Answered: YOU DO: 1) What is the [F-]…

YOU DO: 1) What is the [F-] concentration in a buffer solution with a pH of 3.05? The solution contains 2.00 M of HF, HF has a pK₂ of 3.20.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 33QAP: A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this...

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Ionic Equilibrium

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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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1) What is the [F-] concentration in a buffer solution with a pH of 3.05? The solution contains 2.00 M of
HF, HF has a pKa of 3.20.

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A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
The pH of a Buffer containing 1.0M CH3COOH and 0.1M CH3COONA (pKa of * :CH3COOH =4.74) is 3.0 4.74 O 3.74 O 5.74 O
A buffer solution is prepared in which the concentration of pyruvic acid, HC;H3O3, is 0.300 M and the concentration of pyruvate, C3H3O3- is 0.20 M. What is the pH of this solution? The dissociation constant, Ka, is 4.07 x 10-³. A) 2.21 B) 2.56 C) 11.79 D) -2.21
A buffer is prepared as a solution of 4.7 M HA and 8.3 M NaA. The pH of the solution is 3.81. What is the pK, of the acid, HA? answer to two decimals
what will be the pH of a buffer solution containinf an acid with a pKa of 2.2 with an acid concentration equivalent to that of its conjugate base?
Which of the following statement is correct about a solution contains 0.2 M NaH PO, and 0.5 M H3PO,? O This is NOT a buffer solution. O Adding 0.01 mol NaOH to the solution will slightly decrease the pH. O Adding 0.01 mol NaOH to the solution will slightlyincrease the pH. O The solution pH is more than pk, of H3PO4 O The solution pH is equal to the pK, of H3PO4
A buffer solution contains formic acid and a salt solution containing sodium formate. What is the pH of a solution that is 0.0250 M in formic acid and 0.0625 M in sodium formate? pKa of formic acid is 3.745.
Which of the following 1.0 L solutions would produce a buffer with a pH of approximately 3.2? A solution of 6.3 x 10 moles of HNO3. O A solution of 0.100 moles of CH3CO;H (K, - 1.8 x 10) and 0.100 moles of NaCH3CO2. O A solution of 0.100 moles of NH3 (K, -1.8 x 10 ) and 0.100 moles of NH4CI. O A solution of 0.100 moles of HF (K, = 6,4 x 10 ) and 0.100 moles of KF. %3! O A solution of 0.100 moles of HBr and 0.099 moles of NaOH.
Calculate the pH of a buffer solution containing 1.3 M NaF and 0.80 M HF. Data: pKa (HF) = 3.17
1. Calculate the pH of a buffer solution that is 0.5M CH3COOH and 0.8 M NaCH3COO. (pKa for acetic acid is 4.74)
Be sure to answer all parts. Tris [tris(hydroxymethyl)aminomethane] is a common buffer for studying biological systems. (K = 5.01 × 10 and pK = 8.3) (a) Calculate the pH of the Tris buffer after mixing 11.0 mL of 0.20 M HCl solution with 25.0 mL of 0.10 M Tris. (b) This buffer was used to study an enzyme-catalyzed reaction. As a result of the reaction, 0.00019 mol of H* was produced. What is the pH of the buffer at the end of the reaction? (c) What would be the final pH if no buffer were present?

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