lilpeepxliltracy
08.11.2019 •
Chemistry
If you had a 0.800 l solution containing 0.0240 m of fe3+(aq), and you wished to add enough 1.38 m naoh(aq) to precipitate all of the metal, what is the minimum amount of the naoh(aq) solution you would need to add? assume that the naoh(aq) solution is the only source of oh−(aq) for the precipitation.
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Ответ:
0.041 L = 41.3 mL
Explanation:
This problem we will solve by considering the stoichiometry of the reaction and the definition of molarity.
Number of moles in .800 L solution:
0.800 L x 0.0240 M = 0.800 L x .0240 mol/L = 0.0192 mol Fe³⁺
to form the precipitate Fe(OH)₃ we will need 3 times .0192
mol NaOH required = 0.057
given the concentration of 1.38 mol M NaOH we can calculate how many milliliters of NaOH will contain 0.057 mol:
1.L/1.38 mol NaOH x 0.057 mol NaOH = 0.041 L
0.041 L x 1000 mL/1L = 41.3 mL
Ответ: