Question

Suppose 0.522g of zinc iodide is dissolved in 100.mL of a 63.0mM aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it. Round your answer to 3 significant digits.

Answer 1

ZnIz + K₂CO3 (aa) - car) ZnCO3 +2KI (s) car) the Net Ionic equation 202 + core Zrcoat. ie concentration of Iodide resalt, (s) it doesn't react unchanged. since with zinc Initially, [zn 127 - 00522 g x lovo 329 g/mol room ZrI₂] = 1.64810 2M Iz Zst+2I 1-64810² 1.64010² 3-28 x 10² [I] = 3.28x1024) This is the final concentration. of Iodide ion.