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Chemistry Question on Electrolysis

A 100.0 mL100.0\, mL dilute solution of Ag+Ag ^{+}is electrolysed for 15.015.0 minutes with a current of 1.25 mA1.25 \,mA and the silver is removed completely. What was the initial [Ag+]\left[ Ag ^{+}\right]?

A

2.32×10−12.32 \times 10^{-1}

B

2.32×10−42.32 \times 10^{-4}

C

2.32×10−32.32 \times 10^{-3}

D

1.16×10−51.16 \times 10^{-5}

Answer

1.16×10−51.16 \times 10^{-5}

Explanation

Solution

No. of moles of
Ag+=15×60+1.25×10−396,500×11A g^{+}=\frac{15 \times 60+1.25 \times 10^{-3}}{96,500} \times \frac{1}{1}
=0.0116×10−3=0.0116 \times 10^{-3}
∴[Ag+]=1.16×10−51001000\therefore\left[A g^{+}\right]=\frac{1.16 \times 10^{-5}}{\frac{100}{1000}}
=1.16×10−4=1.16 \times 10^{-4}