Consider the titration of 54.5 mL of 0.110 MHNO3 with 0.470 M NaOH.
How many millimoles of HNO3 are present at the start of the titration?
How many milliliters of NaOH are required to reach the equivalence point?
Express your answer using three significant figures.
What is the pH at the equivalence point?
HNO3 + NaOH ------------> NaNO3 + H2O
millimoles = molarity x volume in mL
initial millimoles of HNO3 = 0.110 x 54.5 = 5.99
NaOH and HNO3 reacts in 1 : 1 ratio
so
millimoles of NaOH = 5.99
5.99 = 0.470 x V
V = 12.7 mL
volume of NaOH required = 12.7 mL
as strong acid strong base titration
at equivalence point pH = 7.0
pH = 7.0
Consider the titration of 54.5 mL of 0.110 MHNO3 with 0.470 M NaOH. How many millimoles...
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