High School

We appreciate your visit to The weak acid text HZ has a K a of 1 55 times 10 4 Calculate the text pOH of 0 045 M text HZ. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!

The weak acid \( \text{HZ} \) has a \( K_a \) of \( 1.55 \times 10^{-4} \). Calculate the \( \text{pOH} \) of 0.045 M \( \text{HZ} \).

Answer :

The pOH of the 0.045 M HZ solution is approximately 3.54.

Given the Ka value of HZ as [tex]\(1.55 \times 10^{-4}\),[/tex] we can determine the concentration of [tex]\(H^+\)[/tex] ions in the solution using the dissociation equilibrium of the weak acid:

[tex]\[K_a = \frac{[H^+][Z^-]}{[HZ]}\][/tex]

Since HZ is a weak acid, we can approximate that the concentration of[tex]\(Z^-\) ions (\([Z^-]\))[/tex] is equal to the concentration of [tex]\(H^+\)[/tex]ions [tex](\([H^+]\))[/tex] produced by the dissociation of HZ. Hence, we can rewrite the equation as:

[tex]\[K_a = \frac{[H^+]^2}{[HZ]}\][/tex]

Solving for [tex]\([H^+]\),[/tex] we find:

[tex]\[ [H^+] = \sqrt{K_a \times [HZ]} = \sqrt{1.55 \times 10^{-4} \times 0.045} \approx 1.57 \times 10^{-3} \text{ M}\][/tex]

The pOH can be calculated using the relationship between pH and [tex]\(H^+\) concentration (\([H^+]\)), which is \(pH = -\log([H^+])\). Since \(pH + pOH = 14\),[/tex] we can find the pOH:

[tex]\[pOH = 14 - pH = 14 - (-\log(1.57 \times 10^{-3})) \approx 3.54\][/tex]

Thus, the pOH of the solution is approximately 3.54.

Thanks for taking the time to read The weak acid text HZ has a K a of 1 55 times 10 4 Calculate the text pOH of 0 045 M text HZ. We hope the insights shared have been valuable and enhanced your understanding of the topic. Don�t hesitate to browse our website for more informative and engaging content!

Rewritten by : Barada