Question

In: Chemistry

How is the shape of a monoprotic acid titration curve determined by the pk of the...

How is the shape of a monoprotic acid titration curve determined by the pk of the acidic proton?

Solutions

Expert Solution

Titration curves for strong acid vs. strong base

We'll take hydrochloric acid and sodium hydroxide as typical of a strong acid and a strong base.

Running acid into the alkali

You can see that the pH only falls a very small amount until quite near the equivalence point. Then there is a really steep plunge. If you calculate the values, the pH falls all the way from 11.3 when you have added 24.9 cm3 to 2.7 when you have added 25.1 cm

Running alkali into the acid

This is very similar to the previous curve except, of course, that the pH starts off low and increases as you add more sodium hydroxide solution.

Again, the pH doesn't change very much until you get close to the equivalence point. Then it surges upwards very steeply.

he equivalence point on the graph is where all of the starting solution (usually an acid) has been neutralized by the titrant (usually a base). It can be calculated precisely by finding the second derivative of the titration curve and computing the points of inflection (where the graph changes concavity); however, in most cases, simple visual inspection of the curve will suffice (in the curve given to the right, both equivalence points are visible, after roughly 15 and 30 mL of NaOH solution has been titrated into the oxalic acid solution. To calculate the acid dissociation constant (pKa), one must find the volume at the half-equivalence point, that is where half the amount of titrant has been added to form the next compound (here, sodium hydrogen oxalate, then disodium oxalate). Halfway between each equivalence point, at 7.5 mL and 22.5 mL, the pH observed was about 1.5 and 4, giving the pKa.

In monoprotic acids, the point halfway between the beginning of the curve (before any titrant has been added) and the equivalence point is significant: at that point, the concentrations of the two species (the acid and conjugate base) are equal. Therefore, the Henderson-Hasselbalch equation can be solved in this manner:


Related Solutions

how does titration of a strong monoprotic acid with a strong base differ from a titration...
how does titration of a strong monoprotic acid with a strong base differ from a titration for a weak monoprotic acid with a strong base with respect to the following a) quantity of base required to reach the equivalance point b) ph at the beginning of the titration c) ph at the equivalance point d) ph after addition of a slight access of base e) choice of indicator for determining the equivalence point
1. How does the titration of a diprotic acid differ from a monoprotic acid (like HF)?...
1. How does the titration of a diprotic acid differ from a monoprotic acid (like HF)? 2. How does the titration of a weak base with a strong acid differ from weak acid-strong base titration. (Review pages 848 - 850.) Note: you could perform these titrations from the chemical cabinet in this lab. 3. What kind of pH (above 7, below 7, or 7) do you expect at the equivalence point from the titration of a weak acid with a...
While running the titration of your unknown monoprotic acid with NaOH, the pKa of the acid...
While running the titration of your unknown monoprotic acid with NaOH, the pKa of the acid is 3.14. Considering the data in the following table, at what volume of NaOH would you need to reach the equivalence point? units mL, 1 decimal place Volume NaOH added (mL) pH 0 2.46 1.0 2.55 2.0 2.65 3.0 2.80 4.0 2.97 5.0 3.14 6.0 3.77 7.0 4.07 8.0 4.41
3. Plot a schematic titration curve for acetic acid with NaOH. Superimpose the titration curve of...
3. Plot a schematic titration curve for acetic acid with NaOH. Superimpose the titration curve of HCl on this graph. What are the main differences? How can we determine the pKa of acetic acid from its titration curve?
1.) Acetic acid is a weak monoprotic acid with Ka=1.8*10^-5. In an acid base titration, 100...
1.) Acetic acid is a weak monoprotic acid with Ka=1.8*10^-5. In an acid base titration, 100 mL of 0.100M acetic acid is titrated with 0.100M NaOH. What is the pH of the solution: a.)Before any NaOH is added b.)Before addition of 15.0mL of 0.100M NaOH c.)At the half-equivalence point d.)After addition of total of 65.0mL of 0.100M NaOH e.)At equivalence point f.)After addition of a total of 125.0mL of 0.100M NaOH
how many equivalence point(s) will appear on the titration curve during titration of phosphoric acid, H3PO4...
how many equivalence point(s) will appear on the titration curve during titration of phosphoric acid, H3PO4 with a strong base such as KOH
Titration without the PH meter: Calculate the molarity of your unknown, assuming it is monoprotic acid...
Titration without the PH meter: Calculate the molarity of your unknown, assuming it is monoprotic acid or monobasic base. Show all calculations for one titration with good precision including units and correct number of significant figures. Summarize only the results for the runs that you are using for the runs that you are using for your analyze concentration determination. Remember to account for any dilutions. Run 1 Run 2 Final burette reading (ml) 15.60 30.70 Initial (ml) 0.50 15.60 Volume...
Oxalic acid is a common dibasic acid. Draw a qualitative sketch of the titration curve for...
Oxalic acid is a common dibasic acid. Draw a qualitative sketch of the titration curve for a sample of oxalic acid titrated with a solution of NaOH. Label the end point(s). Assume the pKa's of oxalic acid are approximately 1.2 and 4.2 **Please Answer Correctly and show work. I will give you thumbs up (+1)**
REPORT FORM ; ACID TITRATION CURVE. Name of acid (or acid salt) NH4Cl mass of solid...
REPORT FORM ; ACID TITRATION CURVE. Name of acid (or acid salt) NH4Cl mass of solid acid = 0.160g NH4Cl volume of water used to dissolve acid =40ml NaOH(titrant)=30ml Data analysis: PH at equivalent point=11.25, pH at half equivalent point =9.49 Ka of =3.2*10^-10 Questions: calculate pH at beginning of titration, pH at equivqlent point, pH after 20.0ml of titrant were added. Thank you.kindly assist
Draw a titration curve for both a strong acid titrated by a strong base and a...
Draw a titration curve for both a strong acid titrated by a strong base and a weak acid titrated by a strong base. Identify the equivalence point and the half equivalence point on these graphs. Define each of these points and tell what information these points can give you. Also tell what species are present at the beginning of the titration, at the half equivalence point, at the equivalence point and after the equivalence point. . Draw a titration curve...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT