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1. Keeping in mind the definition of a buffer, prec Start with 50 mL of buffer at pH 9.00. Add b. Start with 50 mL of buffer at pH 9.00. Add Start with 50 mL of buffer at pH 9.00. Add d. Start with 50 mL of buffer at pH 9.00. Add a. Buffer: C. e. Start with 50 mL of pure water at pH 7.00. f. Start with 50 mL of pure water at pH 7.00

1. Keeping in mind the definition of a buffer, prec Start with 50 mL of buffer at pH 9.00. Add b. Start with 50 mL of buffer at pH 9.00. Add Start with 50 mL of buffer at pH 9.00. Add d. Start with 50 mL of buffer at pH 9.00. Add a. Buffer: C. e. Start with 50 mL of pure water at pH 7.00. f. Start with 50 mL of pure water at pH 7.00

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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ar 19, 2023 at 10:09 PM Buffers I Objectives The goal of this lab experiment is to investigate the inherent properties of a buffer system. From this lab you will: Prepare a buffer and measure pH before and after changes to the system Find the limits of a buffer system . Compare a buffer system to a non-buffer system Design a buffer system given a particular pH using two different methods Theory A buffer simply consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an important buffer in our bloodstream consists of H₂CO3 and HCO3 as shown in Eq 1. (1) H₂CO3(aq) + H₂O(1) H3O* (aq) + HCO3(aq) The main function of this buffer is to resist pH changes. This buffer acts of hold the pH of blood in the narrow range of 7.36 to 7.42 to allow proteins in our blood to function properly. To be more specific, the buffer will neutralize added base (Eq 2) by reacting with the weak acid in the system and producing more conjugate base. H₂CO3(aq) + OH(aq) → H₂O(1) + HCO3(aq) In contrast, the addition of acid (Eq 3) to the buffer system will react with the conjugate base and form more weak acid. (2) HCO3(aq) + H3O+ (aq) → H₂CO3(aq) + H₂O (1) One toxic compound that has been known to destroy this blood buffering system is ethylene glycol, the main component of antifreeze. When metabolized ethylene glycol is converted to glycolic acid, and then it rapidly enters the bloodstream. At first, the bicarbonate ion, HCO3, neutralizes the added acid; however, the conjugate base is rapidly consumed, and the pH of the blood begins to drop to dangerously low levels. In any buffer system, the addition of large amounts of acid or base will eventually destroy the neutralizing power of the buffer. This is called exceeding the buffer capacity. Buffer capacity will be further investigated in next week's lab. (3) When studying different living organisms, it is often important to work within the living systems' pH range. The pH of a buffer is established by the relative concentrations of weak acid and conjugate base in the solution. The acid dissociation constant, Ka, is a great tool to establish the relationship between these concentrations using Eq 1. The Ka of the carbonic acid-bicarbonate system is shown below (Eq 4). 1
Transcribed Image Text:ar 19, 2023 at 10:09 PM Buffers I Objectives The goal of this lab experiment is to investigate the inherent properties of a buffer system. From this lab you will: Prepare a buffer and measure pH before and after changes to the system Find the limits of a buffer system . Compare a buffer system to a non-buffer system Design a buffer system given a particular pH using two different methods Theory A buffer simply consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an important buffer in our bloodstream consists of H₂CO3 and HCO3 as shown in Eq 1. (1) H₂CO3(aq) + H₂O(1) H3O* (aq) + HCO3(aq) The main function of this buffer is to resist pH changes. This buffer acts of hold the pH of blood in the narrow range of 7.36 to 7.42 to allow proteins in our blood to function properly. To be more specific, the buffer will neutralize added base (Eq 2) by reacting with the weak acid in the system and producing more conjugate base. H₂CO3(aq) + OH(aq) → H₂O(1) + HCO3(aq) In contrast, the addition of acid (Eq 3) to the buffer system will react with the conjugate base and form more weak acid. (2) HCO3(aq) + H3O+ (aq) → H₂CO3(aq) + H₂O (1) One toxic compound that has been known to destroy this blood buffering system is ethylene glycol, the main component of antifreeze. When metabolized ethylene glycol is converted to glycolic acid, and then it rapidly enters the bloodstream. At first, the bicarbonate ion, HCO3, neutralizes the added acid; however, the conjugate base is rapidly consumed, and the pH of the blood begins to drop to dangerously low levels. In any buffer system, the addition of large amounts of acid or base will eventually destroy the neutralizing power of the buffer. This is called exceeding the buffer capacity. Buffer capacity will be further investigated in next week's lab. (3) When studying different living organisms, it is often important to work within the living systems' pH range. The pH of a buffer is established by the relative concentrations of weak acid and conjugate base in the solution. The acid dissociation constant, Ka, is a great tool to establish the relationship between these concentrations using Eq 1. The Ka of the carbonic acid-bicarbonate system is shown below (Eq 4). 1
rs I prelab handout F22 023 at 10:09 PM a. Buffers 1 prelab 1. Keeping in mind the definition of a buffer, predict the resulting pH in the following scenarios: Start with 50 mL of buffer at pH 9.00. Add 5 drops of 0.10 M KOH. b. Start with 50 mL of buffer at pH 9.00. Add 5 drops of 0.10 M HCI. e. Name: f. Hailey Gary C. Start with 50 mL of buffer at pH 9.00. Add 10 mL of 0.10 M KOH. d. Start with 50 mL of buffer at pH 9.00. Add 10 mL of 0.10 M HCI. Start with 50 mL of pure water at pH 7.00. Add 5 drops of 0.10 KOH. Start with 50 mL of pure water at pH 7.00. Add 5 drops of 0.10 HCI. pH = pH = pH = pH = pH = pH =
Transcribed Image Text:rs I prelab handout F22 023 at 10:09 PM a. Buffers 1 prelab 1. Keeping in mind the definition of a buffer, predict the resulting pH in the following scenarios: Start with 50 mL of buffer at pH 9.00. Add 5 drops of 0.10 M KOH. b. Start with 50 mL of buffer at pH 9.00. Add 5 drops of 0.10 M HCI. e. Name: f. Hailey Gary C. Start with 50 mL of buffer at pH 9.00. Add 10 mL of 0.10 M KOH. d. Start with 50 mL of buffer at pH 9.00. Add 10 mL of 0.10 M HCI. Start with 50 mL of pure water at pH 7.00. Add 5 drops of 0.10 KOH. Start with 50 mL of pure water at pH 7.00. Add 5 drops of 0.10 HCI. pH = pH = pH = pH = pH = pH =
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