12) To determine the titration acidity of a bottled cherry juice, 0.01 L of cherry juice was transferred to a flask and 0.09 L distilled water was added. For the titration, 28.1 mL of 0.1 N NaOH was consumed. Calculate the titration acidity in terms of the dominant organic acid (g/L) in the cherry juice (Equivalent values of some organic acids; malic acid: 67, citric acid: 64, tartaric acid: 75). a) 20.13 b) 24.58 d) 32.67 e) 17.940 ( 18.83

12) To determine the titration acidity of a bottled cherry juice, 0.01 L of cherry juice was transferred to a flask and 0.09 L distilled water was added. For the titration, 28.1 mL of 0.1 N NaOH was consumed. Calculate the titration acidity in terms of the dominant organic acid (g/L) in the cherry juice (Equivalent values of some organic acids; malic acid: 67, citric acid: 64, tartaric acid: 75). a) 20.13 b) 24.58 d) 32.67 e) 17.940 ( 18.83

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.102QE

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The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?
You prepared 500 mL buffer solution that contains 0.50 moles monoprotic weak acid (HA) and 0.30 moles conjugate base (NaA). The solution has a pH of 4.20. (a) What is the Kp of the conjugate base, NaA? (b) What is the pH of the buffer solution after adding 400 mL of 0.30 M H,SO4? pH = pKa – log(THA), [A*]
Consider the titration of 25.0 mL of 0.125 M acetic acid (CH, COOH, pKa = 4.75) with 0.102 M NaOH. CH, COОН(aq)+NaOH(aq) — СH, СОО" (аq) + H,О1) + Na*(aq) Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.102 M NaOH is added. pH = Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.
A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).
A 50.00-mL sample of white wine required 24.57 mL of 0.03291M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated.)
4) A highly toxic hydrogen cyanide (HCN) is a weak acid. A chemical engineer plans to determine pH of a 50 mL sample of HCN (0.10 M) in a titration process. To this end, she used 0.20 M NaOH as a titrant in varying volumes. Calculate the pH of the solution at the following points: (Ka for HCN=6.2×10-¹0) (a) Before addition of NaOH (initial pH), (b) After 10.00 mL of titrant addition, (c) After 25.00 mL of titrant addition, (d) After 50.00 mL of titrant addition.
Propanoic acid, CH₂CH₂COOH, is a weak monoprotic acid that is used to inhibit mould formation in bread. A student prepared a 0.10 mol/L solution of propanoic acid and found that the pH was 2.96. What is the acid dissociation constant for propanoic acid? [Hint: Setup an I.C.E. table] CH3CH₂COOH (aq) Ka for propanoic acid is: ←CH3CH₂COO (aq) + H (aq)
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Enter your answer in the provided box. A buffer solution is prepared in such a way that the concentration of propanoic acid is 5.55 × 10¬1 M and the concentration of sodium propanoate is 5.90 × 10~2 M. If the buffer equilibrium is described by CH3COOH(aq) + H2O(1) =H3O*(aq) + C2HgCOO¯(aq) propanoic acid propanoate ion with K=1.34 x 105, calculate the pH of the solution. pH =
Petanoic (or valeric) acid is a weak organic acid with an unpleasant odour. Like other small carboxylic acids, it is used to make pleasant smelling esters that are used in perfumes, cosmetics, and food additives. Completed Part D In Part B, a 20.00 mL aliquot of a 0.195 mol L-1 pentanoic acid solution was titrated to its equivalence point with 19.7 mL of 0.198 mol L- 1 NaOH solution. At the equivalence point, all of the weak acid, pentanoic acid, is converted to its weak conjugate base, pentanoate. In part A, the Ka for pentanoic acid was determined to be 1.48×10-5. What is the pH at this equivalence point? 5.089 6.997 pentanoic acid 9.170 4.830 The pka of pentanoic acid is 4.830. 8.911
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