Question

How do you tell equivalence point from a pH graph in titration lab? How to tell...

How do you tell equivalence point from a pH graph in titration lab? How to tell if an acid is triprotic

Homework Answers

Answer #1

in the graph almost the straight line which parellel to y-axis we observe at certain point . this is called equailvalence point.

or at one drop volume of titration addition the value drastacally changes. volume is very little amount but the pH change is very large . which you can see in the image

acid triprotic acid which gives three equivalence points . becuase it is triprotic acidic .

in the titration curve of acid and base , if we get three equivalence points that indicates it is triprotic acid

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What is the pH at the EQUIVALENCE POINT of the titration of 0.100 M NaOH into...
What is the pH at the EQUIVALENCE POINT of the titration of 0.100 M NaOH into a solution of 12.5 mL of 0.243 M butanoic acid
Before the equivalence point during a weak acid-strong base titration, the pH will be determined from...
Before the equivalence point during a weak acid-strong base titration, the pH will be determined from the concentration of the ____. a. strong base b. weak base c. strong acid d. weak acid e. conjugate base
a. What is the theoretical pH at the stoichiometric equivalence point for the titration of the...
a. What is the theoretical pH at the stoichiometric equivalence point for the titration of the weak acid? ACETIC ACID REACTING WITH NaOH Hint: Your volume at the stoichiometric point should include the amount of base you added to reach the stoichiometric point (4.174 mL) as well as the initial amount of stock HAc and the water added to cover the pH meter bulb. You should use the actual concentration of the HAc (from question 8a) in this calculation. Again,...
What is the pH at the equivalence point in the titration of a 23.6 mL sample...
What is the pH at the equivalence point in the titration of a 23.6 mL sample of a 0.385 M aqueous hydrocyanic acid solution with a 0.318 M aqueous sodium hydroxide solution?
This is in regards to a titration lab and how dilution would affect certain aspects of...
This is in regards to a titration lab and how dilution would affect certain aspects of it. I know that the initial unknown acid solution which has been diluted would have a higher pH, but a little confused about the remaining parts. Thanks for your help! Consider if the initial unknown acid solution used in this experiment started out more dilute. Predict any differences you would expect to see in the titration curve ‐ clearly identify what changes, if any,...
What is the pH at the equivalence point of a titration of the weak base NH3(aq)...
What is the pH at the equivalence point of a titration of the weak base NH3(aq) with the strong acid HBr(aq) if 30.00 mL of 0.200 M NH3 solution requires 30.00 mL of 0.200 M HBr to reach the equivalence point? Kb = 1.8 x 10–5 for NH3.
Determine the pH at the equivalence (stoichiometric) point in the titration of 31 mL of 0.15...
Determine the pH at the equivalence (stoichiometric) point in the titration of 31 mL of 0.15 M acrylic acid(aq) with 0.15 M NaOH(aq). The Ka of C2H4COOH is 5.5 x 10-5.
Calculate the pH at the equivalence point for the following titration: 0.100 M NaOH versus 1.60...
Calculate the pH at the equivalence point for the following titration: 0.100 M NaOH versus 1.60 g formic acid (HCO2H Ka = 1.8 x 10-4).
What is the pH at the equivalence point for the titration of a 25.0mL sample of...
What is the pH at the equivalence point for the titration of a 25.0mL sample of 0.175 M CH3NH2 with 0.150M HBr (Kb = 4.4x10-4)
What will be the pH at the equivalence point in the titration of 45.00 mL of...
What will be the pH at the equivalence point in the titration of 45.00 mL of 0.115 M NaClO with 0.106 M HCl? ClO–(aq) + HCl(aq) → HClO(aq) + Cl–(aq) Ka(HClO)=3.0·10-8 You only need to provide the final answer (pH).