One of the buffers that can be used for running an agarose gel is 1x TBE (tris borate EDTA) buffer. The recipe for 1x TBE is: • 0.13 M tris • 45 mM boric acid • 2.5 mM EDTA How will you make 1 L of this buffer from 1 M stock solutions of tris, boric acid, and EDTA? Put your answers in the blanks. To make 1 Lof this buffer, would need: Lof 1 M Tris ml of 1 M boric acid ml of 1 M EDTA Then, these will be topped up with distilled water in a volumetric flask up to the 1 L mark.

One of the buffers that can be used for running an agarose gel is 1x TBE (tris borate EDTA) buffer. The recipe for 1x TBE is: • 0.13 M tris • 45 mM boric acid • 2.5 mM EDTA How will you make 1 L of this buffer from 1 M stock solutions of tris, boric acid, and EDTA? Put your answers in the blanks. To make 1 Lof this buffer, would need: Lof 1 M Tris ml of 1 M boric acid ml of 1 M EDTA Then, these will be topped up with distilled water in a volumetric flask up to the 1 L mark.

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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Name Formula Ka Kb Nitrous acid HNO2 1.4 x 10–11 Hypochlorous acid HClO 3.0 x 10–8 Phenol C6H5OH 9.52 x 10–5 Benzoic Acid C6H5COOH 6.28 x 10–5 Which of the following compounds could be used to create a buffer with a pH of 3.80? Nitrous acid Hypochlorous acid Phenol Benzoic acid 4 only 2 only 1 only 1 and 4 2 and 3
Calculate the pH of a dihydrogen phosphate/hydrogen phosphate buffer prepared with each of the following concentrations: 1. 0.10 M NaH2РОд and 0.10 Mм NazHPO4 2. 1.0 M NaH2РOд and 1.0 M NazHPO4 3. 0.50 M NaH2PO4 and 0.50M Na2HPO4 What do you conclude about the pH of a buffer when equal concentrations of the weak acid and conjugate base are used to prepare it?
A buffer contains 0.040 mol of lactic acid (pK₁ = 3.86) and 0.065 mol of sodium lactate per liter. H₂C. OH Lactic acid OH Calculate the pH of the buffer. H₂C OH Sodium lactate Calculate the change in pH after adding 7.0 mL of 0.30 M HCl to 1.0 L of the buffer. O Na+ Calculate the change in pH after adding 7.0 mL of 0.30 M HCl to 1.0 L of pure water. buffer pH: 4.07 buffer pH change: water pH change: 0.4 Incorrect 3.15 Incorrect units units
What is the pH of the buffer that results when 20.6 g sodium acetate (NaCH3CO2) is mixed with 431.8 mL of 1.6 M acetic acid (CH3CO2H) and diluted with water to 1.0 L?
You want to prepare a Glycine buffer (pKa’s 2.3 and 9.6) to simulate the pH in the intestine. You decide to make 150 mL of 300 mM glycine at pH 8.6. However, you only have glycinyl chloride (MW 111.5), 10 M HCl, 10 M NaOH, and water. Describe how to make this buffer with these materials.
What is the least volume of 3.10 M HCl(aq) that will exceed the buffer capacity of 1.00 L of a buffer that is composed of 0.40 M acetic acid and 0.72 M sodium acetate?(Ka for acetic acid = 1.8 × 10−5.) a. 0.55 L b. 5.5 L c. 0.14 L d. 1.6 L e. 0.20 L
Consider the following reaction:CH3COOH(aq)+OH−(aq)CH3COO−(aq)+H2O(l) pKa: 4.75 How much 5.60 M NaOH must be added to 420.0 mL of a buffer that is 0.0205 M acetic acid and 0.0260 M sodium acetate to raise the pH to 5.75?
What is a primary reason for needing to standardize strong base titrants like KOH? Select the single best answer. OKOH is not very soluble in aqueous solutions, thus making the concentrations difficult to determine. KOH reacts with moisture in the air, thereby making accurately-determined concentrations of their solutions difficult. O Standardization is the process of reacting a strong base, like KOH, with an acid. O Standardization is the process of dissolving KOH in aqueous solution. OKOH is a very inexpensive, highly soluble, and easy-to-use base.
-10 A chemistry graduate student is given 125. mL of a 1.80 M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K=4.9 × 10, What %3D mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH =9.20? You may assume that the volume of the solution doesn't change when the NACN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
-4 = A chemistry graduate student is given 500. mL of a 0.20M nitrous acid (HNO₂) solution. Nitrous acid is a weak acid with K = 4.5 × 10 What mass of NaNO₂ should the student dissolve in the HNO₂ solution to turn it into a buffer with pH = 3.46? You may assume that the volume of the solution doesn't change when the NaNO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. [] x10 Ś
You are tasked with making a buffer solution containing equal amounts of propionic acid from a 99.5 wt% solution (d = 0.993 g/mL, FW = 74.08 g/mol) and sodium propionate (solid, FW = 96.06 g/mol). What concentration of the buffer must be prepared to prevent a change in the pH by more than 0.5 pH units after the addition of 10.00 mL of 3.00 M HCl to 100.0 mL of the buffer solution? The Ka for propionic acid is 1.76 x 10-5.
A buffer must be prepared. The materials that may be used to prepare the buffer are: solid Na3PO4 12.1 Molar HCl The pKa's of the phosphate buffer are: pKa1=2.16 and pKa2=7.21. Question: How would a scientist prepare 2 Liters of 0.1 Molar buffer to obtain a. pH=3.5 and b. pH=7.3?