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…

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Chemistry

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ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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65 mL of 0.65 M benzoic acid (Ka = 6.4×10-5) is titrated by 0.05 M NaOH. 1)Calculate the pH of the acid solution before any titrant is added. 2)Calculate the pH after 795.9 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. 3)Calculate the pH after 845 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. 4)Calculate the pH after 1.58 x 10^3 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid.
A 50.0 mL aliquot of a 0.00100M solution of acetic acid (K, = 1.8 x 10-5) is titrated with 0.00993M NaOH. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration. Properties of Several Indicators Write the letter corresponding to your choice of indicator in the box
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O ACIDS AND BASES Calculating the pH of a buffer A solution is prepared at 25 °c that is initially 0.077M in trimethylamine ((CH3)3N), a weak base with K₁=7.4× 10-4, and 0.50M in trimethylammonium Calculate the pH of the solution. Round your answer chloride ((CH3), NHCI) to 2 decimal places. pH = 1/3 X
Determine the mass of solid NaCH,COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH;COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH,COOH is 1.8 x 10. NEXT > Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH;COOH(aq) + H2O(1) H,O (aq) CH;COO (aq) Initial (M) Change (M) Equilibrium (M)
When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?
You have 150 mL of 1 M ammonia solution (pKa=9.25). What volume of 1 M hydrochloric acid is needed to prepare buffer with pH=9.5?
Do not give answer in image and hand writing
The following table shows the values of ionization constants for a number of acids and bases at 25 °C: Formula Ka HC2H302 1.8x10-5 HCIO2 NH3 HCIO 1.1x10-2 2.9x10-8 Kb 1.76x10-5 For the best system, calculate the ratio of the masses of the buffer components required to make the buffer. Express your answer to two significant figures. PH = 7.30
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Observing the chart below, inform which curve represents the titration of a weak acid and which represents the titration of a strong acid. Both the acids are in the same concentration. Justify.

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