Just as pH is the negative logarithm of [H3O+],pKa is the negative logarithm of Ka,- log KaThe Henderson-Hasselbalch equation is used tocalculate the pH of buffer solutions:How many grams of dry NH4C1 need to be added to2.00 L of a 0.600 mol L-' solution of ammonia, NH3,to prepare a buffer solution that has a pH of 8.80? Khfor ammonia is 1.8 × 10–5.pKabase]pH = pKa +log acidExpress your answer to two significant figures andinclude the appropriate units.Notice that the pH of a buffer has a value close tothe pKa of the acid, differing only by the logarithmof the concentration ratio [base]/[acid].• View Available Hint(s)?X•10nValuemass ofNHẠCI =Units

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How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L¬' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kp for ammonia is 1.8 × 10¬5. Express your answer to two significant figures and include the appropriate units.

How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L¬' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kp for ammonia is 1.8 × 10¬5. Express your answer to two significant figures and include the appropriate units.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 31QAP: Enough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a)...

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Question

100%

Just as pH is the negative logarithm of [H3O+],
pKa is the negative logarithm of Ka,
- log Ka
The Henderson-Hasselbalch equation is used to
calculate the pH of buffer solutions:
How many grams of dry NH4C1 need to be added to
2.00 L of a 0.600 mol L-' solution of ammonia, NH3,
to prepare a buffer solution that has a pH of 8.80? Kh
for ammonia is 1.8 × 10–5.
pKa
base]
pH = pKa +log acid
Express your answer to two significant figures and
include the appropriate units.
Notice that the pH of a buffer has a value close to
the pKa of the acid, differing only by the logarithm
of the concentration ratio [base]/[acid].
• View Available Hint(s)
?
X•10n
Value
mass of
NHẠCI =
Units

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