Your goal is to make a buffer with a pH of 4.95 from acetic acid and sodium acetate. ASsume the pKa for acetic acid is 4.74. What is the volume of acetic acid added make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the ml of base and acid to add.

Your goal is to make a buffer with a pH of 4.95 from acetic acid and sodium acetate. ASsume the pKa for acetic acid is 4.74. What is the volume of acetic acid added make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the ml of base and acid to add.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 95AP

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Similar questions

The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
For the titration of 50.0 mL of 0.100-M HCl with 0.100-M NaOH, calculate the pH when these volumes of NaOH have been added: (a) 10.0 mL (b) 25.00 mL (c) 45.0 mL (d) 50.5 mL
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Your goal is to make a buffer with a pH of 4.95 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of acetic acid added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.
Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of 1 M sodium acetate added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.
A 1.0L buffer is made at 25°C that consists of 0.80 mol of a weak acid HA and 0.80 mol of its conjugate base A-. The acid ionizarion constant is Ka= 1×10^-4. To this buffer solution 0.80 mol NaOH is added. Assuming that the volume change due to the added NaOH is negligible, calculate pOH in the resulting solution.
Use the Henderson-Hasselbach equation to determine the ratio of acid to conjugate base if a buffer is being created with a pH of 4.00 and a pKa of 4.75. Henderson-Hasselbalch: pH = pKa + log[base]/[acid]
Calculate the molarity of the acid (HA) and the conjugate base (A- ) . For acetate, use grams-to-mol conversion and divide it by the total volume. For (aceitic acid), use M1V1=M2V2. Consider the total volume of your buffer (50 mL + 10 mL). a) [A-] = b) [HA] = I am not sure how to answer this or if it is related to this info that we were given at the top of the page: "A buffer is made by mixing 2.0 g of sodium acetate (NaA: 1 mol / 82 g) and 10 mL of 3.0 M acetic acid. Then 50 mL of water is added to the mixture. Find the pH of this buffer!"
Consider exactly one litre of a propanoic acid buffer solution, containing 0.600 M C3H5OOH and 0.252 M C3H5OO- . 1.1 Determine the pH of the buffer solution. - You may use “HA” to denote the formula of the acid. - You may make certain assumptions to simplify your calculations - Ka for hydrofluoric acid is 1.3 × 10−5 . 3.2 Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. mL of a 1.00 × 10−2 M HCℓ solution is added to it. You must indicate all the relevant reaction equations in your working.
The Henderson-Hasselbalch equation (pH = pKa + log([A-]/[HA]) fails at the start of a weak acid/strong base titration as well as before the equivalence point is reached. pKa 1 is the expected buffering capacity of a buffer where the Henderson-Hasselbalch equation is valid. Describe why this is the case.
You are asked to prepare a pH = 3.00 buffer starting from 2.00 L of 0.025 M solution of benzoic acid (C6H5COOH). (a) What is the pH of the benzoic acid solution prior to adding sodium benzoate? (hint: write the reaction equation for the acid dissociation and then use the equilibrium constant expression to calculate [H + ]) (b) How many grams of sodium benzoate should be added to prepare the buffer? Neglect the small volume change that occurs when the sodium benzoate is added.(hint: use the equilibrium constant expression to calculate [C6H5COO− ] in the buffer)