Question 11 A weak base (Ka = 1.585 x 10-8, intrinsic solubility = 0.0002M) prepared at a concentration of 0.01M, in pH 7.4 buffer, will contain precipitates. True False Question 12 A weak acid with a pKa of 7.2 and intrinsic solubility of 0.002M was prepared at a concentration of 0.05M. In which of the following buffers will the preparation be completely soluble? Borate buffer pH 9 Phosphate buffer pH 8 Acetate buffer, pH 5 Question 13 In the Noyes-Whitney equation, D refers to which of the following? Dissolution rate Dissolution rate constant O Diffusion Coefficient Diffusant

Question 11 A weak base (Ka = 1.585 x 10-8, intrinsic solubility = 0.0002M) prepared at a concentration of 0.01M, in pH 7.4 buffer, will contain precipitates. True False Question 12 A weak acid with a pKa of 7.2 and intrinsic solubility of 0.002M was prepared at a concentration of 0.05M. In which of the following buffers will the preparation be completely soluble? Borate buffer pH 9 Phosphate buffer pH 8 Acetate buffer, pH 5 Question 13 In the Noyes-Whitney equation, D refers to which of the following? Dissolution rate Dissolution rate constant O Diffusion Coefficient Diffusant

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.84QE: Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink...

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(a) Calculate the pH of 1.00 x 10-2 M acetic acid solution. Ka for acetic acid is 1.75 x 10-5. (b) Sketch a titration curve for a 50.0 mL of 0.01M Sr2+ solution, buffered at pH 11 when 0.0,10.0, 24.0, 25.0, 26.0, 30.0, and 40.0 mL of 0.02 M EDTA are added. Given the KSrY2- is 4.3X108 and α4 is 0.85.
Question 2.5 select the most suitable indicator for the titration of 0.1 M aqueous sodium acetate with 0.1M HCl. Data: Р K₂ (sodium acetate ) = 9.26 colour change range (pH musts) →4.0-5.8 a) Bromacresol green. (b) 2,4-Dinitrophenol → 2.5-3.5 (c) Phenol red d) Thymol blue 6.3-8.0 8.0-10.9
A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 ml ot a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONA). [Ka= 1.8 x 10-1 What is the new concentration of the conjugate base, CH3COO after buffering? 0.3385 0.2434 0.1172 0.2269 0.4287
(5e) Which two of the following compounds would you make a buffer of pH = 12.5. H3PO4 (MM=98.00 g/mol), NaH2PO4 (MM=119.98 g/mol), NazHPO4 (MM=141.96 g/mol), and Na3PO4 (MM = 163.94 g/mol)? [For H3PO4: pK; = 2.148; pKz=7.199; pK3=12.15]
5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (K, = 5.2 x 10), with 0.1000 M HCl solution after the following additions of titrant. %3D (a) 10.00 mL: pH =9.72 (b) 20.70 mL: pH =|8.25 (c) 28.00 mL: pH =|10.17 %3D
A 270.00 mL solution of 0.00150 M AB4 is added to a 380.00 mL solution of 0.00250 M C3D4. What is pQsp for A3D4?
The Ką of Benzoic acid (C6H5COOH) is 6.3 x 10-5. A 0.72 M C6H5COOH of 40.0 mL is titrated with 0.48 M NAOH. Which of the following is correct for the following two processes? (1) After add resulting solution. ml of N2OH into the above 0.72 M C6H5COOH of 40.0 mL, we have [ C6H5COOH ] = [ C6HSCO0" ] in the (2) After add the resulting solution. ml of NaOH into the above 0.72 M CGH5COOH of 40.0 mL, we have [ CgHgCOOH ] = [OH" ] in O a. The answer for (1) is 40.0 ml. The answer for (2) is 20.0 ml. O b. The answer for (1) is 20.0 ml. The answer for (2) is 40.0 ml. O. The answer for (1) is 30.0 ml. The answer for (2) is 60.0 ml. d. The answer for (1) is 60.0 ml. The answer for (2) is 30.0 ml. O e. None of the above is correct.
A 25.0mL mixture solution contains NaNO3 and KIO4, titrated against 0.02M Na2S2O3. The volume of titrants is 18.2 mL, the concentration of KIO4 is:a) 3.64 × 10-4 b) 9.1 × 10-5c) 1.82 × 10-3 d) 2.35e) 3.64 × 10-4
Calculate the pH at the equivalence point in titrating 0.028 M solutions of each of the following with 0.015 M NaOH. (a) perchloric acid (HCIO4) pH = (b) benzoic acid (HC7H502), Ka = 6.3e-05 pH = (c) hydrazoic acid (HN3), Ka = 1.9e- 05 %3D
3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124
10)25.0 mL of a 0.15 M solution of the diprotic base EDA is titrated with 0.30 M HNO3. What will be the approximate pH when 25.0 mL of the acid has been added? EDA: pKsi pKs2 Ve (0,3) = 0.15(25s) Ve - 12.5 mL 4.07 7.15 COH-J = pka +log (ANHA]) -log (AGHA]) %3D V2 ( 9.93+ 6.8S) = 8.39=H %3D