1. Make the following solutions:Lysis buffer (100 mL): 0.1 M NaH,PO4, 10 mM Tris, 6 M Urea, pH 8.0Dissolve the bulk reagents, adjust the pH with HCl as necessary, dilute to 500 mlBradford Dye (500mL): 0.01% (w/v) Coomassie Blue G-250, 5% (v/v) ethanol, 8.5% phosphoric acidDissolve Coomassie in ethanol, then add the phosphoric acid. Dilute to 500 mLand filter through #1 Watman filter paper.Bovine Serum Albumin: 1 mg/mL in diH20

Buffer solution will not allow the sudden increase or decrease in the pH of the solution by the…

Answered: 1. Make the following solutions: Lysis…

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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To prepare 1 liter of 0.10 M acetate buffer at PH 5.20.I need to mix _____g of CH3COONa molecular weight 82.03 g/mol with ______ml of 6.0 moler HCL and dilute the solution to the volume of 1 liter .pKa of acetic acid is 4.76..fill in the above blanks.??.
A water at a drinking water plant has an alkalinity of 4*10-3 eq/L at a pH of 9.5. a) Find the TOTCO3 of this water, assuming carbonate is the only significant weak acid/base species b) 1.5*10-3 M HOCl is added to the water for disinfection. What will be the final pH and alkalinity of this water?
30.0 mL of the 1.0 M LIOH is added to 50.0 mL of 0.20 M H2SO4. What is the pH at this point in the titration? H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O pH = [?] Hint: How many moles of H+ and OH- are present? pH at 30 mL base Enter
A student needs to prepare a buffer made from CH3COOH and CH3COOK with pH 5.074. If K₂ for CH3COOH is [CH, COOH] [CH₂COOT] is required? C 1.80 x 10-5, what ratio of [CH3COOH] [CH, COO Submit Answer $ 000 R F V = % 5 [Review Topics] [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining T G Cengage Learning | Cengage Technical Support FS ^ 6 B MacBook Air ---F6 Y H & 7 N ◄◄ F7 U J * 00 8 ►ll M - ( 9 K F9 O Save and Exit dele
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A reaction was carried out between 18 ml of a 0.05 M solution of hydrochloric acid with 24 ml of a 0.2 M solution of ammonium hydroxide with (Kb-1.8x 10-5) at a temperature of 25 C. What is pH and pOH respectively of the solution product after the reaction. Note that the molecular weight of ammonium hydroxide is 35 g /mole and the molecular weight of hydrochloric aeid is 36.5 q/mole.
HOWICX S Geometry w/Datax S Practice 10.10 | Sex S Practice | SchoolcX G Sign in - Google/X Logins & Passwo X + gagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator= assignment-take ★ Other Booki [Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution contains 0.493 M C6H5NH3Br and 0.337 M C6H5NH2 (aniline). Determine the pH change when 0.088 mol NaOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change Submit Answer Retry Entire Group 1 more group attempt remaining HANA D ?? ak
2. Kinn and Porsche need to store a certain biomolecule in 300 mL of 0.50 M citrate buffer maintained at pH 5.90. Relevant equation: H3C6H507 (aq) Solids Ka1 = 8.4 x 10-4 H3C6H5O7 The available solids in the laboratory are as follows. NaH₂C6H5O7 Na2HC6H5O7 H₂C6H507 (aq) Na3C6H5O7 Ka2 = 1.8 x 10-5 Molar Mass, g/mol 192.124 214.100 236.090 HC6H507² (aq) 258.060 Ka3 = 4.0 x 10-6 -C6H507³- (aq) 2a. Help Kinn and Porsche prepare the buffer by supplying the missing information in the following table. Provide calculations as basis of choosing the identity of each solid. Show your solution on the computation of the mass of each solid needed to prepare the buffer. MASS (g) NEEDED TO
@ Prepare a "pH curve" as follows: a) Find the pH of the acid solution just before the end point when 0.1 ml of base less than the end point voiume has been added. potnt, therefore at the end of the titration ph - 7. We are assuming that end point equals equivalence b) Repeat calculation 'a' for a volume 1 ml less and 5 ml less then end point and before any base is added. That is Oml base added.) Before end point, we assume that all the base is used up by the acid. c) Assuming you had continued the titration past the end point, calculate the pH when 0.1 ml of base beyond end point had been added. d) Repeat calculation 'c' for 1 ml, S ml and 10 ml of base beyond end point. Show all calculations and record your results in a table similar ta the one shown below: excess H+ excess OH 0 -5 -1 END PT -.1 +.1 +1 +5 +10 (ML) BASE VOLUME 20 24 24-9 25 25.1|26 30 35 pH
Measurement of the pk, of an unknown acid by the half-neutralization method 0.1037 Concentration of standardized NaOH titrant mol/L Trial 1 Trial 2 Mass of unknown acid solution 30.01 30.00 Volume of NaOH added to half-neutralize the unknown acid 14.68 14.68 ml. ml Measured pH of half-neutralized solution 4.92 4.74 Average pH value pk, - Calculate the (H,0') and the concentration of A and HA, in the half-neutralized solution. K- (Note: In this solution, (H,0'1 (A 1) MH,0 MA M HA
How can you prepare 30 mM Phosphate buffer of pH=6.6 using the correct combination of the chemicals below? KH2PO4 (136.086 g/mol) K2HPO4 (174.2 g/mol) K3PO4 (212.27 g/mol) H;PO4 (98.00 g/mol; d=1.88 g/mL; 85%)

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