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For acetate with a pKa of roughly 4.2, what is a lowest pH where this molecule could serve as a good buffer?
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- For an acid HA with a pKa of 5.2, what is the ratio of the concentration of the conjugate base to that of the acid at pH 7.2.What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?For an acid with a pKa of 5.00, what is the pKb of its conjugate base?
- similar to the question what is the pKa of formic acid when the pH of buffer is 4.18?What is the pKb of the conjugate base of a weak acid that has a pKa equal to 5.29 at 25ºC?You need to perform an enzymatic reaction at pH 6.0. Someone suggests a weak acid with pKa of 5.5 as the basis of the buffer. Will this substance and its conjugate will make a appropriate buffer for your experiment? Why / why not?”
- I need help understanding why the ratio of Acetate:Acetic acid = 3.5:1 and why the total amount would be 4.5. The question was calculate the ratio of the concentrations of acetate and acetic acid required in a buffer system of pH 5.30. The pka of acetic is 4.76. Where is the 1 coming from in the ratio 3.5:1 The second part of the question said what if the question aked for the molar concentration of acetate and acetic acid in this buffer given that the over all buffer was 0.5 M. Why is the total amount 4.5?5.Which substance would be the best buffer at pH 7.6 if it had to be able to buffer against either acid or base? A. one with a pKa of 5.6 B. one with a pKa of 7.6 C. one with a pKa of 9.6 D. The pKa of a substance doesn't tell you whether it would be a good buffer at this pH. 6.For the following reaction, which of the following is true? A B AG = +15.9 A. The conversion of A to B is spontaneous B. The conversion of A to B is exergonic C. Both A and B D. Neither A nor BYou have a 1L 0.1M citric acid solution at a pH of 3.95 and you add to it 1 molar equivalent of NaOH. What is the resulting pH of the solution? Assume there is no volume change when the NaOH is added to the solution. Citric acid has the following pKa values associated with it: 3.1, 4.8 and 6.4. How can you tell the pka value to use?
- Which of the following acid/ conjugate base pairs would function best as a buffer at physiological pH? Lactic acid / Lactate ion; pka = 3.86 Carbonic acid / Bicarbonate ion; pka = 6.37 Bicarbonate ion / Carbonate ion; pKa = 10.25 Dihydrogen phosphate / Monohydrogen phosphate ion; pKa = 6.86 Acetic acid / Acetate ion; pka = 4.765. The pKa of acetic acid (HA) is approximately 4.8. If a solution of acetic acid is brought to pH= 4.8, what can we say about the concentrations of HA and its conjugate base A? a) The solution is acidic so there is more HA than A. b) HA is a weak acid so it dissociates easily and [A'] is higher than [HA]. c) Their concentrations are the same. d) We can't say, it depends on the initial concentration of HA. e) We can't say, it depends on temperature.3. The pH of the given solution of lactic acid and lactate is 4.30. Calculate the pKa of lactic acid, when the concentration of lactic acid and lactate are 0.020 M and 0.073 M respectively.