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Chapter 14: Problem 80

Someone with severe diabetes obtains energy by the breakdown of fats, which produce large amounts of acidic substances. How would this affect the \(\mathrm{pH}\) of the blood plasma?

Short Answer

Expert verified
The breakdown of fats in severe diabetes produces acidic ketones, which lowers the blood plasma pH.

Step by step solution

01

- Understand the relationship between acids and pH

pH is a measure of the hydrogen ion concentration in a solution. Lower pH values indicate higher acidity, meaning more hydrogen ions are present.
02

- Identify the substances produced

In severe diabetes, the breakdown of fats produces acidic substances called ketones.
03

- Determine the effect of ketones on blood plasma pH

Ketones are acidic, so their presence in the blood will increase the concentration of hydrogen ions, leading to a decrease in the pH of the blood plasma.
04

- Conclude

The increase in acidic substances (ketones) due to fat breakdown will lower the pH of the blood plasma, making it more acidic.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

acidic substances
When we talk about acidic substances, we refer to compounds that can increase the concentration of hydrogen ions (H+) in a solution. As a result, they lower the pH, making the environment more acidic.
  • Examples of acidic substances include vinegar (acetic acid), lemon juice (citric acid), and battery acid (sulfuric acid).
  • In the body, ketoacids are important acidic substances that are produced during the breakdown of fats, especially in diabetic patients.

Understanding how these substances interact with the blood can help us see how they affect overall health.
ketones
Ketones are specific types of acidic substances produced in the body during fat metabolism. They are usually made when glucose, the body's primary energy source, is in short supply.
  • In diabetes, when the body's ability to use glucose is impaired, it breaks down fats for energy, leading to the production of ketones.
  • The most common ketones are acetoacetate, beta-hydroxybutyrate, and acetone.
  • While small amounts of ketones can be safely used by the heart, brain, and muscles, high levels build up in the blood, causing a condition known as ketoacidosis.

Ketoacidosis can significantly lower the blood pH, making the blood more acidic.
hydrogen ion concentration
Hydrogen ion concentration determines the acidity or alkalinity of a solution, measured by pH.
  • A higher concentration of hydrogen ions (H+) indicates an acidic solution and results in a lower pH value.
  • A lower concentration means a more basic or alkaline solution, with a higher pH value.

The pH scale ranges from 0 to 14:
  • 0-6.9 is acidic
  • 7 is neutral
  • 7.1-14 is alkaline

Therefore, when ketones increase in the blood, they raise hydrogen ion concentration, thereby lowering the pH and increasing acidity.
blood plasma pH
Blood plasma pH is a critical aspect of maintaining homeostasis in the body. Normal blood plasma pH is tightly regulated between 7.35 and 7.45, which is slightly alkaline.
  • Enzyme function, oxygen transport, and cellular processes all rely on maintaining this pH range.
  • A drop in pH below 7.35 is termed acidosis, while an increase above 7.45 leads to alkalosis.

In severe diabetes, the production of acidic ketones increases hydrogen ion concentration, causing the blood plasma pH to drop, resulting in diabetic ketoacidosis.
fat breakdown
Fat breakdown, also known as lipid metabolism, occurs when the body needs an alternative energy source beyond glucose.
  • Fat stores are broken down into fatty acids and glycerol.
  • Fatty acids are further broken down in a process called beta-oxidation, producing ketones as a by-product.

This process is useful in normal conditions but becomes problematic in uncontrolled diabetes. Continuous fat breakdown and ketone production without sufficient insulin lead to ketoacidosis, making the blood acidic.
Efficient management of blood sugar levels and insulin intake can help control and prevent these severe complications.

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Most popular questions from this chapter

A \(10.0-\mathrm{mL}\) sample of vinegar, which is an aqueous solution of acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\), requires \(16.5 \mathrm{~mL}\) of a \(0.500 \mathrm{M} \mathrm{NaOH}\) solution to reach the endpoint in a titration. What is the molarity of the acetic acid solution? (14.8) $$ \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) $$

Consider the following acids and their dissociation constants: $$ \begin{array}{r} \mathrm{HPO}_{4}{ }^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{PO}_{4}{ }^{3-}(a q) \\ K_{\mathrm{a}}=2.2 \times 10^{-13} \\ \mathrm{HCHO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{CHO}_{2}^{-}(a q) \\ K_{\mathrm{a}}=1.8 \times 10^{-4} \end{array} $$ a. Which is the weaker acid, \(\mathrm{HPO}_{4}^{2-}\) or \(\mathrm{HCHO}_{2}\) ? b. What is the conjugate base of \(\mathrm{HPO}_{4}^{2-}\) ? c. Which acid has the weaker conjugate base? d. Which acid has the stronger conjugate base? e. Which acid produces more ions?

Calculate the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) for a solution with each of the following \(\mathrm{pH}\) values: \((14.6)\) a. \(2.2\) b. \(7.2\) c. \(10.6\) d. \(12.1\)

$$ \begin{aligned} &\text { Complete the following table: (14.2) } \\ &\begin{array}{ll} \text { Acid } & \text { Conjugate Base } \\ \text { HI } & \\ & \mathrm{Cl}^{-} \\ \mathrm{NH}_{4}^{+} & \\ & \mathrm{HS}^{-} \end{array} \end{aligned} $$

If a base is added to pure water, why does the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) decrease?
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