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AP Chemistry Problem

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1: Consider mixing solutions of silver nitrate and calcium chloride.

a. write a net ionic equation for the formation of the precipitate.

b. If 200.0 mL of .300 M silver nitrate are mixed with 350.0 ml of .500 M calcium chloride, how many grams of precipitate are formed? How many moles of each ions are present after orecipitation?

c. What volume of .250 M calcium chloride would be required to precipitate silver chloride if it is mixed with 600.0 ml of 0.650 M Silver nitrate.

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AP Problem

Methylamine, CH3NH2, is a weak base that reacts according to the equation CH2NH2 + H2O <--> CH3NH3^1+ + OH^1-. The value of the ionization constant, Kb, is 5,25 x 10^-4. Methylamine forms salts such as methylammonium nitrate, (CH3NH3^1+)(NO3^1-). (b) Calculate the pH of a solution maded by adding 0.0100 mole of a solid methylammonium nitrate to 120.0 mL of a 0.225-molar solution of methylamine. Assume that no volume change occurs. (The answer i got was pH=11.15) (c) How many moles of EITHER NaOH OR HCl (state clearly which you choose) should be added to the solution in (b) to produce a solution that has a pH of 11.00? Assume that no volume change occurs.
(d) A volume of 100 mL of distilled water is added to the solution in (c). How is the pH of the solution affected? Explain.
This is from AP Chem Exam 1993 ques #1

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