If you have 0.20 mol of silver permanganate (AgMNO4), which has a solubility of about 16.7...
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If you have 0.20 mol of silver permanganate (AgMNO4), which has a solubility of about 16.7 g/L, what is the minimum amount of water you’ll need to get it all into solution? At what temperature? Report your answer to the nearest whole mL.
Homework Answers
Given solubility 16.7 g/L is at 25oC hence the calculated amount of water is also at 25oC.
The molar mass of AgMnO4 = 226.8 g/mol
Mass of 0.20 mole of AgMnO4 = 0.20*226.8 = 45.36 g
Thus the minimum amount required to make a solution = 45.36g / 16.7 g/L = 2.716 L = 2716 mL
Thus the minimum amount of water needed is = 2716 mL.
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