Calculating the pH at equivalence of a titration0/5IzabellaA chemist titrates 80.0 mL of a 0.7536M dimethylamine ((CH3)2NH) solution with 0.0940M HBr solution at 25 °C. Calculate the pH at equivalence. ThepK of dimethylamine is 3.27.bRound 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 HBr solution added.pH=☑ك18ArB?

pH = 5.90Explanation:Given: V(CH3)2NH=80.0mL;[(CH3)2NH]=0.7536M;[HBr]=0.0940M;pKb=3.27at the…

Answered: Calculating the pH at equivalence of a…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 55P

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Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
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).
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
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.)
Which of the acid-base indicators discussed in this chapter would be suitable for the titration of (a) HNO3 with KOH. (b) KOH with acetic acid. (c) HCl with NH3. (d) KOH with HNO2. Explain your answers.
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
A 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.
A sample of 50.00 mL of 0.1000 M aqueous solution of benzoic acid (C6H5COOH) K = 6.46 x 10- , is titrated with a 0.1000 M NaOH solution. Calculate the pH at the following points: 5i) after 0 NaOH has been added. Choose from answers A-D. a ii) after 5.00 mL of NaOH has been added. Choose from answers E-H. iii) after 25.00 mL of NaOH has been added. Choose from answers I-L. iv) after 49.90 mL of NaOH has been added. Choose from answers M-P. v) after 50.00 mL of NaOH has been added. Choose from answers Q-T. vi) after 55.00 mL of NaOH has been added. Choose from answers U-X.
A chemist titrates 130.0mL of a 0.6404M acetic acid (HCH3CO2) solution with 0.7306M NaOH solution at 25°C. Calculate the pH at equivalence. The pKa of acetic acid is 4.76. 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 NaOH solution added.
Consider exactly one litre of a hydrofluoric acid buffer solution, containing 0.800 M HF and 0.528 M F-1. Determine the pH of the buffer solution.- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations- Ka for hydrofluoric acid is 6.6 × 10−42. Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. mL of a 1.00 × 10−2 M HCℓ solution is added to it. You must indicate all the relevant reaction equations in your working.

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