1. Tris(hydroxymethyl)aminomethane abbreviated as Tris or TRIŽMA is frequently used to make buffers in biochemistry laboratories. Tris has a Molecular weight 121.1 g/mol and its solution in water is basic with pH = 10.5. Describe in details how to prepare 1L of 0.5 M Tris buffer solution at pH 7.5. 2. If 2L of 0.05 M Tris-HCI buffer solution pH = 7.5 are required for an experiment on column chromatography. Describe in details how to prepare this buffer solution by diluting the buffer prepared in question # 1. 3. Describe in details how to prepare 10 ml of a 15% (v/v) glycerol solution containing Bovine Serum Albumin (BSA) (3 mg/ml). NH, HO-CH,- CH-OH OH

1. Tris(hydroxymethyl)aminomethane abbreviated as Tris or TRIŽMA is frequently used to make buffers in biochemistry laboratories. Tris has a Molecular weight 121.1 g/mol and its solution in water is basic with pH = 10.5. Describe in details how to prepare 1L of 0.5 M Tris buffer solution at pH 7.5. 2. If 2L of 0.05 M Tris-HCI buffer solution pH = 7.5 are required for an experiment on column chromatography. Describe in details how to prepare this buffer solution by diluting the buffer prepared in question # 1. 3. Describe in details how to prepare 10 ml of a 15% (v/v) glycerol solution containing Bovine Serum Albumin (BSA) (3 mg/ml). NH, HO-CH,- CH-OH OH

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

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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2. Determine the best answer on the follow:What buffer pH can be prepared from an arbitrary weak acid whose pKa is 7.20?a. pH 8.30b. pH 6.40c. pH 2.80d. pH 5.80 All salts are products of neutralization reactions between an acid and a base. Thus, all salts form a neutral solution when dissolved.a. Trueb. False
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Find the mass of sodium formate that must be dissolved in 230.0 cm^3 of a 2.0 M solution of formic acid to prepare a buffer solution with pH = 3.10.
3. How much volume of 0.1 M acetic acid should be added to 50 ml of 0.2 M sodium acetate solution if we want to prepare a buffer solution of pH= 4.91. Given pKa for acetic acid is 4.76.
7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?
1. all the aqueous solutions that are good buffer systems 2. a buffer solution is 0.421 m in hcn and 0.281 m in kcn, if Ka for Hcn is 4.0 * 10^-10. what is the PH of this buffer solution. b. a buffer solution is 0.495 m in h2s and 0.354 m in khs, if Ka1 for H2s is 1.0 * 10^-7. what is the PH of this buffer solution. c. a buffer solution is 0.455 m in NaHSO and 0.299 m in Na2SO3, if Ka for HSO3 is 6.4 * 10^-8. what is the PH of this buffer solution. 3. A 28.9 ml sample of a 0.385 m aqueous hydrocyanic acid solution is titrated with a 0.372 m aqueous sodium hydroxide solution. what is the ph at the start of the titration, before any sodium hydroxide has been added. b. A 31.9 ml sample of a 0.599 m aqueous hydrofluoric acid solution is titrated with a 0.242 m aqueous barium hydroxide solution. what is the ph after 15.8ml of base has been added. c. when a 23.8 ml sample of a 0.357 m aqueous acetic acid solution is titrated with a 0.459 m aqueous barium hydroxide solution. what is the ph…
What is the pH of a buffer solution made by mixing 50.0 ml of 0.100M potassium hydrogen phthalate with 13.6 ml of 0.100 M NaOH and diuting the miture to 100.0 ml, with water? The Kaz for hydrogen phthalate is 3.1 10-6. O 3.25 O 5.08 O 5.51 O 5.94
Calculate the pH of the buffers prepared in the following ways: a. by mixing 50.00 mL of 0.200 M ammonium nitrate, NH,NO,, with 25.00 mL 0.200 M NaOH b. by neutralizing half of the acid in 100.00 mL of 0.200 M ammonium nitrate solution with 1.0 M NaOH c. by mixing 60.00 mL of 0.400 M sodium formate (NaCHOO) with 40.00 mL 0.360 M HCI d. by mixing 80.00 mL of 1.00 M NH, with 40.00 mL of 1.00 M HCI e. by mixing equal volumes of 1.00 M NH, and 0.50 M HCI
Imagine that a 50.0 mM MES buffer is made by dissolving an appropriate mass of solid MES in water, adding NaOH ("titrating") until 60.0% of the MES is converted to its conjugate base, then diluting to the required final volume Write the net ionic equation for the reaction that occurs when a little HCl is added to this buffer, then calculate the pH that results when 1.00 mL of 0.250 M HCI is added to 50.0 mL of buffer Calculate the pH that results when 1.00 mL of 0.250 M NaOH is added to 50.0 mL of this buffer. Why does the pH change more when you add NaOH then when you add the same amount of HCI? Calculate the pH that results when 5.00 mL of 0.250 M NaOH is added to 50.0 mL of this buffer.
A scientist wants to prepare 500 ml of 500 mM formate buffer pH 3.00. The pKa for formic acid, нсоон, is 3.75. a. Identify the water components. b. Give the dissociation equation involved. c. Give the buffering action when the buffer system is added with (a) small amount of strong acids and (b) small amounts of strong base. d. What mass (in grams) of sodium formate (molar mass = 68 g/mol) is needed to separate the said buffer? Report the answer in 2 decimal places. (Show complete solution) e. What volume (in milliliters) of formic acid (molar mass = 46 g/mol; density = 1.22 g/mL) is needed to prepare the said buffer? Report the answer in 2 decimals places. (Show complete solution)