slecula... 18.3 Gibbs Free E... Calculating the pH of a weak base titrated with a strong acid 18.3 Gibbs Free E... pH- 0 5.3 Enthalpies of... X 18.5 Gibbs Free E... An analytical chemist is titrating 207.8 ml. of a 0.3200M solution of diethylamine ((C₂H₂)₂NH) with a 0.2900M solution of HCIO. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 269.8 mL of the HCIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HCIO, solution added. Round your answer to 2 decimal places. Reading Schedule Lara V M

slecula... 18.3 Gibbs Free E... Calculating the pH of a weak base titrated with a strong acid 18.3 Gibbs Free E... pH- 0 5.3 Enthalpies of... X 18.5 Gibbs Free E... An analytical chemist is titrating 207.8 ml. of a 0.3200M solution of diethylamine ((C₂H₂)₂NH) with a 0.2900M solution of HCIO. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 269.8 mL of the HCIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HCIO, solution added. Round your answer to 2 decimal places. Reading Schedule Lara V M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 130CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
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.
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
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).
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
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.)
Calculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
2. Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2-9.3? A) CH;COONa / CH;COOH (K, = 1.8 x 10-5) NH3 / NHẠCI (K, = 5.6 x 10-10) B) C) NaOCI / HOCI (Ka = 3.2 x 10-8) D) NaNO2 / HNO2 (Kg = 4.5 x 104)
Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 59.5 mL of 0.436 M nitrous acid (K₂ = 4.5x10-4) by 0.436 M NaOH at the following points. (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.3 mL of NaOH
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