for the titration of 10.0 ml of .15 M HNO2 aqueous solution (Ka=7.2x10^-4) using 2.5 M...

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Chemistry

for the titration of 10.0 ml of .15 M HNO2 aqueous solution(Ka=7.2x10^-4) using 2.5 M NaOH aqueous solution, consider thefollowing points of the titration: A: Initial pH of .15 M HNO2aqueous solution B: .1 mL added base C: 1/2 equivalence point D:Equivalence point E Excess base (assume added 100.0 mL of base)
Set up the init mol, final mol, total volume, and ICEtable for points B and D only:
Point B:
Titration equation:
init mol:
(assume reaction goes to completion)
final mol:
total volume:
flip reaction equation:
I:
C:
E:
Point D:
Titration equation:
init mol:
(assume reaction goes to completion)
final mol:
total volume:
flip reaction equation:
I:
C:
E:

Answer & Explanation Solved by verified expert

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PointB Titration equation HNO2 NaOHaq NaNO2aq H2O Initial moles of HNO2 MxVL 015 molL x 0010 L 00015 mol Initial moles of NaOH during mixing MxVL 25 molL x 000010 L 000025 mol 000025 mol of NaOH will react with 000025 mol of HNO2 to form See Answer

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