In a potentiometric pH titration of a weak acid, why does the pH change rapidly with...

In a potentiometric pH titration of a weak acid, why does the pH change rapidly with the addition of NaOH near the endpoint but changes very slowly for pH values near the pKa of the acid?

Expert Solution

queen_honey_blossom answered 2 years ago

Calculation of pH after Titration of Weak Acid: Calculation of pH after Titration of Weak Acid:...

Calculation of pH after Titration of Weak Acid: Calculation of pH after Titration of Weak Acid: A compound has a p K a of 7.4. To 100 mL of a 1.0 M solution of this compound at pH 8.0 is added 30 mL of 1.0 M hydrochloric acid. What is the pH of the resulting solution? Can you explain what to do after 3.98 = A/HA

The pH change around the equivalence point for strong-base/weak-acid titration is usually not as great as...

The pH change around the equivalence point for strong-base/weak-acid titration is usually not as great as that for strong-base/strong-acid. The statement is true or not. Explain.

Why does the curve of titration of acetic acid begin at a higher pH than the...

Why does the curve of titration of acetic acid begin at a higher pH than the curve for HCl? Why does the pH at the center of the rapidly rising region occur at a higher pH for the acetic acid curve than for the HCl curve?

Weak Acid - Strong Base Titration Calculate the pH at the given amounts below in the...

Weak Acid - Strong Base Titration Calculate the pH at the given amounts below in the titration. You are titrating 35.0 mL of .15 M HNO2 with .1 M NaOH until you reach 100 mL of NaOH added. For this problem the Ka value is 4.6 x 10-4 a) 0.00 mL NaOH added b) 30.0 mL NaOH added c) 60.0 mL NaOH added d) 100.0 mL NaOH added

What is the pH of a weak acid strong base titration after each of the following...

What is the pH of a weak acid strong base titration after each of the following additions? Ka for HF is 3.5 x 10-4. a. 10.0 mL of 0.250 M NaOH added to 15.0 mL of 0.400 M HF b. 25.0 mL of 0.250 M NaOH added to 35.0 mL of 0.1785 M HF c. 20.0 mL of 0.250 M NaOH added to 20.0 mL of 0.350 M HF Please show your work so I can better understand this. thanks!...

What is the approximate pH at the equivalence point of a weak acid-strong base titration if...

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL 21) of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? Ka =1.8 × 10-4 for formic acid. A) 2.46 B) 8.12 C) 11.54 D) 5.88

The titration of weak diprotic acid H2A with strong base is conducted. What is the pH...

The titration of weak diprotic acid H2A with strong base is conducted. What is the pH of the solution at the following volumes, 0,10,25,50,60,75,100,125,and 150mL if Ka1=1.0x10^-4 and Ka2=3.5x10^-4 and the concentrations for both HA- and OH- are 0.1M?

Consider the titration of the weak acid HA with NaOH. At what fraction of Ve does...

Consider the titration of the weak acid HA with NaOH. At what fraction of Ve does pH = pKa -1? At what fraction of Ve does pH = pKa +1? Use these two points, plus Vb = 0, 1/2Ve, Ve, and 1.2Ve to sketch the titration curve for the reaction of 100 mL of 0.100M anilinium bromide ("aminobenzene x HBr") with 0.100M NaOH.

Every weak acid has the following unique characteristic(s): a. at the 50% titration point the pH...

Every weak acid has the following unique characteristic(s): a. at the 50% titration point the pH = pKa b. the best buffering occurs +/- one pH unit of the pKa c. the change in pH with added acid or base is the least when pH = pKa d. the shape of the titration curve is essentially the same for all weak acids e. all of the above If the pH of a buffer with a pKa of 6 changes from...

The potentiometric titration of 25.00 mL of malonic acid C3H4O4 (pKa values 2.83 and 5.69) with...

The potentiometric titration of 25.00 mL of malonic acid C3H4O4 (pKa values 2.83 and 5.69) with 0.2217 M NaOH gave endpoints at 16.47 mL and 32.01 mL. A)Sketch the titration curve (roughly - don’t worry about exact pH values, just the general shape of the curve) and label each of the following points with the major acid or base species and the type of acid/base solution (e.g., strong acid, weak base, amphiprotic, buffer, pka values, endpoints,): i.)the beginning (before any...

Question