A student needs to prepare a buffer solutionwith a pH of 4.54. Assuming a pKg of 4.58, howmany ml of 0.1 M NAOH would need to beadded to 20.0 mL of 0.1 M HB to prepare thisbuffer?Please include a proper (abbreviated) unit.HINT : Use pH = pK, + log ([B minus]/[HB]) or, ifconcentrations are the same,pH = pk, + log (Volume of OH minus/ (Volumeof HB minus Volume of OH minus)

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Answered: A student needs to prepare a buffer…

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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You are asked to prepare a buffer solution with a pH of 3.50. The following solutions, all 0.100 M, are available to you: HCOOH, CH3COOH, H3PO4 , NaCHOO, NaCH3COO, and NaH2PO4. What ratio of [conjugate base]/[acid] would yield the best result for the required buffer solution created in the question above? ENTER YOUR ANSWER AS ONE NUMBER ROUNDED TO TWO DECIMAL PLACES.
A 1.37 L buffer solution consists of 0.298 M propanoic acid and 0.175 M sodium propanoate. Calculate the pH of the solution following the addition of 0.067 mol HCI. Assume that any contribution of the HCl to the volume of the solution is negligible. The K, of propanoic acid is 1.34 × 10-5. pH =
A chemist titrates 150.0 mL of a 0.0676M dimethylamine ((CH,) NH) solution with 0.4402M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, of dimethylamine is 3.27. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added. pH = Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibity MacBook Air
A 1.50 L buffer solution consists of 0.280 M propanoic acid and 0.139 M sodium propanoate. Calculate the pH of the solution following the addition of 0.065 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The Ka of propanoic acid is 1.34×10^−5.
An aqueous solution contains 0.386 M dimethylamine ((CH3)2NH).How many mL of 0.379 M perchloric acid would have to be added to 250 mL of this solution in order to prepare a buffer with a pH of 10.800.
The buffer was made by combining 0.220 M lactic acid (HC3H5O3) and 0.200 M sodium lactate ( NaC3H5O3). The Ka of HC3H5O3 is 1.4 x 10^-4. 1. write the equation describing the conjugate acid base relationship 2. Calculate the pH of the buffer 3. Calculate the pH of the buffer after the addition of 100.0 mL of 0.100 M potassium hydroxide to 0.9000 L of the buffer solution
A chemist titrates 110.0 mL of a 0.7452M aniline (C,H,NH,) solution with 0.5088M HCl solution at 25 °C. Calculate the pH at equivalence. The p K, of aniline is 4.87. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = ||
A student needs to prepare a buffer solution with a pH of 4.60. Assuming a pK a of 4.12, how many mL of 0.1 M B minus would need to be added to 20.0 mL of 0.1 M HB prepare this buffer? Please include a proper (abbreviated) unit.HINT : Use pH = pK a + log ([B minus]/[HB]) or, if concentrations are the same, pH = pK a + log (Volume of B minus / Volume of HB)
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.
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: mL sodium benzoate: mL
For 250.0 mL of a buffer solution that is 0.290 M in CH3CH2NH2 and 0.210 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 0.022 mol of NaOH . ( Kb(CH3CH2NH2)=5.6×10−4 .) What is the initial and final pH?
Imagine that a 50.0 mM MES buffer is made by dissolving an appropriate mass of solid MES in water, adding NaOH ("titrating") until 60.0% of the MES is converted to its conjugate base, then diluting to the required final volume Write the net ionic equation for the reaction that occurs when a little HCl is added to this buffer, then calculate the pH that results when 1.00 mL of 0.250 M HCI is added to 50.0 mL of buffer Calculate the pH that results when 1.00 mL of 0.250 M NaOH is added to 50.0 mL of this buffer. Why does the pH change more when you add NaOH then when you add the same amount of HCI? Calculate the pH that results when 5.00 mL of 0.250 M NaOH is added to 50.0 mL of this buffer.

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