What is the pH of 3.00 L of a buffer made of (4.24x10^-1) M HBrO and(6.8300x10^-1) M KBrO?Enter your answer in scientific notation with 3 sig figs. Do not include any units inyour answer.Do not round any intermediate calculations.Note: Your answer is assumed to be reduced to the highest power possible. What is the pH of 1.00 L of a buffer made of (3.30x10^-1) M (CH3)3N and(8.000x10^-1) M (CH3)3NHCI AFTER adding 0.02 moles of NaOH(s)?Note: Assume the total volume of this solution does NOT change after the additionof the solid.Enter your answer in scientific notation with 3 sig figs. Do not include any units inyour answer.Do not round any intermediate calculations.Note: Your answer is assumed to be reduced to the highest power possible.

It's a multiple question type and according to the guidelines of Bartleby, we are supposed to answer…

What is the pH of 3.00 L of a buffer made of (4.24x10^-1) M HBrO and (6.8300x10^-1) M KBrO? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.

What is the pH of 3.00 L of a buffer made of (4.24x10^-1) M HBrO and (6.8300x10^-1) M KBrO? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.

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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3. If you didn't have a pH meter, how would you make 1.00 L of 40.0 mM potassium phosphate buffer at pH 6.96, given ONLY potassium phosphate monobasic (KH₂PO4) and potassium phosphate dibasic (K₂HPO4)? These are the only two chemical available -no strong acid or base are needed. Include details such as masses and when/how you would bring the volume up to 1L. Show your calculations. Use pka2=7.20 for phosphoric acid.
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a) A student prepares an 750.0 mL buffer solution with a pH of 4.85 by adding sodium acetate to a solution of acetic acid. However, they forgot to document the mass of NaC2H3O2 added to the beaker. Fortunatelly, they know that the concentration of HC2H3O2 is 0.235M. Determine the mass, in grams, of NaC2H3O2 that must have been added to the solution. (Molar Mass of NaC2H3O2=82.0343 g/mol) b) 10 mL is accidentally spilled into the buffer solution from part a. Determing the new pH of the solution.
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