) Many proteins become insoluble (denature and precipitate out of solution) 3. ( when they are heated. An example is what happens when you break an egg into boiling water. A biochemist was studying a protein produced by a bacterium that can grow in very hot water. He discovered that this protein would not precipitate in boiling water unless he added some B-mercaptoethanol (also known as 2- mercaptoethanol or BME). In the presence of BME, the protein precipitated readily. a. Explain how BME could make this protein more sensitive to the denaturing effect of heat. Be a good chemist in your explanation.

) Many proteins become insoluble (denature and precipitate out of solution) 3. ( when they are heated. An example is what happens when you break an egg into boiling water. A biochemist was studying a protein produced by a bacterium that can grow in very hot water. He discovered that this protein would not precipitate in boiling water unless he added some B-mercaptoethanol (also known as 2- mercaptoethanol or BME). In the presence of BME, the protein precipitated readily. a. Explain how BME could make this protein more sensitive to the denaturing effect of heat. Be a good chemist in your explanation.

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter47: Benzocaine

Section: Chapter Questions

Problem 2Q

See similar textbooks

Similar questions

You are asked to make the compound [Ni(en)3]SO4. - By using 2.611 grams of NiSO4*6H2O (s) you dissolve the sample in deionized water completely. - You then add 10ml of 25% en into the solution and mix until a single product forms - When the addition of the en is complete, you then add 15ml of ethanol and mix. - using a bench vaccine and Buchner funnel, you filter the precipitate while carefully breaking up the solid until powder form. - the product is the washed with 15ml of ethanol and 15ml of acetone. Powder the solid and leave to dry Which is the limiting reagent? Write a balanced chemical equation for the reaction. How many miles of the product can you theoretically prepare?
0.5 g mixture of (0.1 N KCI and 4 points KBr) is required to 58.03 mL of 0.1 N AGNO3 to precipitate both bromide and chloride as AgCl and AgBr. Calculate the weight percentage for each of the AgCl and AgBr in a mixture if you know that the molecular weight of KCI = 74.5 and of KBr = 119 * %3D
2. In the preparation of the titrant, the solution must be aged for at least 24 hours in the dark. State in just 1 sentence why this step must be done.
Discuss the effect of branching (organic compounds) on solubility with at least 1 example.
Why is it normal to add a slight excess of silver nitrate solution when precipitating chloride ion?
Transfer 3-4 drops or a pinch of the test compound (Acetanilide) to 3 ml of the solvents, 5% NaOH and 5% NaHCO3 Shake the mixture thoroughly. The time required for the solute to dissolve in the solvent should not be more than 2 minutes. Indicate with (+) or (-) if the test compound is soluble or insoluble in the solvent. What is the theoretical solubility of Acetanilide in 5% NaOH? _______ What is the theoretical solubility of Acetanilide in 5% NaHCO3? _______
A group of wealthy chemistry 1A students had a little too much disposableincome and decided to create the most expensive they could think of. Using various spectroscopictechniques the salt was determined to be rhodium (III) Bromide (RhBr3). When this salt was shaken withpure water at 25°C, the solubility was found to be 0.026 mg/mL. Calculate the Ksp of RhBr3
What would happen to the solubility of BaSO4BaSO4in a 0.10 M CaSO4 solution in comparison to its solubility in water?
A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final precipitate (assumed to be Fe,03) contains 20.0 mg of Al,O3 by mistake, what percentage of Fe does the analyst find?
Magnesium fluoride (MgF2, MW = 62.30 g/mol) is slightly soluble in water, with Ksp = 7.4 x 10^-11 at T= 25. C.a) Give the correctly balanced solubility reaction and expression for Ksp for MgF2.b) What mass of magnesium fluoride will dissolve in 1.000 L of pure water?
The solubility of ferrous carbonate (FeCO3) at 20oC is 0.00066g/L. That is, 0.00066 g FeCO3 can be dissolved in 1 L water at 20oC at chemical equilibrium. Its dissociation is FeCO3 = Fe2+ + CO32-. If we have known that 0.00132 g FeCO3 has been dissolved in a cup of 2 L water, please estimate how many grams of FeCO3 will be additionally dissolved after we add 0.00132 more grams of FeCO3 to the cup?
During the mixing step, briefly discuss why gentle mixing of the solution is necessary after the addition of ferric chloride? How does this impact the next step of sedimentation?