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HEPES is commonly used to make physiological buffers and undergoes the following dissociation:   If a 0.1000 M buffer with a pH of 7.20 is to be made using sodium HEPES (HA–, MM = 260.29) what mass in g of sodium HEPES and what volume in mL of 6.0 M NaOH must be combined to make 2.000 L of this buffer?

HEPES is commonly used to make physiological buffers and undergoes the following dissociation:   If a 0.1000 M buffer with a pH of 7.20 is to be made using sodium HEPES (HA–, MM = 260.29) what mass in g of sodium HEPES and what volume in mL of 6.0 M NaOH must be combined to make 2.000 L of this buffer?

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ISBN:9781305957404
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HEPES is commonly used to make physiological buffers and undergoes the following dissociation:

 

If a 0.1000 M buffer with a pH of 7.20 is to be made using sodium HEPES (HA–, MM = 260.29) what mass in g of sodium HEPES and what volume in mL of 6.0 M NaOH must be combined to make 2.000 L of this buffer?

The image depicts a chemical equilibrium between two molecular structures, labeled as (HA⁻) and (A²⁻). ### Description: - **Left Structure (HA⁻):** - Contains a piperazine ring (a six-membered ring with two nitrogen atoms opposite each other). - Attached to the piperazine ring is a hydroxyethyl group (–CH₂CH₂OH) and an ethanesulfonate group (–CH₂CH₂SO₃⁻). - **Right Structure (A²⁻):** - Similar to the left structure but with the loss of a proton, resulting in an additional negative charge. - The hydroxyethyl group is now an ethoxyde group (–CH₂CH₂O⁻). ### Equilibrium Information: - The arrow between the two structures indicates a reversible reaction. - The equilibrium constant (Kₐ) for the reaction is given as 3.16 x 10⁻⁸. ### Explanation: This diagram illustrates the acid-base equilibrium between two forms of a compound. The (HA⁻) form donates a proton to become (A²⁻), forming a base with a higher degree of ionization. The Kₐ value suggests that the equilibrium greatly favors the reactant (HA⁻) side, indicating that HA⁻ is a weak acid. This concept is fundamental in understanding pH balance, buffer systems, and acid-base reactions in chemistry and biochemistry.
Transcribed Image Text:The image depicts a chemical equilibrium between two molecular structures, labeled as (HA⁻) and (A²⁻). ### Description: - **Left Structure (HA⁻):** - Contains a piperazine ring (a six-membered ring with two nitrogen atoms opposite each other). - Attached to the piperazine ring is a hydroxyethyl group (–CH₂CH₂OH) and an ethanesulfonate group (–CH₂CH₂SO₃⁻). - **Right Structure (A²⁻):** - Similar to the left structure but with the loss of a proton, resulting in an additional negative charge. - The hydroxyethyl group is now an ethoxyde group (–CH₂CH₂O⁻). ### Equilibrium Information: - The arrow between the two structures indicates a reversible reaction. - The equilibrium constant (Kₐ) for the reaction is given as 3.16 x 10⁻⁸. ### Explanation: This diagram illustrates the acid-base equilibrium between two forms of a compound. The (HA⁻) form donates a proton to become (A²⁻), forming a base with a higher degree of ionization. The Kₐ value suggests that the equilibrium greatly favors the reactant (HA⁻) side, indicating that HA⁻ is a weak acid. This concept is fundamental in understanding pH balance, buffer systems, and acid-base reactions in chemistry and biochemistry.
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