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(a)
Interpretation:
The name of the carboxylate ion that is formed from acetic acid has to be given.
Concept Introduction:
The name of the
Carboxylate ion is the negative ion which is formed when one or more acidic protons are lost from carboxylic acid.
Carboxylate ions are named from the parent acid by replacing the suffix “-ic acid” with “-ate”.
(b)
Interpretation:
The name of the carboxylate ion that is formed from benzoic acid has to be given.
Concept Introduction:
The name of the carboxylic acid itself implies that it is acidic. Addition of carboxylic acid to water results in ionization. Hydrogen ion transfer occurs from carboxylic acid to water and hydronium ion is formed. Carboxylate ion is also formed due to the loss of hydrogen ion from carboxylic acid.
Carboxylate ion is the negative ion which is formed when one or more acidic protons are lost from carboxylic acid.
Carboxylate ions are named from the parent acid by replacing the suffix “-ic acid” with “-ate”.
(c)
Interpretation:
The name of the carboxylate ion that is formed from propanoic acid has to be given.
Concept Introduction:
The name of the carboxylic acid itself implies that it is acidic. Addition of carboxylic acid to water results in ionization. Hydrogen ion transfer occurs from carboxylic acid to water and hydronium ion is formed. Carboxylate ion is also formed due to the loss of hydrogen ion from carboxylic acid.
Carboxylate ion is the negative ion which is formed when one or more acidic protons are lost from carboxylic acid.
Carboxylate ions are named from the parent acid by replacing the suffix “-ic acid” with “-ate”.
(d)
Interpretation:
The name of the carboxylate ion that is formed from glutaric acid has to be given.
Concept Introduction:
The name of the carboxylic acid itself implies that it is acidic. Addition of carboxylic acid to water results in ionization. Hydrogen ion transfer occurs from carboxylic acid to water and hydronium ion is formed. Carboxylate ion is also formed due to the loss of hydrogen ion from carboxylic acid.
Carboxylate ion is the negative ion which is formed when one or more acidic protons are lost from carboxylic acid.
Carboxylate ions are named from the parent acid by replacing the suffix “-ic acid” with “-ate”.
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Chapter 16 Solutions
EBK GENERAL, ORGANIC, AND BIOLOGICAL CH
- Consider a buffer solution of acetate. The volume is 500 ml, the concentration is 200 mM, and the pH is 5.0. a. How many total moles of acetate plus acetic acid are present in the solution? Express answer as x.y with one digit before and one after the decimal place. b. What is the ratio of acetate ions (Ac-) to acetic acid ions (HAc) in the buffer solution (pH 5.0) if the pka is 4.76? Express the answer as x.yz with one digit before and two after the decimal place. c. How many moles of acetate are present in the solution? Express your answer to one decimal place. d. How many moles of acetic acid are present in the solution? Express your answer to one decimal place.arrow_forwardGlutamic acid (1one of the 20 amino acids) has a side- chain carboxyl group (COOH, pKa = 4.3) as shown in Figures 4.7 and 4.8 a. Write the chemical equation for the dissociation of the side chain COOH. Label the weak acid and the conjugate base. b. The Henderson-Hasselbalch Equation (shown below) can be used to determine the ionization status of a weak acid: pH = pKa + log [base] Use the Henderson Hasselbalch equation to determine whether the glutamic acid side chain [acid] • carboxyl group is protonated or deprotonated at physiological pH.arrow_forwardConsider these compounds: A. PbBr, B. MnS C. Ag,CO3 D. AIPO, Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine that magnesium fluoride is more soluble than and magnesium fluoride is less soluble than| It is not possible to determine whether magnesium fluoride is more or less soluble than by simply comparing Kgp values.arrow_forward
- Draw the L enantiomer in a Fischer projection for each amino acid; identify the amino acid as neutral, acidic, or basic. Give the three-letter sign [3], and the one-letter symbol [4].arginine a. arginine b. arginine c. a. glutamic acid b. glutamic acid c. glutamic acidtyrosine b. valine c. argininearrow_forwardb) Determine which ionization state corresponds to aspartic acid (shown below) at pH 1, 7, and 10 by selecting the most suitable answer from the statements i-iv. The pK of the amine, carboxylic acid, and side chain of aspartic acid are 9.6, 1.88 and 3.65, respectively. ОН ÓH ÑH2 i) the amine is charged; the carboxylic acids are neutral. ii) the amine and carboxylic acids are all charged. iii) the amine is neutral, and the carboxylic acids are charged. iv) the amine and the carboxylic acids are all neutral. pH Statement (i, ii, iii, or iv) 1 7 10 %3Darrow_forwardThe analgesic phenacetin is synthesized by treating 4- ethoxyaniline with acetic anhydride. a. Which of the following is the structure of 4- ethoxyaniline? OCH₂CH3 NH₂ OCH₂CH3 NH₂ OCH₂CH3arrow_forward
- Refer to the following titration curve below: 13 12 11 10 9 7 6 5 4 3 4 6 8 10 12 14 16 18 20 22 24 26 28 30 Volume of Titrant / mL - Unknown Acid 0.10 mol/L - titrant = NaOH 0.1 mol/L At ph 10.0, which form of histidine is most abundant? His2+ His- His° His+arrow_forwardDefine the following terms: a. alkylating agents b. base analogue c. nonalkylating agent d. intercalating agent e. ethidium bromidearrow_forwardThe structure of ephedrine isgiven, The pKa for ephedrine is 9.6. Answer the following questions about aqueous solutions of ephedrine. a. Draw the structure of the principal chemical form of ephedrine that results when it isdissolved in water.b. Draw the structure of the principal chemical form of ephedrine that results when it is dissolved in a buffer at a physiologically relevant pH of 7.4.c. Calculate the pH that results when 0.3 mole of ephedrine is dissolve in 2.0 L of 0.05 M perchloric acid (HClO4).arrow_forward
- A 100 ml solution of 0.1 M amino acid (AA) at ph 1.0 was titrated with NaOH solution. The pH was monitored, and the results were plotted on the graph. The keypoints in the titration are designated I to VII. What is the possible identity of the amino acid? What is the isoelectric point of AA? what is the pKa corresponding to the dissociation of the alpha carboxylic group? Region/point where AA is predominantly present as a (-1) charged species? The effective buffering range for the amino acid in the acidic region? Region/point where the solution has 50:50 percent mixture of the (0) and (-1) speciesarrow_forwardDraw the following: A. a phosphatidylcholine with two oleic acid as the fatty acids B. a phosphatidylethanolamine with two palmitic acid as the fatty acids C. adenine-thymine base pair (show hydrogen bonds via dashed line) D. guanine-cytosine base pair (show hydrogen bonds via dashed line)arrow_forwardDetermine the weight/volume of the chemicals needed to prepare the following solutions: a) 100 ml of 0.9% (w/v) saline (NaCl) b) 30 ml of 50% glycerol (v/v) c) Electrophoresis requires TAE, which is a specific mixture of Tris base, acetic acid, and EDTA. TAE is normally made as a 50X concentrated stock. Provide a recipe to make 40 ml of 50X TAE. The recipe for one liter of 50X TAE is as follows: 242g Tris base, 57.1 ml glacial acetic acid, 100 ml 0.5 M EDTAarrow_forward
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