1. 24.49 mL of a solution of the acid H 2 C 2 O 4 is titrated, and 84.00 mL of 0

Question

1. 24.49 mL of a solution of the acid H2C2O4 is titrated, and 84.00 mL of 0.2500-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.

______ M

2. An aqueous solution of perchloric acid is standardized by titration with a 0.178 M solution of calcium hydroxide.

If 11.9 mL of base are required to neutralize 15.1 mL of the acid, what is the molarity of the perchloric acid solution?

______ M perchloric acid

3. A stock solution of Fe(NO3)2 is available to prepare solutions that are more dilute. Calculate the volume, in mL, of a 2.0-M solution of Fe(NO3)2 required to prepare exactly 100 mL of a 0.280-M solution of Fe(NO3)2.

______ mL

Explanation / Answer

1. At the equivalence point we can say that

MilliEquivalent of acid= MilliEquivalent of base

Also we know that MilliEquivalent = molarity*volume in ml*n-factor

Let molarity of acid be M so MilliEquivalent of acid:-24,49*M*2

MilliEquivalent of base:-0.25*84*1=21

So M=0.428 molar

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.