When 30.0 mL of an unknown acid was titrated with 0.323 M NaOH
When 30.0 mL of an unknown acid was titrated with 0.323 M NaOH, 33.1 mL of the base was required to reach the equivalence point. What was the concentration of the acid?
Please include units in your answer
Homework Answers
unknown acid is taken as monoprotic acid
HA is monoprotic acid
HA + NaOH -----------------> NaA + H2O
1 mole 1 mole
HA NaOH
M1 = M2 = 0.323M
V1 = 30ml V2 = 33.1ml
n1 =1 n2 = 1
M1V1/n1 = M2V2/n2
M1 = M2V2n1/V1n2
= 0.323*33.1*1/30*1 = 0.3564M
molarity of unknown acid = 0.3564M
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