Reference no: EM132582634

Copper(ii) ions are an environmental hazard and as such, must be removed from waste products before any waste is added to the ecosystem. You have been given the task of removing Copper(ii) ions present as Copper(ii) iodide in the waste water of an industrial facility. You have decided to use sodium carbonate to help in this regard. With respect to this, answer the following questions.

a)?Write the complete balanced equation for the addition of Copper(ii) iodide to sodium carbonate.

b)?Which of the compounds in part (a) are soluble and which are insoluble? Write the Net Ionic Equation for the reaction in (a).

c)?Why can the reaction in part (a) be used to remove Copper(ii) ions from the waste water. Suggest a method that can be used to ensure that the process is as effective as possible at removing the Copper(ii)ions.

d)?Use what you've learned in this unit to explain why Copper(ii) carbonate is less of an environmental concern than Copper(ii) iodide?

e)?What assumptions are being made regarding the toxicity of sodium iodide and sodium carbonaterelative to either Copper(ii) iodide or Copper(ii)carbonate?

f)?The concentration Copper(ii) iodide in waste water is 25 ppm. How many grams of Copper(ii) iodide are in a 1000 L sample of waste water?

g) ?What is the molar concentration of the Copper(ii)Iodide in the waste water in question f)?

h)?How many Kg of sodium carbonate is required to remove the soluble Copper(ii) ions from 10 000 L of waste water (in question f.)?

i)?Suggest some factors that a company would need to consider in adopting any method of cleaning it's waste water?