Suppose there is a buffer solution (pK,=4.75) made of one aqueous solution of acetic acid (0.001M) and an aqueous solution of acetate (0.01M). Based on the information given, does this buffer have a bigger acid or base buffer capacity? Select one: Bigger base capacity Same capacity for acid and base O Bigger acid capacity O There is not enough information provided

Suppose there is a buffer solution (pK,=4.75) made of one aqueous solution of acetic acid (0.001M) and an aqueous solution of acetate (0.01M). Based on the information given, does this buffer have a bigger acid or base buffer capacity? Select one: Bigger base capacity Same capacity for acid and base O Bigger acid capacity O There is not enough information provided

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 4RQ: A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If...

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A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is the pKa of the solution would it be considered a buffer
How many moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) to make a buffer with a pH of 10.90? Let x represent the original concentration of CH3COO- in the water. Based on the given values, set up the ICE table in order to dtermine the unknown.
A laboratory manager wants to prepare 500.00 mL of a buffer with a pH of 4.471 from equimolar solutions of CH3CO2H (Ka = 1.800e-5) and LiCH3CO2. What volume of the LiCH3CO2 solution would be required? Key Concept: Buffers resist pH change and are prepared by mixing the conjugate acid and base together. The pH is determined from the Henderson-Hasselbach equation: pH = pKa + log([A−]/[HA]).Solution: Since the molarities of the two solutions making the buffer are the same, the Henderson-Hasselbach equation can be written as: pH = pKa + log(V(A−)/V(HA)) where V(A−) = the volume of the conjugate base and V(HA) = the volume of the conjugate acid.
For 480.0 mLmL of a buffer solution that is 0.160 M� in CH3CH2NH2CH3CH2NH2 and 9.00×10−2 M� in CH3CH2NH3ClCH3CH2NH3Cl, calculate the initial pHpH and the final pHpH after adding 1.5×10−2 molmol of HClHCl. ( Kb(CH3CH2NH2)=5.6×10−4�b(CH3CH2NH2)=5.6×10−4.)
What quantity (moles) of must be added to 1.0 L of 1.7 M to produce a solution buffered at pH = pKa?Ka = 1.8 x 10-5Quantity = _______ mol What quantity (moles) of must be added to 1.0 L of 1.7 M to produce a solution buffered at pH = 4.00? Ka = 1.8 x 10-5 Quantity = _______ mol 3. What quantity (moles) of must be added to 1.0 L of 1.7 M to produce a solution buffered at pH = 5.00 ? Ka = 1.8 x 10-5 Quantity = _______ mol
Calculate the pH of a bicarbonate buffer that is composed of a solution that is 0.5 M sodium carbonate and 0.05 M carbonic acid. The pK is 6.10.
A buffer of acetic acid and sodium acetate is prepared by mixing 10.0 mL of 0.50 M acetic acid with 0.41 grams of sodium acetate (molar mass = 82.0343 grams/mole). Calculate the concentration of acetic acid and acetate ion in the buffer (total volume of the solution is 100.0 mL). Additionally, the pH of the solution is 4.75. Explain why this is significant.
[20] ml of [4] M HC2H3O2 is titrated with 2.25 M sodium hydroxide. Ka for HC2H3O2 is 1.8 x 10-5 a. How many mL of sodium hydroxide will be needed to reach the equivalent point? b. What will the pH be at the midpoint to equivalent point (half equivalent)? c. What will the pH be at the equivalent point? d. What will be the pH when an excess 25 mL of sodium hydroxide is added?
Only typed explanation otherwise leave it Calculate the molar solubility of CaSO4(s) in 0.450 M Na2SO4(aq) at 25°C. The ?sp of CaSO4 is 4.93×10−5.
what volume of acetic acid 0.1 M and what volume of sodium acetate 0.1 M should be added together to produce a solution (buffer) with a pH of 4.6?
What is the proper unit of molar ratio of weak acid and its conjugate base in a buffer solution? Is it mol to mol or part to part? Or is it unitless? I need to express the answer 1.45/1 = [A]/[HA] to the right unit. See image for more details. the buffer is acetic acid/sodium acetate buffer.