Chemistry - stoichiometry, solutions

[excel000]

Homework Statement

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.

Homework Equations

AgNO₃ + KBrO₃ -> AgBrO₃(s) + KNO₃

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

 

[Borek]

You are right to ignore water, it doesn't take part in the reaction. That's assuming AgBrO₃ is completely insoluble.

https://www.physicsforums.com/showthread.php?t=257528