Please don't provide handwritten solution .... Consider the titration of 20.00 mL of 0.400 Mbenzoic acid (C6H5COOH) with 0.600 M NaOH.Determine the pH of the solution after theaddition of 7.03 mL of the NaOH. You can use"HA" to represent the benzoic acid in thereaction equation.Notes: K₂ of benzoic acid = 6.5 x 10-5

Benzoic acid (HA) is a weak organic acid, when reacted with a strong base (OH-) from NaOH yields the…

Answered: Consider the titration of 20.00 mL of…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 7P

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
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.)
Consider the titration of 20.00 mL of 0.400 M benzoic acid (C6H5COOH) with 0.600 M NaOH. Determine the pH of the solution after the addition of 7.03 mL of the NaOH. You can use "HA" to represent the benzoic acid in the reaction equation. Notes: K₂ of benzoic acid = 6.5 x 10-5
Malonic acid is a dicarboxylic acid with structure CH2(COOH)2 with Ka1 = 1.5 × 10-3 and Ka2 = 2.0 × 10-6. Consider the titration of 50.0 mL of 0.2 M disodium malonate (Na2CH2(COO)2) by 0.2 M HCl and answer the following questions. Calculate the pH after the following total volumes of HCl have been added.
The next 11 questions are related to the titration of 30.00 mL of a 0.1000 M acetic acid solution with 0.0800 M KOH. Assume that the temperature is 25 oC.What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration? How many mmol of acetate are present at the equivalence point? Report the analytical amount, not the equilibrium amount of acetate at the equivalence point. What is the total volume of the solution at the equivalence point?
How will you prepare a pH 4.50 acetic acid-acetate buffer such that when1.00 mL of 10 M NaOH is added to 100.00 mL of this buffer, the resulting pHwill be raised by exactly 1 pH unit? Show calculations for the concentrations(in 3 decimal places) of the components that must be present in the bufferas well as the volumes of 1 M acetic acid and 1 M sodium acetate that needto be mixed and diluted to 100.00 mL to prepare the buffer. (There is nospecific final buffer concentration required here. You can verify your answersby using the Virtual Lab).
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
A student is preparing to titrate 25.00 mL of 0.2 M NaOH. He has options to use among 3 weak monoprotic acid at same concentration, with different acid dissociation constants, WA1= 1 X 10-4, WA2= 1 X 10-5 , WA3= 1 X 10-8. Which is the best acid titrant you would recommend ?
8. You are titrating 50.0 mL of 0.200 M propanoic acid with 0.100 M NaOH. Use the data in the table to answer the questions. Name Propanoic acid Structure CH3CH2CO2H pka 4.874 Ka 1.34 × 10-5 a) Assuming that the equivalence point is considered 100% completion, calculate the pH at the following points: 0%, 10%, 50%, 90%, 100%, and 120%. b) Sketch the titration curve. c) What would be an ideal pKa for an indicator to use in this titration?
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Consider the titration of 20.00 mL of 0.400 M benzoic acid (C6H5COOH) with 0.600 M NaOH. Determine the pH of the solution after the addition of 7.03 mL of the NaOH. You can use "HA" to represent the benzoic acid in the reaction equation. Notes: K₂ of benzoic acid = 6.5 x 10-5