Problem: Calculate the number of grams of ammonium chloride that must be added to 2.00 L of a 0.500 M ammonia solution to obtain a buffer of pH = 9.20. Assume the volume of the solution does not change as the solid is added. exttip{K_{ m b}}{K_b} for ammonia is 1.80 10-5.

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FREE Expert Solution

2.00 L ×0.500 mol NH31 L= 1.00 mol NH3


pH = pKa + log(conjugate baseweak acid)pH = -log Ka + log(conjugate baseweak acid)pH = -log (KwKb) + log(conjugate baseweak acid) 9.20 = -log(1.0×10-141.80×10-5) + log(conjugate baseweak acid)log(conjugate baseweak acid) = 9.20 - 9.2553log(conjugate baseweak acid) = -0.0553(conjugate baseweak acid) = 10-0.0553(conjugate baseweak acid) =0.8805


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Problem Details

Calculate the number of grams of ammonium chloride that must be added to 2.00 L of a 0.500 M ammonia solution to obtain a buffer of pH = 9.20. Assume the volume of the solution does not change as the solid is added. for ammonia is 1.80 10-5.

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Based on our data, we think this problem is relevant for Professor Vickrey's class at UNL.