Timeline for Why doesn't pH = pKa1 in the buffer zone for this titration?
Current License: CC BY-SA 4.0
11 events
| when toggle format | what | by | license | comment | |
|---|---|---|---|---|---|
| Aug 4, 2018 at 22:36 | vote | accept | Cyclopropane | ||
| Aug 4, 2018 at 12:03 | answer | added | Oscar Lanzi | timeline score: 1 | |
| Aug 4, 2018 at 3:23 | comment | added | Zhe | @MaxW Thanks for the correction, but a pKa value of 0.6 is still a fairly strong acid. | |
| Aug 4, 2018 at 0:10 | comment | added | MaxW | @Zhe - $\ce{H2S2O3}$ is thiosulfuric acid not sulforous acid which is $\ce{H2SO3}$. | |
| Aug 3, 2018 at 23:53 | comment | added | Zhe | Sulfurous acid is pretty strong. It's pretty much fully deprotonated as soon as you add it to water. | |
| Aug 3, 2018 at 23:46 | comment | added | Cyclopropane | @MaxW So it doesn't apply in this case because the original concentration of the acid is too high? | |
| Aug 3, 2018 at 23:27 | comment | added | MaxW | @KaienYang - Even if both protons ionized you could only get a acid concentration of 0.02 molar which is only a pH of 1.69. In other words the Henderson–Hasselbalch equation doesn't apply in this case. | |
| Aug 3, 2018 at 23:03 | comment | added | Cyclopropane | @Mithoron So pKa doesn't always equal pH at the half equivalence point? | |
| Aug 3, 2018 at 22:14 | comment | added | Mithoron | How could you have pH=0.6 if concentration was only 0.01 to begin with? | |
| Aug 3, 2018 at 21:37 | history | edited | user7951 | CC BY-SA 4.0 |
added 139 characters in body
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| Aug 3, 2018 at 21:21 | history | asked | Cyclopropane | CC BY-SA 4.0 |