Question

the ph of a solution is 2.0. which statement is correct? useful formulas include $\ce{h3o+} = 10^{-\text{ph}}$, $\ce{oh-} = 10^{-\text{poh}}$, $\text{ph} + \text{poh} = 14$, and $\ce{h3o+}\ce{oh-} = 10^{-14}$

• the poh of the solution is 12.0.
• the concentration of $\ce{oh-}$ ions is $1.0 \times 10^{-2}$ m.
• the concentration of $\ce{h3o+}$ ions is 100.0 m.
• the poh of the solution is 16.0.

Explanation:

Step1: Recall the relationship between pH and pOH

We know that the formula relating pH and pOH is $pH + pOH = 14$.

Step2: Calculate pOH using the given pH

Given that $pH = 2.0$, we substitute this value into the formula $pOH=14 - pH$.
So, $pOH = 14 - 2.0 = 12.0$.

Step3: Analyze other options

• For the option "The concentration of $\ce{OH-}$ ions is $1.0\times10^{-2}\ M$": Using the formula $[\ce{OH-}]=10^{-pOH}$, and $pOH = 12.0$, so $[\ce{OH-}]=10^{- 12.0}=1.0\times10^{-12}\ M

eq1.0\times10^{-2}\ M$.

• For the option "The concentration of $\ce{H3O+}$ ions is $100.0\ M$": Using the formula $[\ce{H3O+}]=10^{-pH}$, and $pH = 2.0$, so $[\ce{H3O+}]=10^{-2.0}=1.0\times10^{-2}\ M

eq100.0\ M$.

• For the option "The pOH of the solution is 16.0": From $pH + pOH = 14$, with $pH = 2.0$, $pOH = 14 - 2.0 = 12.0

eq16.0$.

Answer:

A. The pOH of the solution is 12.0.