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Chapter 21: Problem 19

Distinguish between the terms deliquescent and hygroscopic.

Short Answer

Expert verified
Deliquescent substances dissolve in absorbed moisture, forming a solution; hygroscopic substances absorb moisture without dissolving.

Step by step solution

01

Define Deliquescent Substances

Deliquescent substances are materials that have the ability to absorb moisture from the air to the extent that they dissolve in the absorbed water. They form a solution as they take up moisture. Common examples include calcium chloride and magnesium sulfate.
02

Define Hygroscopic Substances

Hygroscopic substances are those that absorb moisture from the air but do not dissolve in the absorbed moisture. These substances just attract and hold water molecules from the surrounding environment. Common examples include silica gel and glycerol.
03

Compare Absorption and Solubility

The key difference is in solubility upon moisture absorption. Deliquescent substances not only absorb water but also become a liquid solution, while hygroscopic substances do not dissolve.

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Key Concepts

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

Deliquescent Substances
Deliquescent substances are fascinating because they can transform into a liquid state simply by absorbing moisture from the air. These substances don't just attract water; they absorb it until they dissolve completely. This is why you'll often find them in a saturated or liquid form once exposed to humid environments.

Common examples of deliquescent substances include calcium chloride and magnesium sulfate. Next time you see these substances, remember their magic-like ability to seemingly melt into water through moisture absorption. They are distinct because they ensure they don't just soak up water but completely dissolve, forming a liquid solution.
Hygroscopic Substances
Hygroscopic substances are avid water seekers, pulling moisture from the air but not going as far as to dissolve in it. These materials maintain their solid state, although they may become slightly damp. Unlike deliquescent substances, hygroscopic ones stop short of forming a liquid.

Some typical examples are silica gel packs, often used to keep products dry, and leaves of plants designed to pull in as much air moisture as possible. While they do not dissolve in the moisture they attract, they essentially work as mini dehumidifiers.
Moisture Absorption
Moisture absorption is a process where substances draw in water from the surrounding air. Both deliquescent and hygroscopic substances are experts at this. However, their methods of dealing with the absorbed moisture differ.

Understanding this absorption is crucial in multiple industries, such as packaging and chemical processing, where control of humidity can be paramount. So, whether you鈥檙e encountering water-absorbing salts or the silica packs in your shoebox, they are all leveraging moisture absorption to achieve their goal.
Solubility Differences
When it comes to solubility differences, deliquescent and hygroscopic substances each have unique characteristics. Deliquescent substances take in moisture until they dissolve completely, becoming a solution. This means they have a solubility threshold that, once reached, causes them to transition to a liquid state.

Hygroscopic substances, in contrast, can absorb moisture to a certain degree without dissolving. They stay in their original form but may bulk up slightly or become damp to the touch. These solubility differences are critical in certain applications, such as in controlling fine consistency and moisture levels in manufacturing processes.

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Most popular questions from this chapter

An absorption in an IR spectrum of an organic compound comes at \(3100 \mathrm{cm}^{-1}\) and is assigned to an \(\mathrm{X}-\mathrm{H}\) bond where \(\mathrm{X}=\mathrm{C}, \mathrm{O}\) or \(\mathrm{N}\). Determine the shift in this band upon deuteration of the \(X-H\) bond for (a) \(\mathrm{X}=^{12} \mathrm{C}\), \((b) X=^{16} O\) and \((\mathrm{c}) \mathrm{X}=^{14} \mathrm{N}\)

For each of the following molecules \(\mathrm{EH}_{n}:\) state whether the \(\mathrm{E}-\mathrm{H}\) bond is polar and if \(\mathrm{so},\) show in which direction the dipole moment acts; and state whether the molecule is polar and if so, indicate the direction of the resultant molecular dipole moment: (a) \(\mathrm{CH}_{4}\) (b) \(\mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{BH}_{3}\) (d) \(\mathrm{NH}_{3}\) (e) \(\mathrm{SiH}_{4}\) (f) \(\mathrm{HCl}\) \((\mathrm{g}) \mathrm{H}_{2} \mathrm{Se}\)

What is the oxidation state of nitrogen in (a) \(\mathrm{NH}_{3}\) (b) \(\left[\mathrm{NH}_{4}\right]^{+},(\mathrm{c}) \mathrm{N}_{2} \mathrm{H}_{4}\) and \((\mathrm{d})\left[\mathrm{NH}_{2}\right]^{-} ?\)

'Hard water' is a characteristic of areas where limestone \(\left(\mathrm{CaCO}_{3}\right)\) is present and contains \(\mathrm{Ca}^{2+}\) ions. The following equilibrium describes how calcium ions are freed into the tap-water: \\[ \begin{aligned} \mathrm{CaCO}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g}) & \rightleftharpoons \\ \mathrm{Ca}^{2+}(\mathrm{aq}) &+2\left[\mathrm{HCO}_{3}\right]^{-}(\mathrm{aq}) \end{aligned} \\] Carbon dioxide is less soluble in hot water than cold water. Use these data to explain why scales of calcium carbonate form inside a kettle when the tap-water is hard.

Discuss how hydrogen bonding affects the properties of \(\mathrm{HF}\) and \(\mathrm{H}_{2} \mathrm{O}\) with respect to \(\mathrm{HCl}\) and \(\mathrm{H}_{2} \mathrm{S}\)
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