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100.0mL of 0.400 mol/L CoCl2 (aqueous) is mixed with 100.0mL of 1.600 mol/L NaOH. Determine the moles of precipitate which form, and the molarity of each ion (including spectator ions) after the precipitation process is complete. The ksp=(2.5x10^-16) of the precipitate.Now add 300.0mL of 0.500 mol/L ethylenediammine (addreviated "en") to the above solution. How many moles, if any, of precipitate remain?kf,[Co(en)3]^2+=8.7x10^13
Gold has a face-centered cubic arrangement with a unit cell edge length of 4.08 Angstrom. How many moles of gold fit in a sheet with a length of 51.6 nm, a width of 24.3 nm, and a thickness of 16.7 nm?
For each titration I need to calculate the moles of base needed to neutralize the acid sample. How do I go about doing this?
The normal boiling point for acetone is 56.5 C. At an elevation of 5300 ft the atmospheric pressure is 630 torr. What would be the boiling point of acetone Hvap = 32.0 kJ/mol at this elevation
5 gram of solid calcium sulfate is added to 1 leter of pure water. what is the soncentration of dissolved sulfate once equilibrim is achieved
Explain which of the following aqueous solutions has the strongest ion-dipole attractions:0.3 M Na3PO4, 0.1 M NiF2,0.2 M Rb2CO3, 0.01 M Sr(OH)2 , 0.03 M ScBr3.
Phenol is a weak organic acid with Ka=1.0x10^-10. How many grams of phenol do you need to add to 500. mL of water to make a pH=5.75 solution
calculate the molar concentration of the final solution. assume volume remains constant
What carbonyl compound would the following condensation product? Which of the following could result from a self-aldol condensation followed by dehydration?
Nitrobenzene, C6H5NO2, an important raw material for the dye industry, is prepared from benzene, C6H6, and nitric acid. When 22.4g of benzene and an excess of HNO3
Copper and zinc (elements 29 and 30, respectively) appear next to each other on the periodic table. A 5.50 g sample of zinc has a volume of 0.770 mL, while a 5.50 g sample of copper has a volume of 0.616 mL. Why?
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed at the indicated values. Ksp = 7.9 x 10-16. (a) pH 7.2
An ammonia/ammonium buffer solution contains 0.49 M NH3 and 0.62 M NH4+. The Kb value of ammonia is 1.8x10^5. Calculate the pH of this buffer.
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