answer

watching

views

12 Dec 2019

You will need to make 50X TAE so that you can do gel electrophoresis. One of the ingredients is 0.5 M EDTA pH = 8.0. â¨EDTA stands for disodium ethylenediamindetratraacetateâ¢2(H2O). This EDTA solution will be provided to you. However, you should know how it was made, and the following two questions address this.

3. Determine the amount of EDTA needed to prepare 100 ml of 0.5 M EDTA pH = 8.0. The EDTA MW = 372.2 g/mole

4. As EDTA dissolves in water, the [H+] will increase (note that full name of EDTA includes "acetate"). To increase to a pH = 8.0, would you need to add HCl or NaOH?

answer

watching

128

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Lelia LubowitzLv2

13 Dec 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

Determine the amounts/volumes of the chemicals needed to prepare the following solutions:

5. 100 ml of 0.1 N HCl from concentrated (12.0 M) HCl [you will be asked to make this solution as practice]

6. 100 ml of 1.0 M Tris pH = 7.6 MW of Tris base is 121 g/mole [you will be asked to make this solution as practice]

7. pH 7.6 is close to a neutral pH. When making 1.0 M Tris base, would you expect to need HCl or NaOH to adjust the pH to 7.0?

To do electrophoresis, you will need to make a solution called TAE, which is a specific mixture of Tris base, acetic acid, and EDTA. Assuming no errors and no spills, you will need a minimum of 50 ml 1X TAE to make your agarose gel plus 1 liter of 1X TAE for gel running buffer. TAE is normally made as a 50X concentrated stock.

8. What is the minimum volume of 50X TAE that you will need to make?

I need help doing problem number 4 listed below. If someone could show the work required for this problem it would be a great help!

Below is a list of solutions you will need for the mini-prep. Make 5mL of each solution as a team and store each in a 15mL Falcon tube. Store solution 1 and 70% ethanol at 4 degrees Celsius. Solution 3 and Elution Buffer can be stored at room temperature. Show your calculations in the space provided below.

1. Solution 1 (lysis buffer) is (25mM Tris-HCl, pH 8.0, 50mM glucose, 10mM EDTA)

â Recall that you have Tris and EDTA stock solutions

â You will be provided with a 3M glucose stock solution

2. Solution 2 (Denaturing solution) is (0.2N NaOH, 1.0% SDS)

â Do NOT make today (it needs to be made fresh on the day of the mini-prep)

â You will be provided stocks of 1N NaOH and 10% SDS

3. Solution 3 (Renaturing Solution) is 5M potassium acetate.

â Add 3mL of 5M potassium acetate to 0.575mL of glacial acetic acid and 1.425mL of water

4. 70% ethanol (v/v)

â You will be provided with 100% (200 proof) ethanol

5. Elution Buffer (EB) is (10mM Tris-HCl, pH 8.0)

â Recall that you have Tris stock solution

This is for the lab practical I take on Tuesday night. If you could answer each one and show your work/ explain that'd be amazing so I can do well on the actual practical on Tuesday! Thank you!

Chemistry 211 Lab Final Study Guide Spring 2015

Useful Information:
1 ampere =coulomb/sec
Faradayâs constant = 96,500 coulombs/mole of electrons
Molar mass of Au = 197.0 g/mole, Molar mass of Cu = 63.55 g/mole
m = moles , ' â

c kg

ÎTf

= Tf

â Tf

where Tf is for the pure solvent and Tf

is for the mixture.

ÎT = (K

)(m ) ,

m = (

(mass of

solute, g )
)( ).

f f c

c molar

mass, g

mol â1

mass of

solvent, kg

7. Next question

(a) If you weigh 6.355 grams of copper, add concentrated nitric acid to dissolve it, and then dilute the solution to a total volume of 50 mL, how many moles of copper are in this solution?

(b) For the equilibrium reaction 3H2(g) + N2(g) â 2NH3(g), what is the equilibrium constant expression, Kc, for this reaction? (5pts)

8. Suppose at some temperature, the equilibrium concentration of H2 is 0.45M, the equilibrium concentration of N2 is 0.38M, and the equilibrium concentration of NH3 is 0.42M. What is the value of the equilibrium constant for the reaction 3H2(g) + N2(g) â 2NH3(g) at this temperature? (Show your work. No credit will be given if your work is not shown.)

9. Next question
(a) If you need 0.0534 moles of NaOH to reach equivalent point in the titration with acetic acid, how many mL of 0.09876M NaOH will you need?

(b) The Ksp of Cu(OH)2 is 2.2x10-20, what is the solubility of Cu(OH)2?

10. Next question
(a) In non-sulfide qualitative analysis of representative cations, the Group A cations comprising of Pb2+,

Hg2+, and Ag+ give a precipitate with solution.
(b) From a solution containing mixture of Pb2+, Fe3+, and Al3+, Pb2+ is removed by adding HCl solution. To the remaining cation mixture, on making the solution basic with NH3 (pH=9 â 10), both the cations form precipitate. Further analysis of the cation mixture containing Fe3+ and Al3+ is carried out by adding NaOH solution.

Aluminum hydroxide (dissolves/remains undissolved) in NaOH solution while Ferric hydroxide ( dissolves/remains undissolved).
(c) Fe(OH)3 precipitate is dissolved in minimal amount of aqueous HCl which gives a

yellow solution. To this solution addition of solution (at pH = 4 â 5) yields a dark blue solid known as Prussian Blue.

(d) Describe the method for checking for completeness of precipitate in qualitative analysis of ions.

Weekly leaderboard

Home

Homework Help 3,900,000

Chemistry 830,000

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard