Question

DULLOH HILL UCUREI LULUS solution in the beaker. 13. When you have finished the testing, dispose of the reaction mixture as d
0 0
Add a comment Improve this question Transcribed image text
Answer #1

Solution:

1) In the titration of a weak acid, the pKa of the acid is equivalent with the pH at half equivalence point.

Thus,

>>>pKa for trial 1 = 5.67

Hence, Ka = 10 -pka = 10-5.57

Ka = 2.14 x 10-6

>>>pKa for trial 2 = 5.53

Hence, Ka = 10 -pka = 10-5.53

Ka = 2.95 x 10-6

2) The accepted value of Ka and pka fior acetic acid are:

pKa = 4.74

Ka = 1.8 x 10-5

3) At half equivalence point, the concenmtrations of CH3COOH and its anion CH3COO- is equal.

Hence, according to Hendersen- Haseelbalch equation,

pH = pKa + log [ CH3COO-] / [CH3COOH]

pH = pka + 0

pH = pKa

4) Indicators are the chemical agents which changes its color even in slight change in pH. Since, acetic acid is a weak acid and it forms buffer on its dissociation. This will causes a slight change in pH on addition of base or acid. Therefore, indicator is more suitable for detection by changing its color.

Add a comment
Know the answer?
Add Answer to:
DULLOH HILL UCUREI LULUS solution in the beaker. 13. When you have finished the testing, dispose of the reaction mi...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • Follow up questions 01. Find the accepted values for the pKa and Ka of acetic acid....

    Follow up questions 01. Find the accepted values for the pKa and Ka of acetic acid. How well do the accepted values compare with your calculated values? Explain. Lab 7 Determining Ka by the Half-Titration of a Weak Acid 1. Data table Titration Results NaOH volume at equivalence point NaOH volume at half equivalence point pH at the equivalence point pH at half equivalence point pKa of acetic acid Ka of acetic acid Trial 1 22.72 11.36 7.63 Trial2 23.26...

  • 1. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid,...

    1. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 2. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid that has been titrated to its endpoint using NaOH, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 3. What pH did you...

  • How do I calculate the ionization constant for acetic acid from the measured pH of the acedic aci...

    How do I calculate the ionization constant for acetic acid from the measured pH of the acedic acid samples? Data and Calculations 1. Measurement of pH and fitration of acetfic acid solution Concentration of standardized NaOH titrant Mass concentration of acetic acid-aao Trial 3 Trial 2 Trial 1 Measured pht of the acetic acid solution Mass of acetic acid solution taken for titration. Initial buret reading of NaOH titrant Final buret reading of NaOH titrant Net volume of NaOH Millimoles...

  • millimoles of NaOH titrant Chemical Equilibria: K, of a Weak Monoprotic Acid Report Form Name: Partner's...

    millimoles of NaOH titrant Chemical Equilibria: K, of a Weak Monoprotic Acid Report Form Name: Partner's Name: (if any) Lab Section MWITTHM-TH (Circle) Data and Calculations 1. Measurement of pH and titration of acetic acid solution Concentration of standardized NaOH titrant 0.1054 Mass concentration of acetic acid 2.40 - mol/L Trial 3 Measured pH of the acetic acid solution Mass of acetic acid solution taken for titration Trial 1 3.09 20.16 0 11.4 Trial 2 3.32 30.06 Initial buret reading...

  • I don't understand what calculations I would have made to create the buffer solution from Part...

    I don't understand what calculations I would have made to create the buffer solution from Part D of the lab. I understood the procedures I took to create the solution but when the report asks to show the calculations used to prepare the buffer solution I am not sure other than mixing the volumes indicated in the procedures section. Thank you pH of Butter Assigned by Instructor 5.12. Measured pH of Assigned B r .9 (Read the procedural Show the...

  • can someone help me answer these 5 questions and figire this graph out please? Acid-Base Titration...

    can someone help me answer these 5 questions and figire this graph out please? Acid-Base Titration of a Weak Acid with a Strong Base: Determination of K. Introduction: You will be titrating a solution of a weak acid with 0.100 M NaOH, while monitoring the reaction using a pH meter. Weak acids have characteristic acid-ionization constants, K. The purpose of this lab is to use the titration to determine the value of this constant for the weak acid called “benzoic...

  • 22. Acetic acid, CH,COOH, is placed in an Erlenmeyer flask and titrated with NaOH solution. Sketch...

    22. Acetic acid, CH,COOH, is placed in an Erlenmeyer flask and titrated with NaOH solution. Sketch a titration curve. Your graph should have the value of 7 indicated on the pH-axis. Show the following on the graph. a. Equivalence point b. Half-equivalence point c· The region with the maximum buffering effect d. The point where pH-pKa e. The point where [CH,COOH [CH COO] f. The region where pH is controlled by the excess of a strong base

  • ALT CHEM 125 Name Determining the Ksp of Calcium Hydroxide Calcium hydroxide is an ionie solid...

    ALT CHEM 125 Name Determining the Ksp of Calcium Hydroxide Calcium hydroxide is an ionie solid that is sparingly soluble in water. A saturated, aqueous, solution of Ca(OH), is represented in equation form as shown below. Ca(OH)2 (5) --- Ca' (aq) + 2OH(aq) The solubility product expression describes, in mathematical terms, the equilibrium that is established between the solid substance and its dissolved ions in an aqueous system. The equilibrium expression for calcium hydroxide is shown below. Kp - [Ca][OHT...

  • the concentration is .1000 M for NaOH. you cN disregard the second column. but there is...

    the concentration is .1000 M for NaOH. you cN disregard the second column. but there is no further information. equivalence point is 22.95. i dont have mL NaOH this is all i have DATA TABLE sor CHCOOH Trial Volume CHCOOH (ml) [NTOH (M) Equivalence point Md point (ML) (ml) NE 100CM 1000M a.so DATA ANALYSIS moles -(CX) 1. Calculate the number of moles of NaOH used in the reaction with the acetic acid (CH.COOH) solution . OOON NaoH 2. How...

  • DATA AND CALCULATIONS Time at equivalence point (s) Time of color Trial *Equation for acid-base reaction...

    DATA AND CALCULATIONS Time at equivalence point (s) Time of color Trial *Equation for acid-base reaction change (s) NaOH+HCI - 21 0s 1 250.5 NaOH+ HC2H3O2- 2 8l.55 99s 3 NH3+ HCl- 930s 4 NH3 + HC2H3O2- 90.55 81.Os Complete the reactions above. Attach copies of all four graphs to this report. 1. 2. Examine the time data for each of the Trials 1- -4. In which trial(s) did the indicator change color at about the same time as the...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT