Suppose a current of is passed through an electroplating cell with an aqueous solution of agno3 in the cathode compartment for seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.

The given question is incomplete. The complete question is:

Suppose a current of 0.920 A is passed through an electroplating cell with an aqueous solution of agno3 in the cathode compartment for 47.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.

  0.0484 g

Explanation:

where Q= quantity of electricity in coloumbs

I = current in amperes = 0.920 A

t= time in seconds = 47.0 sec

96500 Coloumb of electricity electrolyzes 1 mole of Ag

43.24 C of electricity deposits = of Ag

Thus the mass of pure silver deposited on a metal object made into the cathode of the cell is 0.0484 g

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.

the answer is na (sodium)