Consider a weak acid, HX. If a 0.10 M solution of HX has a pH of 5.83 at 25 C. What is ΔG for the acids dissociation?
Added by Patricia S.
Step 1
We can use the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions. From the given pH of 5.83, we can calculate [H+] as 10^-5.83 M. Since it's a weak acid, we can assume that the concentration of HX at equilibrium is approximately the Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 58 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Consider a weak acid HX. If a $0.10 M$ solution of $mathrm{HX}$ has a pH of 5.83 at $25^{circ} mathrm{C},$ what is $Delta G^{circ}$ for the acid's dissociation reaction at $25^{circ} mathrm{C} ?$
David C.
At $25^{\circ} \mathrm{C},$ a $0.327 \mathrm{M}$ solution of a weak acid HX has a $\mathrm{pH}$ of $5.12 .$ What is $\Delta G^{\circ}$ for the dissociation of the weak acid?
An aqueous solution of 0.057 M weak acid, HX, has a pH of 4.65. What is the pH of the solution if 0.018 mol of KX is dissolved in one liter of the weak acid?
Tianyu L.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
600,000+
Students learning Chemistry with Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD
