Question
In: Chemistry
A buffer solution contains 0.227 M ammonium bromide and 0.427 M ammonia. If 0.0488 moles of...
A buffer solution contains 0.227 M
ammonium bromide and
0.427 M ammonia.
If 0.0488 moles of nitric acid
are added to 225 mL of this buffer, what is the pH
of the resulting solution?
(Assume that the volume does not change upon adding nitric
acid.)
pH =
Solutions
Expert Solution
no of moles of NH4Br = molarity * volume in L
= 0.227*0.225 = 0.051 moles
no of moles of NH3 = molarity * volume in L
= 0.427*0.225 = 0.096 moles
0.0488 moles of HNO3 is added
no of moles of NH4Br after addition of HNO3 = 0.051+0.0488 = 0.0998 moles
no of moles of NH3 after addition of HNO3 = 0.096-0.0488 = 0.0472 moles
POH = Pkb + log[NH4Br]/[NH3]
= 4.75 + log0.0998/0.0472
= 4.75+0.325 = 5.075
PH = 14-POH
= 14-5.075 = 8.925 >>>>>answer
queen_honey_blossom answered 2 years agoRelated Solutions
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