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A 100.0 ml dilute solution of Ag⁺ Is electrolysed for 15 mins. With a current of 1.25mA and the silver is removed completely. What was the initial (Ag⁺)

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Last updated date: 15th Jul 2024
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Answer
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Hint: Electrolysis is a chemistry and manufacturing process that uses direct electric current (DC) to drive a chemical reaction that would otherwise be non-spontaneous. Electrolysis is important in the commercial separation of elements from naturally occurring sources like ores using an electrolytic cell. The decomposition potential is the voltage needed for electrolysis to occur. The word "lysis" means "to split or split," so electrolysis may be described as "electrical breakdown" or "electrical breakdown."

Complete answer:
Electrolysis is the process of moving a direct electric current into an electrolyte, which results in chemical reactions at the electrodes and substrate decomposition. Electrolysis requires an electrolyte, electrodes, and an external power source, among other things.
Q = It
Where Q is the electric charge in coulombs (C), which is the unit of electric charge, t = time (s), I = current flow in amperes (A).
Given Q = 1.25 mA = 1.25 x 10⁻³ A
t = 15 x 60 s
\[{\text{Q}} = 1.25 \times {10^{ - 3}} \times 15 \times 60 = 1.125{\text{C}}\]
Ag is electrolysed as
\[{\text{A}}{{\text{g}}^ + }({\text{aq}}) + {{\text{e}}^ - } \to {\text{Ag}}({\text{s}})\]
1 mole of electrons =96500 C
As a result, electron moles passed through the circuit, \[ = \dfrac{{1.125}}{{96500}} = 1.16 \times {10^{ - 5}}\]
It takes 1 mole of electrons to form Ag
Hence, moles of Ag = \[\dfrac{{1.16 \times {{10}^{ - 5}}}}{1} = 1.16 \times {10^{ - 5}}\]
Moles of Ag = Moles of Ag⁺
So,
\[\left[ {{\text{A}}{{\text{g}}^ + }} \right] = \dfrac{{1.16 \times {{10}^{ - 5}} \times 1000}}{{100}} = 1.16 \times {10^{ - 4}}{\text{M}}\]

Note:
Silver is a chemical element with atomic number 47 and the symbol Ag (from the Latin argentum, which is derived from the Proto-Indo-European term "shiny" or "white"). It is a lustrous, soft, white transition metal with the highest electrical conductivity, thermal conductivity, and reflectivity of any metal.