Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 46 g of NH4CI dissolved in 1.00 L of 0.920 M NH3? pH = 9.24 (b) How many moles of acid are required to change the pH of this solution by 0.07 pH units? i 5.5E-2 mol (c) Suppose 4.8 mL of 11.8 M HCI solution is added to 146 mL of the solution of Part (a). Calculate the new pH. pH = 9.08

Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 46 g of NH4CI dissolved in 1.00 L of 0.920 M NH3? pH = 9.24 (b) How many moles of acid are required to change the pH of this solution by 0.07 pH units? i 5.5E-2 mol (c) Suppose 4.8 mL of 11.8 M HCI solution is added to 146 mL of the solution of Part (a). Calculate the new pH. pH = 9.08

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Your answer is partially correct.
Ammonia is a convenient buffer system in the slightly basic range.
(a) What is the pH of a buffer solution containing 46 g of NH4CI dissolved in 1.00 L of 0.920 M NH3?
pH =
9.24
(b) How many moles of acid are required to change the pH of this solution by 0.07 pH units?
i
5.5E-2
mol
(c) Suppose 4.8 mL of 11.8 M HCI solution is added to 146 mL of the solution of Part (a). Calculate the new pH.
pH =
i
9.08
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