. A co-worker in a biochemistry laboratory suggests to you that a buffer solutio
ID: 1053618 • Letter: #
Question
. A co-worker in a biochemistry laboratory suggests to you that a buffer solution with a pH of 8.00 may be prepared by mixing 72.00 mL of 0.200 MNH3 solution with 128.0 mL of 0.200 M NH Cl solution. a. Is your co-worker correct? What is the pH of the resultant solution? f the resultant buffer solution were diluted to a volume of 1.00 L, would its pH change? 0 1 SOLUTION Anonymous 5 minutes later pOH-pKb+ log [NH4 INH3] moles of NH4 0.2*128/1000-0.0256 and moles of NH3-0.2 72/1000-0.0144 pKb of NH3-9.25 pOH-9.25+log (0.0250.0144) (since moles ratio is equal to concentration ratio)-9.5 b) no both NH3 and NH4CI are diluted to same extent and the ratio of NH4+/NH3 remains constant. So pH will not change. -0!Was this answer helpful?Explanation / Answer
for the NH3 (base) and NH4Cl (salt) , we have to use henderson equation in the pOH form using Kb and then we can calculate pH by pOH + pH = 14.
but
if you want to use henderson equation in the form of ka and pH then
you have to use NH3 as salt and NH4Cl as the acid.
and using the equation
Kw = ka * kb , we have to calculate ka as
Ka = Kw / kb
and then we can use the henderson equation in the form
pH = pka + log [NH3]/[NH4Cl]
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