Question
What is the $\mathrm{pH}$ of a buffer solution containing $2 \mathrm{M}$ potassium oxalate solution and $0.02 \mathrm{M}$ oxalic solution in one-liter, assuming the $\mathrm{pK}_{\mathrm{a}}$ of oxalic acid is 4.21 at $25^{\circ} \mathrm{C}$ ?
Step 1
Step 1: Write the chemical equation for the dissociation of oxalic acid (H2C2O4) in water: \[H_{2}C_{2}O_{4} \rightleftharpoons H^{+} + HC_{2}O_{4}^{-}\] Show more…
Show all steps
Your feedback will help us improve your experience
David Collins and 88 other 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
What is the $\mathrm{pH}$ of a $0.25 \mathrm{M}$ solution of sodium oxalate, $\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4} ?$
Calculate the $\mathrm{pH}$ at $25^{\circ} \mathrm{C}$ of a $0.25 \mathrm{M}$ aqueous solution of oxalic acid $\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right) .\left(K_{\mathrm{a}_{1}} \text { and } K_{\mathrm{a}_{2}} \text { for oxalic acid are } 6.5 \times 10^{-2}\right.$ and $6.1 \times 10^{-5}$, respectively.)
What is the $\mathrm{pH}$ of a buffer solution that is $0.15 \mathrm{M}$ chloroacetic acid and $0.10 \mathrm{M}$ sodium chloroacetate? $K_{a}=$ $1.3 \times 10^{-3}$
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD