Question #46084
1 Answer
Explanation:
As you know, a solution's pH is a measure of the concentration of hydronium cations,
#color(blue)(|bar(ul(color(white)(a/a)"pH" = - log( ["H"_3"O"^(+)])color(white)(a/a)|)))#
In order to find the concentration of the hydronium cations when given the pH of the solution, use the fact that
#color(purple)(|bar(ul(color(white)(a/a)color(black)(10^log(a) = a)color(white)(a/a)|)))#
Rearrange the equation that defines the pH to get
#-"pH" = log(["H"_3"O"^(+)])#
This will be equivalent to
#10^(-"pH") = 10^log(["H"_3"O"^(+)])#
Finally, rearrange to find
#color(blue)(|bar(ul(color(white)(a/a)["H"_3"O"^(+)] = 10^(-"pH")color(white)(a/a)|)))#
Plug in the value given to you for the pH of the solution to get
#["H"_3"O"^(+)] = 10^(-7.25) = color(green)(|bar(ul(color(white)(a/a)5.6 * 10^(-8)"M"color(white)(a/a)|)))#
It's worth noting that a neutral aqueous solution at room temperature has equal concentrations of hydronium and hydroxide ions
#["H"_3"O"^(+)] = ["OH"^(-)] = 10^(-7)"M"#
As you can see, decreasing the concentration of hydronium ions results in an increase in pH. As a result, the solution goes from being neutral to being slightly basic.