Determine the cell notation for the redox reaction given below. Sn(aq) + 2 H^+(a

Question

Determine the cell notation for the redox reaction given below. Sn(aq) + 2 H^+(aq) rightarrow Sn^2+ (aQ) + H_2(g) a) H^+(aq) | H_2(g) | Pt || Sn(s) | Sn^2+(aq) b) H_2(g) | H^+(aq) | Pt || Sn^2+ (aq) |Sn(s) c) Sn^2+ (aq) | Sn(s) || H_2(g) | H^+(aq) | Pt d) Sn(s) | Sn^2+(aq) || H^+(aq) | H_2(g) | Pt e) Sn(s) | H_2(g) ||Sn^2+ (aq) | H^+ (aq) | Pt Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25 degree C. The acid is followed by its K_a value. a HCIO_2, 1.1 times 10^-2 b) HCN, 4.9 times 10^-10 c) HNO_2, 4.6 times 10^-4 d) HF, 3.5 times 10^-4 e) HCHO_2, 1.8 times 10^-4 Which one of the following combinations can produce a buffer solution? a) HNO_2 (weak acid) and Ba (NO_2)_2 b) HCN (weak acid) and KBr c) HI (strong acid) and Bal_2 d) NH_3 (weak base) and NaNO_2 e) HCIO_4 (strong acid) and NaCIO_4 What is the concentration of Ba(OH)_2 in a solution with a pH = 9.0? Ba(OH)_2 (aq) rightarrow Ba^2+ (aq) + 2OH^1- (aq) a) 1.0 times 10^-5 b) 1.0 times 10^-9 c) 5.0 times 10^-5 d) 1.0 times 10^-6 e) 5.0 times 10^-6

Explanation / Answer

Q10

cell notation:

oxidation // reduction

then

Sn(s) --> Sn2+(aq) is getting oxidized

2H+(aq) --> H2(g) is getting reduced

so

ignore a and b, since it includes H in the oxidation

ignore c, since Sn2+ is not oxidized

then only d and e are possible answers

ignore e, since H2(g) is in the oxidation half cell

therefore

only D

Sn(s) / Sn2+(aq) // H+(aq) /H2(g) / Pt

is the answer

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