Question

A student titrated a 25.00 mL sample of a solution containing an unknown weak, diprotic acid...

A student titrated a 25.00 mL sample of a solution containing an unknown weak, diprotic acid (H2A) with NaOH. If the titration required 17.73 mL of .1036 M NaOH to completely neutralize the acid, calculate the concentration (in M) of the weak acid in the sample.

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
A sample of a diprotic weak acid (H2A) was titrated with 0.0500M NaOH (a strong base)...
A sample of a diprotic weak acid (H2A) was titrated with 0.0500M NaOH (a strong base) The initial acid solution had a concentration of 0.0250M and had a volume of 50.0mL. For the acid Ka1=1.0*10-3 and Ka2=1.0*10-6. a) calculate Ve1 and Ve2 b) Calculate the pH after 40.0mL of NaOH was added c)Calculate the pH after 40.0mL of NaOH was added
A solution containing an unknown concentration of HBr was titrated with 0.100 M KOH. 25.00 mL...
A solution containing an unknown concentration of HBr was titrated with 0.100 M KOH. 25.00 mL of the HBr solution was pipetted into a beaker. The HBr solution was then titrated with the 0.100 M KOH and 18.60 mL of KOH was added to reach the end point. Calculate the concentration of the HBr in the original solution
A 25.00 mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1322...
A 25.00 mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 41.22 mL of KOH is required to reach the equivalence point. What is the concentration of the unknown H2SO4 solution? Express your answer in molarity to four significant figures.
In titrating an acid of unknown concentration, a 20.00 mL sample of the acid was titrated...
In titrating an acid of unknown concentration, a 20.00 mL sample of the acid was titrated using standardized sodium hydroxide. The NaOH had a concentration of 0.1105 M. The titration required 35.45 mL of the base to reach the end-point in the titration. a) How many moles of H+ was in the 20.00 mL sample of acid? b) The solution of acid was prepared by adding 9.605 grams of the acid to 1.000 liter of water. What was the molecular...
An 80.9 mL sample of a 0.100 M solution of a diprotic acid, H2A, is titrated...
An 80.9 mL sample of a 0.100 M solution of a diprotic acid, H2A, is titrated with 0.100 M KOH. For H2A, Ka1 = 8.09 x 10^-5 and Ka2 = 8.09 x 10^-10. A) Calculate the concentration of A2- prior to the addition of any KOH. B) What is the pH of the initial solution? C) What is the pH exactly halfway to the first equivalence point? D) What is the pH exactly halfway between the first and second equivalence...
14.27mL of a solution of the diprotic acid H2SO4 is titrated, and 53.90 mL of 0.35M...
14.27mL of a solution of the diprotic acid H2SO4 is titrated, and 53.90 mL of 0.35M NaOH is required to reach the equivalence point. What is the originial concentration of the acid solution?
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...
A  25.00-mL  sample of propionic acid,  HC3H5O2,  of unknown concentration A  25.00-mL  sample of propionic acid,  HC3H5O2,  of unknown concentration  was titrated w
A  25.00-mL  sample of propionic acid,  HC3H5O2,  of unknown concentration A  25.00-mL  sample of propionic acid,  HC3H5O2,  of unknown concentration  was titrated with  0.151  M  KOH. The equivalence point was reached when was titrated with  0.151  M  KOH. The equivalence point was reached when  41.28  mL  of base had been added. What is the pH at the equivalence point?    41.28  mL  of base had been added. What is the pH at the equivalence point?     Ka   for propionic acid is    1.3×10–5   at  25°C.Ka   for propionic acid is    1.3×10–5   at  25°C. Select one: a. 8.93 b. 7.65 c. 9.47 d. 5.98 e. 9.11
1)A 40.0 mL sample of 0.045 M ammonia is titrated with 25.00 mL of 0.080 M...
1)A 40.0 mL sample of 0.045 M ammonia is titrated with 25.00 mL of 0.080 M HCl. If pK_bb​ = 4.76 for ammonia, what is the solution pH? 2) The single equivalence point in a titration occurs at pH = 5.65. What kind of titration is this? A Strong acid titrated with a strong base B Weak acid titrated with a strong base C Weak base titrated with a strong acid
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH....
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH. To reach the endpoint of the titration, 30.00 mL of NaOH solution is required. Ka = 1.8 x 10-4 What is the concentration of formic acid in the original solution? What is the pH of the formic acid solution before the titration begins (before the addition of any NaOH)?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT