Answer :
Final answer:
The molarity of the LiBr solution is around 1.5 M. The concentration of the H2SO4 solution can be found through titration with LiOH, considering the stoichiometry in the balanced equation, and using the concept of molarity. Exact concentration will depend on the final calculations.
Explanation:
The first part of your question asks for the molarity of a LiBr solution. This can be calculated by the formula: Molarity = moles of solute / liters of solution. Firstly, convert 97.7 g LiBr into moles. LiBr has a molar mass of about 87 g/mol, so 97.7 g is approximately 1.12 moles. Secondly, convert 750.0 mL into liters, which is 0.75 liters. Using the formula yields a molarity of approximately 1.5 M.
For the second part, the titration of H2SO4 with LiOH is considered. From the balanced chemical equation H2SO4 + 2LiOH -> Li2SO4 + 2H2O, it is observed that the mole ratio of H2SO4 to LiOH is 1:2. Thus, the moles of H2SO4 is half the moles of LiOH. Given that the molarity of LiOH is 0.12 M and the volume used in the titration is 83.6 mL (or 0.0836 liters), the moles of LiOH can be calculated by multiplying the molarity and volume. Dividing this result by 2 will give the moles of H2SO4. Then, the concentration of H2SO4 (in M) can be found by dividing the moles of H2SO4 by the volume of H2SO4 solution (25.0 mL or 0.025 liters).
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