a solution containing hcl would likely have\na high ph and a low poh.\na low ph and a high poh.\na high ph…

Answer:

a low pH and a high pOH.

Explanation:

Step1: Analyze the nature of HCl

HCl is a strong acid. In aqueous solution, it dissociates completely: $HCl\rightarrow H^{+}+Cl^{-}$.

Step2: Recall the relationship between pH and $H^{+}$ concentration

The formula for pH is $pH =-\log[H^{+}]$. Since HCl produces a high concentration of $H^{+}$ ions ($[H^{+}]$ is large), using the formula $pH =-\log[H^{+}]$, a large $[H^{+}]$ leads to a low pH value. For example, if $[H^{+}]=1M$, then $pH =-\log(1) = 0$.

Step3: Recall the relationship between pH and pOH

We know the relationship $pH + pOH=14$ (at $25^{\circ}C$). Rearranging this formula gives $pOH = 14 - pH$. Since pH is low (from Step 2), substituting into the $pOH = 14 - pH$ formula, when pH is small (e.g., pH = 1), then $pOH=14 - 1=13$, so pOH is high.