The following titration curve shows the titration of triethylamine (C2H5]3N with hydrochloric acid. Which net ionic reaction explains the pH of the solution after 60 mL of titrantis added?1210PH50mL of HCI10307090110O H,O(1) --> H*(aq) + OH (aq)(C,H5)3N(aq) + H*(aq) --> (C,H5)3NH* (aq)(C,H5)3N(aq) + H3O*(aq) <=> (C,H5)3NH*(aq) + OH (aq)(C,H5)3NH (aq) + H2O(1) <=> (C,H5)3N(aq) + H3O*(aq)(C2H5)3N(aq) + H20(1) <=> OH (aq) + (C2H5)3NH*(aq)O O O O O

Answered: The following titration curve shows the…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.38QAP

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Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?
C10H12NO4N is a weak base and has a Kb of 1.58x10-10. One, 0.650g, is dissolved in 235mL of distilled water. a. What is the initial concentration, in units of molarity, of the zalcitabine? b. Write an expression for Kb for zalcitabine. c. What are the equilibrium concentrations of the products and reactant? d. What is the pH, pOH, and % ionization of this weak base?
A biochemist needs 750 mL of an acetic acid–sodiumacetate buffer with pH 4.50. Solid sodium acetate(CH3COONa) and glacial acetic acid (CH3COOH) areavailable. Glacial acetic acid is 99% CH3COOH by massand has a density of 1.05 g/mL. If the buffer is to be 0.15 Min CH3COOH, how many grams of CH3COONa and howmany milliliters of glacial acetic acid must be used?
Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2—Tris, or THAM] is a weak base frequently used to prepare buffers in biochemistry. Its Kb is 1.2 × 10−6 and pKb is 5.92. The corresponding pKa is 8.08, which is near the pH of the physiological buffers, and so it exhibits good buffering capacity at physiological pH. What weight of THAM must be taken with 100 mL of 0.50 M HCl to prepare 1 L of a pH 7.40 buffer?
The acid–base indicator bromcresol green is a weak acid.The yellow acid and blue base forms of the indicator arepresent in equal concentrations in a solution when the pHis 4.68. What is the pKa for bromcresol green?
A 50.00-mL sample of a 1.00 M solution of the diprotic acid H2A (Ka1 = 1.0 × 10–6 and Ka2 = 1.0 × 10–10) is titrated with 2.00 M NaOH. How many mL of 2.00 M NaOH must be added to reach a pH of 12? Give answer in 15 min.
The base ionization constant of ethylamine (C2H5NH2) in aqueous solution is Kb= 6.41 × 10-4 at 25°C. Calculate the pH for the titration of 40.00 mL of a 0.1000 M solution of ethylamine with 0.1000 M HCl at the following volumes of added HCl: 0, 5.00, 20.00, 39.90, 40.00, 40.10, and 50.00 mL.
A primary amine R-NH2 has pKb = 5.65 at 25°C. A buffer solution is made by adding 66.0 mL of 1.55 mol L-1 HCl(aq) to 66.0 mL of 3.95 molL-1 R-NH2(aq). What is the pH of the buffer solution at 25°C?
Consider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is: HC7H5O2 (aq) + H2O (l) ↔ C7H5O2- (aq) + H3O+ (aq) A 25.00 mL sample of a solution of benzoic acid, concentration unknown, is titrated with 0.0500M NaOH solution. A plot of the titration is shown below. 1. what is the pKa (approximately) of benzoic acid? Its Ka? 2. on the plot, indicate the buffering region of the titration 3. From the pH at the equivalence point, estimate the pKb of benzoate ion (conjugate base to benzoic acid)______________[Remember, at the equivalence point, C7H5O2- (aq) + H2O (l) ↔ HC7H5O2 (aq) + OH- (aq) ]
MUST ANSWER BOYH SUBPARTS A AND B A 1.161g sample of pure maleic acid (H2M, 116.1 g/mol) with Ka1 and Ka2 values of 1.42 × 10-2 and 8.57 ×10-7, respectively, was contained in a 100.0 mL solution with a pH of 5.0. In solution, maleic acid can dissociate into HM- and M2- species. The three species (H2M, HM- and M2-) exist in the solution at varying concentrations that depend on the pH of the solution. a) Calculate the values of α1 (alpha 1) and α3 (alpha 3). b) Calculate the concentration of HM- in the above solution.
Given the following experimental data, calculate the molarity and the pKa of the acid analyte (HA) in the titration, with the following data: HA + NaOH à NaA + H2O. -A pH reading of 3.65 is obtained when 13.0 mL of 0.413 M NaOH is added to the 25.0 mL analyte. -The endpoint of the titration is achieved when 31.25 mL of NaOH have been added. Show all your calculations.

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