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Chapter 12: Problem 16

State whether each of the following refers to a saturated or an unsaturated solution: a. A spoonful of salt added to boiling water dissolves. b. A layer of sugar forms on the bottom of a glass of tea as ice is added.

Short Answer

Expert verified
a. Unsaturated solution. b. Saturated solution.

Step by step solution

01

Identify Point A

Examine if the added salt dissolves in the solution. Since the problem states that the spoonful of salt added to boiling water dissolves, it indicates that the water can accept more solute (salt).
02

Determine the Nature of Point A

Because the salt dissolves completely in the boiling water, the solution can still dissolve more solute, indicating it鈥檚 an unsaturated solution.
03

Identify Point B

Observe the condition where a layer of sugar forms on the bottom of a glass of tea as ice is added. The presence of undissolved sugar means the solution has reached its solubility limit.
04

Determine the Nature of Point B

Since the sugar is no longer dissolving and remains undissolved at the bottom, the solution is saturated, meaning it cannot dissolve any more sugar.

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Key Concepts

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

Solubility
Solubility refers to the capacity of a substance (solute) to dissolve in a solvent. This is an important concept to understand when dealing with solutions. The solubility of a solute depends on various factors:
  • Temperature: Higher temperatures generally increase solubility for solids and liquids.
  • Pressure: This mostly affects gases. Higher pressure increases gas solubility in liquids.
  • Nature of the solute and solvent: The chemical nature of both the solute and solvent plays a crucial role. Water, for example, is good at dissolving salts but not oils.
Understanding these factors will help you determine whether a solution is saturated or unsaturated.
Solvents
A solvent is a substance that dissolves a solute, resulting in a solution. The most common solvent is water, often referred to as the 'universal solvent'. Different solvents can dissolve different kinds of solutes:
  • Water (polar): Good for dissolving ionic compounds and polar solutes.
  • Alcohol: Effective for organic compounds and moderately polar substances.
  • Oil (non-polar): Suitable for dissolving non-polar substances such as fats and oils.
The type of solvent you choose will determine what solutes can be dissolved and affect the properties of your solution.
Solute
A solute is the substance that is dissolved in a solvent to form a solution. Common examples include salt in water and sugar in tea. When considering solutes, keep in mind:
  • Solubility: Check how much of the solute can be dissolved in a given amount of solvent at a specified temperature.
  • Particle Size: Smaller particles dissolve faster because they have a larger surface area relative to their volume.
  • Polarity and Ionic Nature: Like dissolves like. Polar and ionic solutes tend to dissolve in polar solvents, while non-polar solutes dissolve in non-polar solvents.
Recognizing these characteristics of solutes will help you understand and predict their behavior in different solutions.

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Most popular questions from this chapter

Answer the following for the reaction: \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{KCl}(a q) \longrightarrow \mathrm{PbCl}_{2}(s)+2 \mathrm{KNO}_{3}(a q)\) a. How many grams of \(\mathrm{PbCl}_{2}\) will be formed from \(50.0 \mathrm{~mL}\) of a \(1.50 \mathrm{M} \mathrm{KCl}\) solution? b. How many milliliters of a \(2.00 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) solution will react with \(50.0 \mathrm{~mL}\) of a \(1.50 \mathrm{M} \mathrm{KCl}\) solution? c. What is the molarity of \(20.0 \mathrm{~mL}\) of a \(\mathrm{KCl}\) solution that reacts completely with \(30.0 \mathrm{~mL}\) of a \(0.400 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) solution?

A patient needs \(100 . \mathrm{g}\) of glucose in the next \(12 \mathrm{~h}\). How many liters of a \(5 \%(\mathrm{~m} / \mathrm{v})\) glucose solution must be given?

For each of the following solutions, calculate the: a. grams of \(2.0 \%(\mathrm{~m} / \mathrm{m}) \mathrm{NaCl}\) solution that contains \(7.50 \mathrm{~g}\) of \(\mathrm{NaCl}\) b. milliliters of \(25 \%(\mathrm{~m} / \mathrm{v})\) NaF solution that contains \(4.0 \mathrm{~g}\) of \(\mathrm{NaF}\) c. milliliters of \(8.0 \%(\mathrm{v} / \mathrm{v})\) ethanol solution that contains \(20.0 \mathrm{~mL}\) of ethanol

For each of the following solutions, calculate the: a. liters of a \(2.00 \mathrm{M} \mathrm{KBr}\) solution to obtain \(3.00 \mathrm{~mol}\) of \(\mathrm{KBr}\) b. liters of a \(1.50 \mathrm{M} \mathrm{NaCl}\) solution to obtain \(15.0 \mathrm{~mol}\) of \(\mathrm{NaCl}\) c. milliliters of a \(0.800 \mathrm{M} \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) solution to obtain \(0.0500 \mathrm{~mol}\) of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\)

A doctor orders \(100 . \mathrm{mL}\) of \(2.0 \%(\mathrm{~m} / \mathrm{v})\) ibuprofen. If you have \(8.0 \%(\mathrm{~m} / \mathrm{v})\) ibuprofen on hand, how many milliliters do you need?
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