When 20mL of 1.40M solution of calcium nitrate is mixed with 70.0mL of 0.234M po

Question

When 20mL of 1.40M solution of calcium nitrate is mixed with 70.0mL of 0.234M potassium iodate a precipitate (Ca(IO3)2) is formed. a) Write a balanced equation for this reaction b) Determine the limiting reagent. show work c) Calculate the concentration of both NO3- and IO3- before mixing and after mixing, keeping in mind the large excess of one reagent involved. Because of this, we can assume the precipitation reaction goes to completion.

Explanation / Answer

Ca(NO3)2 + 2KIO3----> 2KNO3 + Ca(IO3)2 mmoles Ca(NO3)2: 20*1.40 = 28mmol mmoles KIO3: 70*0.234 =16.38mmol You need 2 moles of KI per mole of Ca(NO3)2, so 16.38 mmoles KIO3 would react with 14 mmoles Ca(NO3)2, KIO3 is the limiting reagent. [NO3-] = 28mmol*2/90mL = 0.6222M [IO3-] = 16.38mmol*2/90mL = 0.364M

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