To determine the amount of copper ions present in the solution after electrolysis, we can use Faraday's laws of electrolysis. First, we need to calculate the total charge Q passed through the solution during electrolysis. Q = current I time t Q = 0.3 A 10 minutes 60 seconds/minute = 0.3 A 600 s = 180 CoulombsNext, we need to find the number of moles of electrons n transferred during electrolysis. We can use Faraday's constant F , which is approximately 96485 Coulombs/mol of electrons.n = Q / Fn = 180 C / 96485 C/mol 0.001864 mol of electronsNow, we need to consider the stoichiometry of the reaction. The balanced half-reaction for the reduction of Cu ions to Cu metal is:Cu + 2e CuThis means that for every 2 moles of electrons, 1 mole of Cu ions is reduced to Cu metal. So, we can find the moles of Cu ions reduced:moles of Cu = 0.001864 mol of electrons 1 mol Cu / 2 mol of electrons 0.000932 mol of CuFinally, we can find the new concentration of Cu ions in the solution after electrolysis. Assuming the volume of the solution remains constant, we can subtract the moles of Cu ions reduced from the initial moles of Cu ions in the solution:Initial moles of Cu = 0.01 M volume of the solution V New moles of Cu = 0.01 M V - 0.000932 molTo find the new concentration of Cu ions, divide the new moles of Cu by the volume of the solution V :New concentration of Cu = 0.01 M V - 0.000932 mol / VWithout knowing the volume of the solution, we cannot provide a specific numerical value for the new concentration of Cu ions. However, the expression above can be used to calculate the new concentration once the volume is known.