Textbook Question
Calculate the pH of 0.375 L of a 0.18 M acetic acid–0.29 M sodium acetate buffer before and after the addition of (b) 0.0060 mol of HBr. Assume that the volume remains constant.
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Ch.17 - Applications of Aqueous Equilibria
Chapter 17, Problem 73
What is the Henderson–Hasselbalch equation to calculate the ratio of HCO3- and H2CO3 in blood with a pH of 7.40, given that the value of Ka for carbonic acid at body temperature (37 degrees Celsius) is 7.9 x 10^-7?
Verified step by step guidance1
Identify the Henderson–Hasselbalch equation: \( \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \), where \([\text{A}^-]\) is the concentration of the base form (HCO3-) and \([\text{HA}]\) is the concentration of the acid form (H2CO3).
Calculate the pKa from the given Ka value using the formula \( \text{pKa} = -\log(\text{Ka}) \).
Substitute the given pH value (7.40) and the calculated pKa into the Henderson–Hasselbalch equation.
Rearrange the equation to solve for the ratio \( \frac{[\text{HCO}_3^-]}{[\text{H}_2\text{CO}_3]} \).
Use the properties of logarithms to express the ratio in terms of powers of 10, if needed, to simplify the interpretation of the result.
Related Practice
Textbook Question
Use the Henderson–Hasselbalch equation to calculate the pH of a buffer solution that is 0.25 M in formic acid (HCO2H) and 0.50 M in sodium formate (HCO2Na).
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Open Question
A food chemist studying the formation of lactic acid in sour milk prepares a buffer that is 0.58 M in lactic acid (HC3H5O3) and 0.36 M in sodium lactate (NaC3H5O3). Use the Henderson–Hasselbalch equation to calculate the pH of the buffer solution.
Textbook Question
The ratio of HCO3- to H2CO3 in blood is called the 'bicarb number' and is used as a measure of blood pH in hospital emergency rooms. A newly diagnosed diabetic patient is admitted to the emergency room with ketoacidosis and a bicarb number of 10. Calculate the blood pH. Ka for carbonic acid at room temperature (37 degrees Celsius) os 7.9 x 10^-7).
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Textbook Question
In what volume ratio should you mix 1.0 M solutions of NH4Cl and NH3 to produce a buffer solution having pH = 9.80?
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Textbook Question
Give a recipe for preparing a CH3CO2H-CH3CO2Na buffer solution that has pH = 4.44.
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