# Question #5cde3

##### 1 Answer

#### Explanation:

In the context of an *acid - base reaction*, **normality** represents the **number of equivalents** of hydronium cations, **one mole** of an acid or of a base present in **one liter of solution**.

In your case, a **equivalents** of hydroxide anions **for every mole** of base dissolved **per liter** of solution.

You can thus say that you have

#15 color(red)(cancel(color(black)("mL"))) * (1 color(red)(cancel(color(black)("L"))))/(10^3color(red)(cancel(color(black)("mL")))) * ("0.2 equiv. OH"^(-))/(1color(red)(cancel(color(black)("L base solution")))) = "0.0030 equiv. OH"^(-)#

You know that a neutralization reaction implies

#"H"_ 3"O"_ ((aq))^(+) + "OH"_ ((aq))^(-) -> 2"H"_ 2"O"_((l))#

Since **every equivalent** of hydronium cations requires **equivalent** of hydroxide anions, you can say that the acid solution contained **equivalents** of hydronium cations.

Therefore, the normality of the acid will be

#"normality acid" = ("0.0030 equiv. H"_3"O"^(+))/(30 * 10^(-3)"L") = color(green)(|bar(ul(color(white)(a/a)"0.1 N"color(white)(a/a)|)))#

The answer is rounded to one **sig fig**.