WEB To make a buffer with pH=3.0 from HCHO2 and CHO2 ^-, (a) what must the [HCHO2] /[CHO2^-]rati

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WEB To make a buffer with pH=3.0 from HCHO2 and CHO2 ^-, (a)...

WEB To make a buffer with $\mathrm{pH}=3.0$ from $\mathrm{HCHO}_2$ and $\mathrm{CHO}_2{ }^{-}$, (a) what must the $\left[\mathrm{HCHO}_2\right] /\left[\mathrm{CHO}_2^{-}\right]$ratio be? (b) how many moles of $\mathrm{HCHO}_2$ must be added to a liter of 0.139 M $\mathrm{NaCHO}_2$ to give this pH ? (c) how many grams of $\mathrm{NaCHO}_2$ must be added to 350.0 mL of $0.159 \mathrm{M} \mathrm{HCHO}_2$ to give this pH ? (d) What volume of $0.236 M \mathrm{HCHO}_2$ must be added to 1.00 L of a 0.500 M solution of $\mathrm{NaCHO}_2$ to give this pH ? (Assume that volumes are additive.)

WEB To make a buffer with $\mathrm{pH}=3.0$ from $\mathrm{HCHO}_2$ and $\mathrm{CHO}_2{ }^{-}$,
(a) what must the $\left[\mathrm{HCHO}_2\right] /\left[\mathrm{CHO}_2^{-}\right]$ratio be?
(b) how many moles of $\mathrm{HCHO}_2$ must be added to a liter of 0.139 M $\mathrm{NaCHO}_2$ to give this pH ?
(c) how many grams of $\mathrm{NaCHO}_2$ must be added to 350.0 mL of $0.159 \mathrm{M} \mathrm{HCHO}_2$ to give this pH ?
(d) What volume of $0.236 M \mathrm{HCHO}_2$ must be added to 1.00 L of a 0.500 M solution of $\mathrm{NaCHO}_2$ to give this pH ? (Assume that volumes are additive.)

Key Concepts

Molarity and Stoichiometric Calculations

Molarity (moles per liter) and stoichiometry are key concepts in solution chemistry used to calculate the number of moles of reactants and products in a chemical reaction. In the context of buffer preparations, these calculations are necessary for determining how much of a particular acid or base must be added to a solution to obtain a buffer with the desired concentration and pH.

Acid Dissociation and pKa

The acid dissociation constant (Ka) and its logarithmic form, pKa, provide a measure of the strength of a weak acid in solution. Understanding pKa is essential in buffer calculations, as it directly influences the pH of the buffer and the ratio of the acid to its conjugate base required to achieve a target pH.

Buffer Solutions

Buffer solutions are mixtures of a weak acid and its conjugate base (or a weak base and its conjugate acid) that resist changes in pH when small amounts of acid or base are added. They are essential in many chemical and biological systems to maintain a stable pH, and their design often involves selecting appropriate acid-base pairs and calculating the required amounts to achieve the desired pH.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a fundamental tool used to relate the pH of a buffer solution to the acid dissociation constant (pKa) of the weak acid and the ratio of the concentrations of the conjugate base to the acid. This equation, pH = pKa + log([conjugate base]/[acid]), is crucial for determining the necessary proportions of acid and base needed to create a buffer with a specific pH.

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