Problem: A 50.0-mL sample of 0.00200 M AgNO3 is added to 50.0 mL of 0.0100 M NaIO 3. What is the equilibrium concentration of Ag+ in solution? (Ksp for AgIO3 is 3.0 X 10-8.)

FREE Expert Solution

(1)Calculate moles of Ag+ and IO3-

mol Ag+=50 mL (1x10-3 L1 mL)(0.002 mol AgNO31 L)(1 mol Ag+1 mol AgNO3)

mol Ag+ = 0.0001 mol

mol IO3-=50 mL (1x10-3 L1 mL)(0.01 mol NaIO31 L)(1 mol IO3-1 mol NaIO3)

mol IO3-= 0.0005 mol 


(2) Construct an ICF chart

At this point, no Ag+ left

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Problem Details

A 50.0-mL sample of 0.00200 M AgNO3 is added to 50.0 mL of 0.0100 M NaIO 3. What is the equilibrium concentration of Ag+ in solution? (Ksp for AgIO3 is 3.0 X 10-8.)

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