What is the molarity of an HBr solution if 11.0 mL of a 0.48 M LiOH solution are needed to neutralize 30.0 mL of the sample?
Part: 0 / 2
Part 1 of 2
Write the balanced chemical equation for this acid-base reaction. Include the states of matter.
Determine the molarity of the HBr solution. Be sure your answer has the correct number of significant figures.
M HBr
HBr(aq) + LiOH(aq) -> LiBr(aq) + H2O(l)
To find the molarity of the HBr solution, we can use the equation for dilutions:
M1V1 = M2V2
(0.48 M)(11.0 mL) = M2(30.0 mL)
M2 = (0.48 M * 11.0 mL) / 30.0 mL
M2 = 0.176 M
Therefore, the molarity of the HBr solution is 0.176 M.