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Chapter 10: Problem 27

Explain the terms isotonic solution, crenation, and hemolysis.

Short Answer

Expert verified
An isotonic solution is a solution where solute concentration is the same on both sides of a semipermeable membrane, allowing water to move freely without a net movement in or out of the cell. Crenation is the process in which red blood cells shrink due to water loss through osmosis when placed in a hypertonic solution, affecting their ability to transport oxygen effectively. Hemolysis occurs when red blood cells rupture and release their content into the surrounding fluid, typically when placed in a hypotonic solution, leading to potential medical complications like anemia and jaundice.

Step by step solution

01

Isotonic Solution

An isotonic solution is a solution in which the concentration of solutes (such as ions, sugars, or proteins) is the same on both sides of a semipermeable membrane, like the cell membrane. This type of solution allows for the free movement of water across the membrane without causing a net movement of water into or out of the cell. In an isotonic solution, cells are in a state of equilibrium, meaning the rate of water molecules entering the cell is equal to the rate of water molecules leaving the cell. Examples of isotonic solutions include normal saline and some intravenous fluids that are administered to maintain hydration in patients.
02

Crenation

Crenation is the process in which red blood cells (RBCs) shrink due to the loss of water through osmosis when they are placed in a hypertonic solution. A hypertonic solution is a solution with a higher solute concentration compared to the cell's cytoplasm. Due to the higher solute concentration outside the cell, water will move out of the RBCs through the process of osmosis, resulting in a shriveled appearance of the RBCs. This can affect the cells' ability to transport oxygen effectively, leading to potential health problems.
03

Hemolysis

Hemolysis is the process in which red blood cells rupture and release their content, such as hemoglobin, into the surrounding fluid. This can occur when RBCs swell beyond their capacity to maintain their membrane integrity, which typically happens when they are placed in a hypotonic solution. A hypotonic solution is a solution that has a lower solute concentration compared to the cell's cytoplasm. In this case, water will move into the RBCs through the process of osmosis, causing them to swell and eventually burst. Hemolysis can lead to anemia, jaundice, and other medical complications if not managed properly.

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Most popular questions from this chapter

Explain the following on the basis of the behavior of atoms and/or ions. a. Cooking with water is faster in a pressure cooker than in an open pan. b. Salt is used on icy roads. c. Melted sea ice from the Arctic Ocean produces fresh water. d. \(\mathrm{CO}_{2}(s)\) (dry ice) does not have a normal boiling point under normal atmospheric conditions, even though \(\mathrm{CO}_{2}\) is a liquid in fire extinguishers. e. Adding a solute to a solvent extends the liquid phase over a larger temperature range.

You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: "The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil." What do you say to your friend?

a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. $$\begin{array}{|llc|} \hline & \text { Lattice Energy } & \Delta H_{\text {soln }} \\ \hline \mathrm{CaCl}_{2}(s) & -2247 \mathrm{kJ} / \mathrm{mol} & -46 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Cal}_{2}(s) & -2059 \mathrm{kJ} / \mathrm{mol} & -104 \mathrm{kJ} / \mathrm{mol} \\ \hline \end{array}$$ b. Based on your answers to part a, which ion, \(\mathrm{Cl}^{-}\) or \(\mathrm{I}^{-}\), is more strongly attracted to water?

The weak electrolyte \(\mathrm{NH}_{3}(g)\) does not obey Henry's law. Why? \(\mathrm{O}_{2}(g)\) obeys Henry's law in water but not in blood (an aqueous solution). Why?

Calculate the solubility of \(\mathrm{O}_{2}\) in water at a partial pressure of \(\mathrm{O}_{2}\) of 120 torr at \(25^{\circ} \mathrm{C}\). The Henry's law constant for \(\mathrm{O}_{2}\) is \(1.3 \times 10^{-3} \mathrm{mol} / \mathrm{L} \cdot \mathrm{atm}\) for Henry's law in the form \(C=k P\) where \(C\) is the gas concentration (mol/L).
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