Okay, this is a two-part question and the unit is acids and bases.
Ka for NH4 is 5.6 x 10^ -10
Kb for NH3 is 1.8 x 10^ -5
1. Determine the pH of a solution prepared by adding 0.0500 mole of solid ammonium chloride to 100mL of a 0.150 molar solution of ammonia.
2. If 0.0800 mole of solid magnesium chloride, MgCl2 is dissolved in the solution prepared in part (1) and the resulting solution is well-stirred, will a precipitate of Mg(OH)2 form? Show calculation to support your answer. (Assume the volume of the solution is unchanged. The solubility product constant for Mg(OH)2 is 1.5 x 10^ -11)
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1.
Use the Henderson-Hasslebalch equation to calcualte the pH of the solution.
2. From question 1, calculate (OH^-), then use that and (Mg^2+) to determine if (Mg^2+)(OH^-)^2 exceeds Ksp.
Post work if you get stuck.
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