves in 1 M HCl. For these metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. Zn Express your answer as a chemical equation. Enter noreaction if there is no reaction. Identify all of the phases in your answer. Co Express your answer as a chemical equation. Enter noreaction if there is no reaction. Identify all of the phases in your answer. Na Express your answer as a chemical equation. Enter noreaction if there is no reaction. Identify all of the phases in your answer.

Explanation / Answer

The acid HCl at 1 M is pretty acidic.

It will have the next dissociation

HCl(aq) ---> H+(aq) + Cl-(aq)

so, there are H+ ions ready to react if reactivity/reduction potentials are achieved

We will need the reactivity series or reduction potentials in order to know which one will react aand which one will not

Recall that H+ may reduce as follows:

2 H+ + 2 e H2(g) E = 0 V

Anything lower than that of E = 0 V will react 2H+ ions to form H2 and the solid metal to ionic metals in solution, which is a reaction

For Zn (Zinc)

Zn2+ + 2 e --> Zn(s) E = 0.7618

The reduction potential of H+ is tronger, then, expect H2(g) formation

Overall reaction

Zn(s) + 2H+(aq) --> H2(g) + Zn2+(aq)

For Co (Cobalt)

Co2+ + 2 e ---> Co(s) E = 0.28

same case as Zn

Co(s) + 2H+(aq) --> H2(g) + Co2+(aq)

For Na (Sodium)

Na+ + e --> Na(s) E = 2.71

Same case, it is actually pretty likely to see Na reacting in acid

2Na(s) + 2H+(aq) --> H2(g) + 2Na+(aq)

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