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QUESTION

# What is the hydroxide ion concentration in a solution of "NH"_3 with a "pOH" of 4.65?

["OH"^(-)] = 2.24 * 10^(-5)"M"

Your starting point here will be the definition of a solution's "pOH", which as you know is defined as the negative log base 10 of the concentration of hydroxide anions, "OH"^(-)

color(blue)(ul(color(black)("pOH" = - log(["OH"^(-)]))))

Now, in order to solve for the concentration of hydroxide anions, you must rearrange this equation as

log(["OH"^(-)]) = - "pOH"

and rewrite it using exponents of base 10

10^log(["OH"^(-)]) = 10^(-"pOH")

This is equivalent to

color(blue)(ul(color(black)(["OH"^(-)] = 10^(-"pOH"))))

Now all you have to do is to plug in the value given to you for the "pOH" of the solution

["OH"^(-)] = 10^(-4.65) = color(darkgreen)(ul(color(black)(2.24 * 10^(-5)"M")))

I'll leave the answer rounded to three .