Question

11.2 g of tin is deposited on passing 1 ampere of current for 5 hours in its aqueous salt solution. Tin is present in the form of:

a. Sn2+
b. Sn4+
c. SnO2
d. SnO

Answer 1

Tin is deposited in its Sn2+ form when current is passed through its aqueous salt solution for electroplating.

Step-by-step explanation:

When 11.2 grams of tin is deposited by passing 1 ampere of current for 5 hours in its aqueous salt solution, the form of tin present in the solution can be determined by the chemical reactions taking place during the electrolysis process. In such a reaction, the anode often consists of a metal strip of the substance to be deposited, and a Pt electrode serves as the cathode. Referring to exercise information related to galvanic cells, we find that tin is present as Sn2+ in the anode compartment, written as Sn(s) | Sn2+(aq). The sulfate ion does not participate in the overall reaction, thus not altering the charge state of tin in the solution.

Considering example 20.3.1, the balanced chemical equation for the spontaneous redox reaction is: 3 Sn(s) + 2NO3(aq) + 8 H+ (aq) → 3 Sn2+ (aq) + 2 NO(g) + 4 H2O(l). This indicates that tin is indeed in the Sn2+ oxidation state during plating.

Answer 2

Tin is deposited through an electrochemical process where Sn2+ ions are reduced at the cathode, indicating that tin is present in the form of Sn2+ in the aqueous salt solution.

Step-by-step explanation:

The electrochemical reaction involving tin during the electrolysis process involves Sn2+ ions being reduced and plated out on the cathode. In your scenario, 11.2 g of tin is deposited on passing 1 ampere of current for 5 hours from its aqueous salt solution. This reaction suggests that Sn2+ ions are present in the solution because for tin to be plated out, it would need to gain two electrons (reduction), which corresponds to the Sn2+ oxidation state.

Based on the provided examples and exercises, the spontaneous redox reaction in the galvanic cell description and the electroplating process, we see that tin is involved in the reaction with a 2+ charge in several occasions, further confirming that in your case, tin is present in the form of Sn2+ in its aqueous salt solution.