Question

1)For a titration of 25.00mL of .1000M acetic acid with .1000M NaOH calculate the pH    ...

1)For a titration of 25.00mL of .1000M acetic acid with .1000M NaOH calculate the pH

    a)before the addition of any NaOH solution

    b) after 10.00mL of the base is added

    c) after half the acid is neutralized

    d) at the equivalence point

2) What is the pKa of the acid?

Homework Answers

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
A sample of acetic acid (weak acid) was neutralized with .05M NaOH solution by titration. 34...
A sample of acetic acid (weak acid) was neutralized with .05M NaOH solution by titration. 34 mL of NaOH had been used. Show your work. CH3COOH + NaOH-----CH3COONa + H2O a) Calculate how many moles of NaOH were used? b) How many moles of aspirin were in a sample? c) Calculate how many grams of acetic acid were in the sample d) When acetic acid is titrated with NaOH solution what is the pH at the equivalence point? Circle the...
Titration of acetic acid: How to calculate moles of NaOH added Moles of acetic acid neutralized...
Titration of acetic acid: How to calculate moles of NaOH added Moles of acetic acid neutralized by NaOH Mass of acetic acid Mass % of acetic acid in solution Average mass % of acetic acid
Calculate the pH of a titration mixture of acetic acid with NaOH when 45.00 mL of...
Calculate the pH of a titration mixture of acetic acid with NaOH when 45.00 mL of NaOH has been added, considering that the equivalence point of the mixture is 22.98 mL. Concentration of acetic acid = 0.1081mol/L Concentration of NaOH = 0.1185 mol/L Volume of Acetic Acid sample = 25.00 mL DO NOT use henderson hasselbalch equation
Consider the titration of a 60.0 mL of a 0.20M formic acid solution (HCHO2) with 0.10M...
Consider the titration of a 60.0 mL of a 0.20M formic acid solution (HCHO2) with 0.10M NaOH. A) Calculate the initial pH of the formic acid solution, before any base is added. B) At what point in the titration is pH = pKa? What volume of the NaOH will have been added to get to this point? C) Calculate the pH after 30.0 mL of the base has been added.
You titrate a 20.0 mL acid sample containing 1.104 g of ascorbic acid (molar mass=176.12 g/mol...
You titrate a 20.0 mL acid sample containing 1.104 g of ascorbic acid (molar mass=176.12 g/mol and pKa=4.10) with 0.200 M NaOH. Calculate the following 1. The pH at the begining of the titration, before any base was added 2. The volume of base (NaOH) required to reach the equivalence point 3. The pH at the equivalence point and the half-equivalence point 4. The pH after 35.5 mL of base have beedn added
1) If 25.2 mL of 0.109 M acid with a pKa of 5.55 is titrated with...
1) If 25.2 mL of 0.109 M acid with a pKa of 5.55 is titrated with 0.102 M NaOH solution, what is the pH of the titration mixture after 13.7 mL of base solution is added? 2) If 28.8 mL of 0.108 M acid with a pKa 4.15 is titrated with 0.108 M NaOH solution, what is the pH of the acid solution before any base solution is added? 3)If 27.9 mL of 0.107 M acid with a pKa of...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution? 2. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with...
A 32.44 mL sample of 0.202M acetic acid is titrated with 0.185 M sodium hydroxide. Calculate...
A 32.44 mL sample of 0.202M acetic acid is titrated with 0.185 M sodium hydroxide. Calculate the pH of the solution 1. before any NaOH is added 2. after 24.00 mL of NaOH is added 3. at the equivalence point
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...
A 25.0 mL sample of an acetic acid solution in titrated with a 0.09984 M NaOH...
A 25.0 mL sample of an acetic acid solution in titrated with a 0.09984 M NaOH solution. The equivalence point is reached when 37.5 mL of the base is added. Calculate the concentration of acetic acid in the 25.0 mL sample. Calculate the pH at the equivalence point (Ka acetic acid = 1.75x10^-5)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT