Question

7. Suppose 2.26 g of zinc chloride is dissolved in 150 ml. of 67.0 mM aqueous solution of ammonium sulfate. Calculate the final molarity of zinc cation in the solution. You can assume the volume does not change when the zinc chloride is dissolved in it. Round your answer to 3 significant digits.

Answer 1

first write the balanced equation and then find the no of moles and then calculate the concentration is as follows

The bakanced equation is as follows Zindle ceny + (NH4), S .-> znsoy + ante locals No. of moles = mass moler mass for Inila = 2.269 1 = 0.01658 mol (26.2869ime moes et (NH4)2504 = 0.150lX0.0671 ) 0.0100smal limiting React aut s (NH4)2S0y. . Excess Reactant es znala = IMG(NH4), LMHz) 0.0100g met > 0.0100rmo :Excess rosoles et anche = 0.01658 -0.01005 7) 0.006532... fend concentration of zght 0.0065 sind . "0.150L 20.04355M Auswear Auguera (0,0436M = 3-spruifolt fs seves