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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.

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Most popular questions from this chapter

How do the solubilities of most ionic compounds in water change with temperature?

What is the effect of pressure on the solubility of a liquid in liquid and of a solid in liquid?

A protein has been isolated as a salt with the formula \(\mathrm{Na}_{20} \mathrm{P}\) (this notation means that there are \(20 \mathrm{Na}^{+}\) ions associated with a negatively charged protein \(\mathrm{P}^{20-}\) ). The osmotic pressure of a 10.0 -mL solution containing \(0.225 \mathrm{~g}\) of the protein is \(0.257 \mathrm{~atm}\) at \(25.0^{\circ} \mathrm{C}\). (a) Calculate the molar mass of the protein from these data. (b) What is the actual molar mass of the protein?

Arrange these aqueous solutions in order of decreasing freezing point and explain your reasons: (a) \(0.50 \mathrm{~m}\) \(\mathrm{HCl},\) (b) \(0.50 \mathrm{~m}\) glucose, (c) \(0.50 \mathrm{~m}\) acetic acid.

Basing your answer on intermolecular force considerations, explain what "like dissolves like" means.
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