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18 Nov 2019
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What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 5.0? Note that the concentration and/or pH value 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 2. Use the mole fraction of acetate to calculate the concentration of acetate 3. Calculate the concentration of acetic acid Use the mole traction of acetate to calculate the concentration of acetate Hasselbalch equation o e for Step 1: Rearrange the Henderson Hasselbalch equation to solve for HA) The Henderson-Hasselbalch equation is pH-pK log HA Use the Henderson- Hasselbalch eguation to Use the Henderson-Hasselbalch equation to solve for if the solution is at pH 5.0 Number Enter your answer as a number. For example, 9.6 Do not enter a formula like 106+2 0223
1.)
2.)
3.)
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 5.0? Note that the concentration and/or pH value 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 2. Use the mole fraction of acetate to calculate the concentration of acetate 3. Calculate the concentration of acetic acid Use the mole traction of acetate to calculate the concentration of acetate Hasselbalch equation o e for Step 1: Rearrange the Henderson Hasselbalch equation to solve for HA) The Henderson-Hasselbalch equation is pH-pK log HA Use the Henderson- Hasselbalch eguation to Use the Henderson-Hasselbalch equation to solve for if the solution is at pH 5.0 Number Enter your answer as a number. For example, 9.6 Do not enter a formula like 106+2 0223
Elin HesselLv2
1 Aug 2019