Question

Draw a titration curve that shows how the pH of a diprotic acid changes as 30...

Draw a titration curve that shows how the pH of a diprotic acid changes as 30 mL total of NaOH is added. Label both equivalence points and half equivalence points, including their associated volumes on the x-axis. You should also label pH values on the y-axis that are associated with the half-equivalence volumes.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The other sheet shows titration curves for reaction of a diprotic acid with NaOH. On this...
The other sheet shows titration curves for reaction of a diprotic acid with NaOH. On this sheet you need to enter the two Ka values of the acid manually, in cells E1 = 1.00 x 10-3 And E2 = 1.0 0x 10-8. Enter the volume and concentration data in the pink cells G1, G2 and G4:             Volume of acid: 100mL:                     Enter 100             Concentration of acid: 0.040M           Enter 0.040             Concentration of NaOH: 0.20M         Enter 0.20 What is the pH after 40 mL of NaOH...
The titration curve for a 25.0 ml sample of benzoic acid shows that 10.0 ml of...
The titration curve for a 25.0 ml sample of benzoic acid shows that 10.0 ml of 0.100M NaOH is required to reach the equivalence point. 1. What is the concentration of the original benzoic acid sample? 2. What is the pH at the equivalence point? 3. Calculate the pH after addition of 5.00 ml of NaOH and the pOH after addition of 20.0 ml NaOH.
The titration curve for a 25.0 ml sample of benzoic acid shows that 10.0 ml of...
The titration curve for a 25.0 ml sample of benzoic acid shows that 10.0 ml of 0.100M NaOH is required to reach the equivalence point. (See #3 for Ka info.) i) What is the concentration of the original benzoic acid sample? ii) What is the pH at the equivalence point? iii) Calculate the pH after addition of 5.00 ml of NaOH and the pOH after addition of 20.0 ml NaOH.
c) Draw a titration curve that represents the titration of a strong acid with a strong...
c) Draw a titration curve that represents the titration of a strong acid with a strong base. Label the axes. d) What is meant by the term "equivalence point"? e) At what point along a titration curve is pKa=pH for a strong acid? f) At what point along a titration curve is pKa=pH for a weak acid?
I am looking for the molecular weight of an unknown acid in a titration. My acid...
I am looking for the molecular weight of an unknown acid in a titration. My acid is diprotic, the equivalence points are at 1.4 mL (of NaOH added) and 3 mL (of NaOH added). The molarity of NaOH is 0.98 M. I used 0.025 g of the unknown acid in the titration. How do I find the molecular weight of the unknown acid?
The titration of 0.02500 L of a diprotic acid solution with 0.1000 M NaOH requires 34.72...
The titration of 0.02500 L of a diprotic acid solution with 0.1000 M NaOH requires 34.72 mL of titrant to reach the second equivalence point. The pH is 3.95 at the first equivalence point and 9.27 at the second equivalence point. What is the pKa1 and pKa2 of the acid? Thank You
16.5 mL of 0.168 M diprotic acid (H2A) was titrated with 0.118 M KOH. The acid...
16.5 mL of 0.168 M diprotic acid (H2A) was titrated with 0.118 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10. At what added volume (mL) of base does the first equivalence point occur? 20.8 mL of 0.146 M diprotic acid (H2A) was titrated with 0.14 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10. At what added volume (mL) of base does the second equivalence point occur? Consider the titration of...
Titration of a weak acid with a strong base. the ph curve for titration of 50.0ml...
Titration of a weak acid with a strong base. the ph curve for titration of 50.0ml of a 0.100 M of acetic acid with a 0.100 M solution of NaOH (aq). For clarity, water molecules have been omitted from the molecular art. a) If the acetic acid being titrated here were replaced by hydrochloric acid, would the amount of base needed to reach the equivalence point change? b) Would the pH at the equivalence point change? -yes the pH at...
draw titration curve and determine pHs A Titration Curve Gives Us A Lot Of Information About...
draw titration curve and determine pHs A Titration Curve Gives Us A Lot Of Information About Acids, Bases, Buffers, and Charge 20 ml of 0.1 M H3PO4 (triprotic acid) is titrated with 0.1 M NaOH. Calculate pH at start, 1/2 way points, and end points. At 1st and 2nd endpoints: pH = 0.5 (pKai + pKa(i+1)) Draw titration curve and show buffer region(s). Show the phosphorus compound and charge at each point.
2. The Ka of nitrous acid is 4.5 x 10-4. In a titration 50.0 mL of...
2. The Ka of nitrous acid is 4.5 x 10-4. In a titration 50.0 mL of a 1.00 M solution is titrated with 0.750 M NaOH. Calculate the pH of the solution: a. Before the titration begins. b. When sufficient NaOH has been added to neutralize half of the nitrous acid originally present. c. At the equivalence point. d. When 0.05 mL of NaOH less than that required to reach the equivalence point has been added. e. When 0.05 mL...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT