Answered: 3. On the following titration curve…

3. On the following titration curve label the equivalence point and the pka(s). PH 12.0 10.0 8.0 6.0 4.0 2.0 0.0 0.0 Titration Curve for an Amino Acid 0.5 1.0 1.5 2.0 OH (equivalents) 2.5 3.0

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section18.4: Neutralization

Problem 50SSC

See similar textbooks

Similar questions

The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
Explain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.
Methyl red has the following structure: It undergoes a color change from red to yellow as a solution gets more basic. Calculate an approximate pH range for which methyl red is useful. What is the color change and the pH at the color change when a weak acid is titrated with a strong base using methyl red as an indicator? What is the color change and the pH at the color change when a weak base is titrated with a strong acid using methyl red as an indicator? For which of these two types of titrations is methyl red a possible indicator?
Each of the solutions in the table has the same volume and the same concentration, 0.1 M. Which solution requires the greatest volume of 0.1-M NaOH to titrate to the equivalence point? Explain your answer.
A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
HEPES is considered a good buffer developed by a scientist of the same name it’s chemical properties are not dependent upon concentration and temperature changes. the PKA of HEPES is 7.55. For a 0.100 molar HEPES buffer at a pH of 6.55 what is the concentration of the protonated form of the buffer a.0.2 b. 0.1 c. 0.009 d. 0.091
The titration curve attached was obtained from the titration of a 0.225 g sample of a solid acid with 0.100 M KOH. How many moles of acid are present? 14 12 10 8 6. 4. 2 10 15 20 25 30 Volume of KOH added (mL) A. 0.000800 moles Acid B. 0,00160 moles Acid O C. 0,00110 moles Acid D. 0.00255 moles Acid
What volume (mL) of 0.2173M NaOH is required to titrate 50.00mL of 0.2980M HCI ?In the titration of 50.00mL of 0.2980M HCl. 71.93mL of 0.2173M NaOH was required to reach the phenolphthalien endpoint. Calculate the percent error between the predicted amount and the experimental amount. What does this tell you about the concentration of the NaOH? This is based on your answers to questions 1 and 2. Question 3 options: The concentration of the NaOH is 0.2173M. The concentration of the NaOH is stronger that 0.2173M. Nothing new The concentration of the NaOH is weaker than 0.2173M. Please answer fast i give upvote.
Related to the titration of 30.00 mL of a 0.0700 M acetic acid solution with 0.0900 M KOH: What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration (in mL)? How many mmol of the salt are present at the equivalence point? (ANALYTICAL AMOUNT, NOT EQUILIBRIUM AMOUNT) What is the volume of the solution at the equivalence point (in mL)? What is the molar concentration of the salt at the equivalence point? (ANALYTICAL CONCENTRATION, NOT EQUILIBRIUM CONCENTRATION) What is the pOH at the equivalence point? How many mL of KOH have been added at the half-equivalence point? What is the pH at the half-equivalence point?
2. Below is a titration curve generated by a similar titration to the ones simulated, Vinegar Titration Curve 14.00 13.00 12.00 11.00 10.00 9.00 8.00 * 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 Volume NaOH (mL) We can use this curve to estimate the pka of our weak acid by what is called the "half equivalence point method". The equivalence point is the middle of the steepest part of this graph. Estimate the volume of NaOH added to the titration at that point by using a rule or other straight edge to follow that point down to the x-axis. Divide that volume by 2 (half the equivalence point) and estimate the pH at that volume of NaOH using your straight edge again. pKa = pH at the half equivalence point. What do you estimate the pka to be? 3. The pka of acetic acid is 4.76. Calculate percent error between the true value and your estimated value from question 2.
When choosing an indicator for the titration of a weak acid with strong base, which of the following requirement should be met? a. pKa of the indicator should be close to 7.0 b. pKa of the indicator should be close to the pH at the equivalence point c. pKa of the indicator should be close to the pKa of the weak acid d. the concentration of the indicator should be large so that we can easily observe color change