# Question #4e291

##### 1 Answer

#### Answer:

#### Explanation:

*Hydrochloric acid*, **strong acid** that ionizes completely in aqueous solution to form hydronium cations,

As you can see, **every mole** of hydrochloric acid will produce **one mole** of hydronium cations and **one mole** of chloride anions

The pH of the solution is calculated by taking the *negative log base*

#color(blue)(|bar(ul(color(white)(a/a)"pH" = - log(["H"_3"O"^(+)])color(white)(a/a)|)))#

You can express the concentration of the hydronium cations in term of the solution's pH by rewriting the above equation as

#log(["H"_3"O"^(+)]) = -"pH"#

This will be equivalent to

#10^log(["H"_3"O"^(+)]) = 10^(-"pH")#

which will give you

#color(blue)(|bar(ul(color(white)(a/a)["H"_3"O"^(+)] = 10^(-"pH")color(white)(a/a)|)))#

In your case, the solution is said to have a pH of

#["H"_3"O"^(+)] = 10^(-4.65)#

#["H"_3"O"^(+)] = color(green)(|bar(ul(color(white)(a/a)2.24 * 10^(-5)"M"color(white)(a/a)|)))#