1. The problem statement, all variables and given/known data 0.790 g of silver nitrate and 0.473 g of potassium bromate are added to 379 mL water. Solid silver bromate is formed, dried, and weighed. What is the mas in g of the precipitated silver bromate? 2. Relevant equations AgNO3 + KBrO3 --> AgBrO3 + KNO3 AgNO3 = 169.87 g KBrO3 = 197.00 g AgBrO3 = 235.776 g KNO3 = 101.10 g 3. The attempt at a solution 169.87g AgNO3 => 235.78g AgBrO3 0.790g AgNO3 => (235.78g AgBrO3/ 169.87g AgNO3) * 0.790g AgNO3= 1.0965 g AgBrO3 167.005 KBrO3 => 235.78g AgBrO3 0.473g KBrO3=> (235.78g AgBrO3/167.005 KBrO3)*0.473g KBrO3 = 0.668 g AgBrO3 Limiting Reactant is KBrO3, thus the answer would be 0.668 g AgBrO3, also how many significant figures should we use?