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Chapter 4: Problem 70

What are common solubility units?

Short Answer

Expert verified
Answer: The common solubility units used in chemistry include: 1. Molarity (M), which represents the number of moles of solute per liter of solution. 2. Mass/volume percentage (mass%), referring to the mass of solute in a given volume of solution. 3. Mass/mass percentage (mass%), which is the mass of solute in the total mass of the solution. 4. Volume/volume percentage (vol%), referring to the volume of solute in the total volume of the solution. 5. Molality (m), which represents the number of moles of solute per kilogram of solvent. 6. Mole fraction (X), denoting the ratio of the number of moles of solute to the total number of moles in the solution.

Step by step solution

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1. Molarity (M)

Molarity is the number of moles of solute dissolved in one liter of the solution. It is a commonly used solubility unit and is expressed in moles per liter (mol/L or M).
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2. Mass/volume percentage (mass%)

Mass/volume percentage refers to the mass of solute dissolved in a given volume of solution, typically expressed as a percentage. It is commonly designated as mass% or m/v%. You may see examples like 5% w/v NaCl, which means 5 grams of sodium chloride (NaCl) have been dissolved in 100 mL of the solution.
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3. Mass/mass percentage (mass%)

Mass/mass percentage is the mass of solute dissolved in the total mass of the solution, generally expressed as a percentage. It is often designated as mass% or m/m%. For instance, a 10% w/w solution of sugar means that 10 grams of sugar are dissolved in 90 grams of water, making a 100-gram solution.
04

4. Volume/volume percentage (vol%)

Volume/volume percentage refers to the volume of solute dissolved in the total volume of the solution, typically expressed as a percentage. It is commonly designated as vol% or v/v%. For example, a 40% v/v ethanol solution means that 40 mL of ethanol is dissolved in 60 mL of water, yielding a 100 mL solution.
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5. Molality (m)

Molality is the number of moles of solute dissolved in one kilogram of solvent. It is expressed as moles per kilogram (mol/kg) and designated by a lowercase 'm.' Unlike molarity, molality does not change with temperature and pressure, making it ideal for studies involving varying conditions.
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6. Mole fraction (X)

Mole fraction represents the ratio of the number of moles of a solute to the total number of moles in the solution. This unitless quantity is denoted by an uppercase 'X' followed by the solute's subscript. For example, the mole fraction of a solute 'A' would be represented as X_A. These are some of the common units used to express solubility in chemistry. Depending on the specific problem or context, a particular unit may be more suitable or convenient to use than another.

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Key Concepts

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

Molarity
Understanding molarity is essential when mixing chemical solutions. Molarity, denoted by the letter 'M', measures the concentration of a solute in a solution. It is defined as the number of moles of solute dissolved per liter of solution. A higher molarity signifies a more concentrated solution. To calculate molarity, divide the moles of solute by the liters of solution. For example, if you have 1 mole of salt in 1 liter of water, the molarity is 1 M. This is one of the most common measures in chemistry because it easily relates to the volume of the solution, which can be crucial in reactions and dilutions.

Mass/Volume Percentage
Mass/volume percentage is another way to express the concentration of a solution, particularly useful when dealing with solid solutes. This percentage is often denoted as w/v% and it illustrates the mass of the solute in grams per 100 mL of solution. It is calculated by dividing the mass of the solute (in grams) by the volume of the solution (in milliliters), and then multiplying by 100. For instance, if you have a solution labeled as 20% w/v, it means there are 20 grams of the solute in every 100 mL of the solution. This unit is quite practical in medical prescriptions and laboratory preparations where precise volumes are key.

Mass/Mass Percentage
Mass/mass percentage is the ratio of the mass of the solute to the mass of the entire solution, multiplied by 100 to get a percentage. Represented as w/w%, this measure is very useful in mixtures of solids or creams where volume is not a deciding factor. A 15% w/w mixture means that there are 15 grams of solute for every 85 grams of solvent, totaling 100 grams of solution. This unit is favored in solid-state chemistry and pharmaceuticals where the pure volume isn't used as a base for comparison.

Volume/Volume Percentage
Volume/volume percentage, abbreviated as v/v%, is a concentration measure used when both solute and solvent are liquids. It is calculated by dividing the volume of the solute by the volume of the solution and then multiplying by 100. For example, if you have a 70% v/v isopropyl alcohol solution, it means there are 70 mL of isopropyl alcohol in every 100 mL solution. This measure is handy in industries like beverages and perfumery where the mixing ratios of liquids are critical.

Molality
Molality is useful for solving problems under varying temperature and pressure because, unlike molarity, it is not affected by changes in these conditions. Designated by a lowercase 'm', it denotes the number of moles of solute per kilogram of solvent. To find the molality, you divide the moles of solute by the kilograms of the solvent. So, if we dissolve 2 moles of sugar in 0.5 kilograms of water, the molality would be 4 mol/kg. It鈥檚 particularly favored in scenarios involving boiling point elevation and freezing point depression since it offers consistency across different temperatures.

Mole Fraction
The mole fraction is a dimensionless quantity that provides the ratio of the number of moles of one component to the total number of moles in the mixture. Represented as 'X', the mole fraction allows for easy stoichiometric calculations in chemical reactions. If you have a solution with a mole fraction of 0.2 for a solute, it means that the solute makes up 20% of the total moles in the mixture. To find the mole fraction of component A, you would divide the moles of A by the total moles in the solution. Mole fraction is ideal for calculations in gas mixtures and when dealing with equilibrium constants in chemical reactions.

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Most popular questions from this chapter

For each of the following aqueous mixtures, determine which ionic concentrations decrease and which remain the same. a. Sodium chloride and iron(II) chloride are dissolved in \(100 \mathrm{mL}\) of water. b. Equimolar amounts of sodium carbonate and sulfuric acid react. c. Potassium sulfate and barium nitrate are dissolved in \(100 \mathrm{mL}\) of water.

A solution of table salt is a good conductor of electricity, but a solution containing an equal molar concentration of table sugar is not. Why?

How many milliliters of \(0.250 M\) HNO \(_{3}\) are needed to neutralize the following solutions? a. \(25.0 \mathrm{mL}\) of \(0.395 M \mathrm{KOH}\) b. \(78.6 \mathrm{mL}\) of \(0.0100 M \mathrm{Al}(\mathrm{OH})_{3}\) c. \(65.9 \mathrm{mL}\) of \(0.475 M \mathrm{NaOH}\)

Toxic chromate can be precipitated from an aqueous solution by bubbling \(\mathrm{SO}_{2}\) through the solution. How many grams of \(\mathrm{SO}_{2}\) are required to treat \(3.0 \times 10^{8} \mathrm{L}\) of \(0.050 \mathrm{mM} \mathrm{CrO}_{4}^{-} ?\) $$\begin{aligned} &2 \mathrm{CrO}_{4}^{2-}(a q)+3 \mathrm{SO}_{2}(g)+4 \mathrm{H}^{+}(a q) \rightarrow\\\ &\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}(s)+2 \mathrm{H}_{2} \mathrm{O}(\ell) \end{aligned}$$

Rank the conductivities of \(1 M\) aqueous solutions of each of the following solutes, starting with the most conductive: (a) acetic acid; (b) methanol; (c) sucrose (table sugar); (d) hydrochloric acid.
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