The pH of amino acid is adjusted to 1.5 prior to titration to make sure that the amino acid has a netnegative charge. write true if the statement is correct, otherwise, change the underlined word/phrase to make it correct. do not useabbreviations please answer all|

There are 20 naturally occurring amino acid. They contain one carboxylic group one amino group, an…

Answered: The pH of amino acid is adjusted to 1.5…

Science

Chemistry

The pH of amino acid is adjusted to 1.5 prior to titration to make sure that the amino acid has a net negative charge.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Ka for ethanoic acid is 1.7*10^-5 moldm-3. Show by calculation that the initial pH in experiment B is 4.8.
What is the general composition of a buffer and in your own words explain why it resists change in PH.
An analytical chemist is titrating 123.0 mL of a 0.5600M solution of diethylamine ((C₂H₂), NH) with a 0.5300M solution of HNO3. The pK, of diethylamine 2 is 2.89. Calculate the pH of the base solution after the chemist has added 111.5 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.
A weak diprotic acid is titrated past the end points with a strong base. Identify which of the following statements is true. O pH at end point 1 and pH at end point 2 are numerically smaller than 7. O the volume of titrant added to reach end point 1 will be the same additional volume of titrant as between end point 1 and end point 2. O the volume of titrant added to reach end point 1 will be twice the additional volume of titrant as between end point 1 and end point 2. O the volume of titrant added to reach end point 1 will be half the additional volume of titrant as between end point 1 and end point 2. O pH at end point 1 and pH at end point 2 ak numerically larger than 7.
A chemist titrates 230.0 mL of a 0.1072M ethylamine (C,H,NH,) solution with 0.5758M HCI solution at 25 °C. Calculate the pH at equivalence. The p K, of ethylamine is 3.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = Explanation Check 2021 McGraw-Hill Education All Rights sved T Le/Py 18 MacBook Air esc F7 FI F2 F3 F4 *
What are the examples of Qualitative Chemistry?
theoretically, the equivalence point and end point of a titration should be the same. Describe four factors that could be responsible for the difference between these two in an actual titration
In Part A, a 15.00 mL aliquot of a 0.155 mol L-1 3-methylbutanoic acid solution was titrated to its equivalence point with 11.7 mL of 0.198 molL-1 NaOH solution. At the equivalence point, all of the weak acid, 3-methylbutanoic acid, is converted to its weak conjugate base, 3-methylbutanoate. What is the pH at this equivalence point? 6.957 4.770 8.855 5.145 O 9.230
An unknown solution is blue with indigo carmine and blue with thymolphthalein. From that information, predict the approximate pH range of the unknown solution, then determine the colour of the following indicators in that solution. Indicator Colour alizarin yellow R yellow/red/orange phenolphthalein colourless/pink thymol blue yellow/red/orange/green/blue
Use the following information as a guide to help answer the next three questions. Your answer MUST be in the same format. Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between .0 and 7.6 6. Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Using the method outlined above in the example of bromothymol blue, indicate what the colours of the indicators tell us about the pH approximation of the solution. Values and wording are very important, so be precise. Be sure to word your pH approximation as outlined in the example. Indicator Colour pH approximation methyl red orange Indicator Colour pH approximation phenolphthalein colourless Indicator Colour pH approximation phenol red red
An analytical chemist is titrating 99.1mL of a 0.7900M solution of aniline C6H5NH2 with a 0.2500M solution of HNO3 . The pKb of aniline is 9.37 . Calculate the pH of the base solution after the chemist has added 39.3mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.
Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between 6.0 and 7.6 Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Indicator Colour pH approximation orange IV orange Indicator Colour pH approximation thymol blue red Indicator Colour pH approximation alizarin yellow R red