Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 48

Explain why it is essential that fluids used in intravenous injections have approximately the same osmotic pressure as blood.

Short Answer

Expert verified
Intravenous fluids must have osmotic pressure similar to blood to prevent damage to blood cells through shrinkage or bursting, ensuring the safe and effective delivery of the treatment.

Step by step solution

01

Understanding Osmotic Pressure

Osmotic pressure is the pressure required to prevent the movement of water across a semipermeable membrane via osmosis. In biological systems, the cell membrane is semipermeable; it allows the free passage of water but limits the movement of solutes. Osmosis naturally occurs from an area of low solute concentration to an area of high solute concentration.
02

Realizing the Importance of Osmotic Pressure Balance

Having the same osmotic pressure (isotonic) is important for any fluid that will be brought into the body, such as through intravenous injections. If the fluid injected has a higher osmotic pressure (hypertonic), water would move from the blood cells into the fluid, causing the cells to shrink or crenate. Conversely, if the fluid has a lower osmotic pressure (hypotonic), water would move into the blood cells, causing them to swell and potentially burst (lysis). Both situations can be highly detrimental to the individual's health.
03

Observing the Outcome

Therefore, intravenous fluids must maintain an osmotic pressure similar to blood. This balance prevents harm to the cells and allows the intended function of the fluid (e.g., delivering medicine or electrolytes) to occur efficiently and safely.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

A man bought a goldfish in a pet shop. Upon returning home, he put the goldfish in a bowl of recently boiled water that had been cooled quickly. A few minutes later the fish was dead. Explain what happened to the fish.

Define boiling-point elevation and freezing-point depression. Write the equations relating boilingpoint elevation and freezing-point depression to the concentration of the solution. Define all the terms, and give their units.

The density of an aqueous solution containing 10.0 percent ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) by mass is \(0.984 \mathrm{~g} / \mathrm{mL}\). (a) Calculate the molality of this solution. (b) Calculate its molarity. (c) What volume of the solution would contain 0.125 mole of ethanol?

What is Henry's law? Define each term in the equa. tion, and give its units. Explain the law in terms of the kinetic molecular theory of gases.

Explain why the solution process invariably leads to an increase in disorder.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free