5. Why do we assume the concentration of acetic acid/acetate are very close to the formal...
what concentration of acetic acid (pka=4.76) and acetate would be required to prepare a .15 M buffer solution at pH 5.0? What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 5.07 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). (AVHA)....
You are making a pH 5.0 buffer with acetic acid (pKa = 4.75) and sodium acetate. You want the total concentration of acetate ([acetic acid] + [sodium acetate] ), to be 0.50 M. What concentrations of acetic acid and sodium acetate do you use to make your buffer? acetic acid sodium acetate
Calculate the pH of an acetic acid/acetate buffer in which the concentration of acetic acid is always 0.21 M, but the concentration of sodium acetate (NaCH,COO) corresponds to the following value: 0.63 M. (K, for CH,COOH is 1.8 x 10 5.) Report your answer to three significant figures.
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that in the first question. 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. That is, there are...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.20 M buffer solution at pH 5.0? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). [A-V[HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1:...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.20 M buffer e may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A]/[HA] 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. That is, there are 1.7 molecules acetate Step 1: The ratio of base to...
You have made 1.5 L of buffer by adding just acetic acid and no acetate to a final concentration of 0.300 M. However, you just adjusted the pH of the solution by adding NaOH to a pH of 4.5. The Ka of acetic acid is 1.7*10^-5. What are the new concentrations of acetic acid and acetate?
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that m the first question. STRATEGY 1. Rearrange the Hendereon-Hasselbalch equation to solve for thfe rabo of base (acetate) to aad (acetic add).[A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration ot acetic acid.
Key Ouestion #2: Determine the initial concentrations for the following solutions. Solution Preparation Acetic Acid Acetate Ion Concentration Concentration Solution #1 50.0 mL of 0.0500 M acetic acid and 0.205 grams of sodium acetate Solution #2 25.0 mL of 0.0500 M acetic acid, 25.0 mL of deionized water, and 0.205 grams of sodium acetate 50.0 mL of 0.0500 M acetic acid and 0.102 grams of sodium acetate Solution #3 Solution # 4 50.0 mL of 0.0500 M acetic acid Solution...
Calculate the mass of acetic acid that must be mixed with 0.88moles of sodium acetate to form a buffers solution of pH 5.2. Ka of acetic acid is 1.8 x 10-5