A chemist needs to determine the concentration of a solution of nitric acid, HNO

Question

A chemist needs to determine the concentration of a solution of nitric acid, HNO_3. She puts 865 mL of the acid in a flask along with a few drops of indicator. She then slowly adds 0.800 M Ba(OH)_2 to the flask until the solution turns pink, indicating the equivalence point of the titration. She notes that 165 mL of Ba(OH)_2 was needed to reach the equivalence point.

How many moles of HNO_3 are present if 0.132 mol of Ba(OH)_2 was needed to neutralize the acid solution?
Express your answer with the appropriate units.

Explanation / Answer

2 HNO3 + Ba(OH)2 ====> Ba(NO3)2 + 2 H2O So at equivalence point , number of moles of HNO3 = number of moles Ba(OH)2 The molar ratio is 2 HNO3: 1 Ba(OH)2 0.132 mol Ba(OH)2 *(2 mol HNO3/1 mol Ba(OH)2 0.66 mol HNO3

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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