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Chemistry - stoichiometry, solutions

  1. Sep 20, 2008 #1
    1. The problem statement, all variables and given/known data

    0.800 g of silver nitrate and 0.473 g of potassium bromate are added to 238 mL water. Solid silver bromate is formed, dried, and weighed. What is the mass, in g, of the precipitated silver bromate? (Be careful to enter the correct number of significant figures. Do not enter units.) Assume silver bromate is completely insoluble.

    2. Relevant equations

    AgNO3 + KBrO3 -> AgBrO3(s) + KNO3

    3. The attempt at a solution

    0.800gAgNO3/169.66gmol-1AgNO3 = 4.7x10^-3mol

    0.473gKBrO3/166.998gmol-1KBrO3 = 2.83x10^-3mol <---- Limiting Reactant

    2.83x10^-3molAgBrO3 x 235.77gmol-1
    = 0.667g AgBrO3

    that was my attempt, but i completely ignored the water part since I don't really know what that is for, so i'm pretty sure i'm wrong. any help on this would be greatly appreciated
  2. jcsd
  3. Sep 20, 2008 #2


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