Ask Question
25 May, 10:55

Find the volume of 0.240 M sulfuric acid necessary to react completely with 72.8 g sodium hydroxide. Express your answer with the appropriate units.

+3
Answers (1)
  1. 25 May, 11:25
    0
    The volume neccesary to complete reaction is 3.79L

    Explanation:

    First step: Think the equation

    H2SO4 + 2NaOH → Na2SO4 + 2H2O

    Afterwards, ballance it.

    Relation in reactants is 1:2, so 2 mol of NaOH react to 1 mol of sulfuric.

    Gotta find my mol of NaOH

    Mass / Molar weight = Mol

    72.8 g / 40 g/m = 1.82 mol NaOH

    As the relation is 1:2, I have the half of sulfuric: 0.91 mol.

    By a rule of three, will be

    2 mol NaOH __ react __ 1 mol H2SO4

    1.82 mol NaOH __react ___ (1.82.1) / 2

    Finally we have to work with molarity, which means mol/L. So, the rule of three is:

    0.240 mol H2SO4 __are in __ 1 L

    0.91 mol H2SO4___ are in ___ (0.91.1) / 0.240 = 3.79L
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Find the volume of 0.240 M sulfuric acid necessary to react completely with 72.8 g sodium hydroxide. Express your answer with the ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers