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CH3-CH2-OH + NAD+ -> CH3-COH + NADH + H+
The rate of this reaction can be measured by following the change in pH. The reaction is run in 1 mL 10mM buffer at pH = 8.6. If the pH of the reaction solution falls to 8.4 after 10 minutes, what is the rate of alcohol oxidation, expressed as nano moles of ethanol oxidized per mL per sec of reaction mixture?
Answer: 1.53 nmol / mL * sec
Ethanol is being oxidized and the pH change is .2 units. I'm not sure how to incorporate the reaction volume or molarity of the buffer. I was thinking of relating everything with the henderson-hasselbalch equation but I got stuck.
Edit (in case anyone else is interested!):
It looks like there was a piece of information left out. pKa of the buffer is 8.08. Using this, plugging into the henderson-hasselbalch equation and solving for the # of mol of the buffer provides two equations to solve for HA and A in nmol. Then the rate is found by dividing delta nmol H / (1 mL * 600 sec).
The rate of this reaction can be measured by following the change in pH. The reaction is run in 1 mL 10mM buffer at pH = 8.6. If the pH of the reaction solution falls to 8.4 after 10 minutes, what is the rate of alcohol oxidation, expressed as nano moles of ethanol oxidized per mL per sec of reaction mixture?
Answer: 1.53 nmol / mL * sec
Ethanol is being oxidized and the pH change is .2 units. I'm not sure how to incorporate the reaction volume or molarity of the buffer. I was thinking of relating everything with the henderson-hasselbalch equation but I got stuck.
Edit (in case anyone else is interested!):
It looks like there was a piece of information left out. pKa of the buffer is 8.08. Using this, plugging into the henderson-hasselbalch equation and solving for the # of mol of the buffer provides two equations to solve for HA and A in nmol. Then the rate is found by dividing delta nmol H / (1 mL * 600 sec).
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