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Author:
Hurterr6
- Replies:
0
- Views: 61
Question regarding pH titration curve and conductimetric titration
Just wanted some input and guidance on my answers if they were correct or not. The questions are as follows:
[size=medium](b)Two 0.0400 M acid solutions were prepared (labelled A1 and A2). One of them was a weak acid and the other was a strong acid. The pH of A1 was 4.52 and of A2 was 1.40. Assume that all activity coefficients are equal to 1.
© 25.00 ml of each of the acids in part (b) was titrated with 0.1000 M KOH.
(i) Sketch the pH titration curve expec
Author:
Aurelius
- Replies:
0
- Views: 74
Help determining a diluted unknown concentration from a standard curve
I need help with the math, I'm not sure where I'm going wrong.
I've measured the potential of calcium standards using an electrode and produced a calibration curve (potential (mV) against log(concentration (mol/L)) with a linear regression of y=19.4x+22.6 (with an rsquared value of 0.962).
Now the unknown sample was was diluted in 50 mL of water and measured to have a potential of -38 mV so:
[size=medium]-38=19.4x+22.6 x=-3.1
Author:
Electra
- Replies:
0
- Views: 99
Equation for Titration Curve
Why doesn't the equation for the pka of an acid, i.e. pKa=-logKa=-log[H3O+]-log[A-/AH]=pH-log[A-/AH], which rearranges to give A-/AH=e^(pH-pka), describe the shape of a titration curve? :-\
It seems to account for all the variables in the titration curve, yet the titration curve is clearly not exponential. This shows that my knowledge of pH is fundamentally flawed..
help would be greatly appreciated