The blank solution used to calibrate the spectrophotometer is 10.0 ml of 0.2 m fe(no3)3 diluted to 25.0 ml with 0.1 m hno3. why is this solution preferred to simply using de-ionized water for the calibration?

Suppose that some of the compound spilled out of the crucible after it was heated. would that cause the percent by mass of water in the compound determined by the experiment to be too low, too high, or unchanged? briefly explain your answer.