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Milk of Magnesia is actually a suspension (that's why instructions often mention shaking before use) of solid Mg(OH)2. 1.00 liter of solution of 0.055 moles of Mg2+ is held at a pH of 7.00. Would a precipitate form? If so, what fraction of the original 0.055 molar Mg2+ would precipitate at that pH? Ksp = 5.61 x10-12
Mg(OH)2 (s) → Mg2+ (aq) + 2 OH- (aq)
(B) At pH = 10.00, would there be precipitation? If so, what fraction of the original 0.055 M Mg2+ precipitate?
Perform the calculatons for the extraciton of 100 mg of P in 300mL of water with three 100-mL portions of ether. assume the partition coefficient is 3.5
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The formula for caluculating a dilution of a solution is M1V1=M2V2, use this equation to calculate the volume of a 2.0 M solution of sodium carbonate required to make 100mL of a 0.25 M solution. A1) calculate the mass of calium chloride dihydrate
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The composition of the flue gas, which is at 720°C is 13% CO2, 14.3%H2O, 67.6% N2 and 5.1% O2. What was the heat transfer to or from the combustion process?
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Based on your answer to (1), would you be more or less confident about your density measurement if you used the smaller sample volume, rather than the normal 8 mL sample volume? Briefly explain.
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