Question

What is the concentration of the barium hydroxide solution if 50.0 mL of a 0.425 M HNO3 solution is required to neutralize a 36.8 mL sample?

Answer 1

Answer:

• 0.289M

Explanation:

1. Balanced chemical equation

• Ba(OH)₂(aq)   +   2HNO₃(aq)   →   Ba(NO₃)₂(aq)   +   2H₂O(l)

2. Determine the number of moles of HNO₃ in the solution

• M = n/V(in liters)

• n = M × V = 0.425M × 0.050 liter = 0.02125‬ mol HNO₃

3. Use the mole ratio from the balanced chemical equation and the number of moles of HNO₃ to determine the number of moles of  Ba(OH)₂.

       $\dfrac{1molBa(OH)_2}{2molHNO_3}\times 0.02125molHNO_3=0.010625molBa(OH)_2$

4. Determine the molar concentration of the solution of Ba(OH)₂

• M = n/V(in liters)

• M = 0.010625mol/0.0368liter

• M = 0.289M ← answer