Asked by Anonymous
Explain how to prepare 1L of a buffer at pH 7.4 using 1M hypochlorous acid (Ka = 3.5 x 10-8) and a 1 M NaOH solution. Indicate the volume of hypochlorous acid and sodium hydroxide to use.
pH = pKa + log ([A-]/[HA])
Ka= [H+][A-]/[HA]
Molarity = moles/L
moles = g/molecular weight
pH = pKa + log ([A-]/[HA])
Ka= [H+][A-]/[HA]
Molarity = moles/L
moles = g/molecular weight
Answers
Answered by
Devron
pka=-log(3.5 x 10^-8)=7.46
pH=pKa+ log ([A-]/[HA]),
solve for [A-]/[HJA]
10^(pH-pKa)=[A-]/[HJA]=0.879
1-0.879=0.121=[A-]
Add 121mL of NaOH solution to a volumetric flask, and add HClO to the 1,000mL mark of a 1,000mL volumetric flask.
pH=pKa+ log ([A-]/[HA]),
solve for [A-]/[HJA]
10^(pH-pKa)=[A-]/[HJA]=0.879
1-0.879=0.121=[A-]
Add 121mL of NaOH solution to a volumetric flask, and add HClO to the 1,000mL mark of a 1,000mL volumetric flask.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.