I usually ask annoyingly hard questions but this is although is simple it's kind of confusing. This question isn't something for an exam or a lab just as a concept for myself.
While titrating I can make a plot of pH vs added titrant which I can find the equivalence point easily (or using color changes due to phenolphthalein indicator) but to find the half equivalence point we needed to plot the first derivative graph to find peaks (one major and one minor which are the equivalence and half equivalence points respectively). so why do all of that if you can just take equivalence point divided by two? Also, the half equivalence point determined through the first derivative graph is different than the one determined through equivelance/2 which is also different than the one determined through color changes in titration! which is correct?
Thanks!
As the title says, what is the significance of equivalence relations.
I am confused as to why does moles of acid equal to the moles of base at equivalence point. Since all the acid has been neutralized at equivalence point, wouldn't there be no more HA left, so the moles of HA (acid) would be zero??
Does time travel violate the mass-energy equivalence principle by adding additional mass at a point in time in the universe? I mean like, if I meet my former self, there'd be two selfs each with 175 pounds of weight or 80 kilos of mass, whereas before there was only one.
Can someone explain to me the relationship of the polyprotic acid equivalence points?
I thought at equivalence points, the moles of base added equals to the moles of acid consumed. So why are the picture using molarity instead of moles?
https://preview.redd.it/8cbuwt4ezbh61.png?width=1210&format=png&auto=webp&s=a8386cd40a022519e59df05e61e53db9e68fbb6c
Writing a report on the Ksp of KNO3 and just wanted to know if the equivalence points denotes a state of equilibrium being reached.
For my entire chemistry career starting from high school through 3 years of undergrad, I have not been able to get a firm grasp of acid/base chem.
To determine what volume of base to add to an acid in a titration problem, can we simply use M1V1=M2V2? Or is this only if we have monoprotic and monobasic species (i.e., HF and NaOH). Would this not work with, say, H3PO4 and NaOH?
Also, if anyone has any tips on resources that helped them solidify acid/base chem, I'd appreciate that!
Came across a Uearth problem that says that in a diprotic acid, where
H2A + OH- <-> HA- + H2O HA- + OH- <-> A^2- + H2O
It says that the second equivalence point is [A^2-]= 0.5[OH-]
Why is there a 0.5 before the OH here? Shouldn't it just be conjugate base= the [OH-]?
I've searched for like an hour online, and I couldn't find any answers...
From what I'm understanding, half-equivalence point is when half of the analyte (let's say HA) is neutralized. I'm not sure why halving the amount of HA would make it so that the concentration of HA = concentration of its conjugate base A-. Could someone break down the reasoning for me?
I mean, would the concentration of HA even be two times the concentration of A- in the first place?? One molecule of HA forms one A-, right? I'm sure I'm not understanding this correctly, bc none of this seems right...
Could someone explain when to use the equivalence point equation: NaVa = NbVb?
Kaplan has a question for a neutralization reaction and asked "How many liters of 2 M Ba(OH)2 are needed to titrate a 4 L solution of 6 M H3PO4?". I incorrectly used dilution equation M1V1= M2V2.
When looking at a titration graph, does the isoelectric point always occur at the first equivalence point?
