Question #a6b5e
1 Answer
Sodium hydroxide.
Explanation:
Start by writing the balanced chemical equation that describes this neutralization reaction
#"H"_ 2"SO"_ (4(aq)) + color(blue)(2)"NaOH"_ ((aq)) -> "Na"_ 2"SO"_ (4(aq)) + 2"H"_ 2"O"_ ((l))#
Notice that the reaction consumes
In other words, the reaction will always consume twice as many moles of sodium hydroxide than moles of sulfuric acid, regardless of how many moles of sulfuric acid take part in the reaction.
Now, you know that you have
- three moles of sulfuric acid,
#3 xx "H"_2"SO"_4# - four moles of sodium hydroxide,
#4 xx "NaOH"#
All you have to do to figure out is you're dealing with a limiting reagent is pick one of the reactants and check to see if you have enough moles of the second reactant available.
For example, let's pick sulfuric acid. You know that
#3 color(red)(cancel(color(black)("moles H"_2"SO"_4))) * (color(blue)(2)color(white)(a)"moles NaOH")/(1color(red)(cancel(color(black)("mole H"_2"SO"_4)))) = "6 moles NaOH"#
Since you only have
More specifically, the reaction will consume all the moles of sodium hydroxide and
#4color(red)(cancel(color(black)("moles NaOH"))) * ("1 mole H"_2"SO"_4)/(color(blue)(2)color(red)(cancel(color(black)("moles NaOH")))) = "2 moles H"_2"SO"_4#
After the reaction is complete, you will be left with
#overbrace("3 moles H"_2"SO"_4)^(color(purple)("what you start with")) - overbrace("2 moles H"_2"SO"_4)^(color(darkgreen)("what is consumed")) = overbrace("1 mole H"_2"SO"_4)^(color(brown)("unreacted"))#