1. You have a solution of 0.430 M sulfuric acid solution and a solution of KOH w

Question

1. You have a solution of 0.430 M sulfuric acid solution and a solution of KOH whose concentration you want to determine. At the end of the reaction, you find that you have used 12.5ml H2SO4 and 25.0ml KOH. What's the concentration of KOH in M? (hint: write a balanced equation first)

2. I want to produce sulfur dioxide, SO2 using the reaction below. In the lab I have 42.5g of oxygen gas and 31.02g of hydrogen sulfide, H2S.

A. How much SO2 is it possible to produce? 2 H2S + 3 02(g) --> 2 SO2(g) + 2 H2O(l)

B. After running the reaction, I determine that 42.6g of SO2 is produced. What is my percent yield (to 2 sig. figs.)?

3. You mix 25.0ml of 6.0m LiOH with 75.0ml of MgSO4. Magnesium hydroxide precipitates from the solution.

A. Write a balanced equation for the reaction.

B. What concentration of MgSO4 is required to react with all the LiOH?

C. What mass of magnesium hydroxide is produced?

D. What is the final concentration of Li2SO4(aq)?

Explanation / Answer

mmol of acid = MV = 0.43*12.5 = 5.375 mmol of acid

ratio is 2:1 with respect to base so

5.375*2 = 10.75 mmol of base needed

[KOH] = mmol/mL = 10.75/25 = 0.43 M

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