Which saturated solution would be most dilute

It's also critical to use units with any values to ensure the correct dosage of medications or report levels of substances in blood, to name just two. Another way of looking at concentration such as in IV solutions and blood is in terms of equivalents.

One equivalent is equal to one mole of charge in an ion. The value of the equivalents is always positive regardless of the charge. Equivalents are used because the concentration of the charges is important than the identity of the solutes. For example, a standard IV solution does not contain the same solutes as blood but the concentration of charges is the same. What mass of sodium did the patient receive? Note that if this problem had a different ion with a different charge, that would need to be accounted for in the calculation.

Allison Soult , Ph. Department of Chemistry, University of Kentucky. Learning Outcomes Define concentration. Use the terms concentrated and dilute to describe the relative concentration of a solution.

Calculate the molarity of a solution. Use concentration units in calculations. Determine equivalents for an ion. Complete calculations relating equivalents to moles, volumes, or mass.

Complete dilution calculations. Percent Concentration One way to describe the concentration of a solution is by the percent of the solution that is composed of the solute. Volume Percent The percentage of solute in a solution can more easily be determined by volume when the solute and solvent are both liquids. Parts per Million and Parts per Billion Two other concentration units are parts per million and parts per billion. Molarity Chemists primarily need the concentration of solutions to be expressed in a way that accounts for the number of particles present that could react according to a particular chemical equation.

Solution Step 1: List the known quantities and plan the problem. Step 2: Solve. If the added solute dissolves, then the original solution was unsaturated. A solution that has been allowed to reach equilibrium but which has extra undissolved solute at the bottom of the container must be saturated.

Watch the video at the link below and answer the following questions:. Skip to main content. Search for:. Define unsaturated solution. Define solution equilibrium.

How do you make sure a compound is pure? Summary Saturated and unsaturated solutions are defined. Solution equilibrium exists when the rate of dissolving equals the rate of recrystallization. What is the heat source for evaporation? Why does the salt precipitate out of solution? Review Why is the preferred equation for solution equilibrium of NaCl an equilibrium between solid NaCl and the ions.

If I add water to a saturated sucrose solution, what will happen? If I heat a solution and remove water, I see crystals at the bottom of the container. As a result, nonpolar gases are less soluble in polar solvents than in nonpolar solvents.

This is precisely the trend expected: as the gas molecules become larger, the strength of the solvent—solute interactions due to London dispersion forces increases, approaching the strength of the solvent—solvent interactions. Virtually all common organic liquids, whether polar or not, are miscible.

If the predominant intermolecular interactions in two liquids are very different from one another, however, they may be immiscible.

Just because two liquids are immiscible, however, does not mean that they are completely insoluble in each other. For example, mg of benzene dissolves in mL of water at Only the three lightest alcohols methanol, ethanol, and n-propanol are completely miscible with water. As the molecular mass of the alcohol increases, so does the proportion of hydrocarbon in the molecule. Correspondingly, the importance of hydrogen bonding and dipole—dipole interactions in the pure alcohol decreases, while the importance of London dispersion forces increases, which leads to progressively fewer favorable electrostatic interactions with water.

Organic liquids such as acetone, ethanol, and tetrahydrofuran are sufficiently polar to be completely miscible with water yet sufficiently nonpolar to be completely miscible with all organic solvents. The same principles govern the solubilities of molecular solids in liquids. In contrast, glucose contains five —OH groups that can form hydrogen bonds. The structure of one isomer of glucose is shown here.

These hydrocarbons are therefore powerful solvents for a wide range of polar and nonpolar compounds. In contrast, the solubility of ionic compounds is largely determined not by the polarity of the solvent but rather by its dielectric constant, a measure of its ability to separate ions in solution, as you will soon see. Identify the most important solute—solvent interactions in each solution. Identify all possible intermolecular interactions for both the solute and the solvent: London dispersion forces, dipole—dipole interactions, or hydrogen bonding.

Determine which is likely to be the most important factor in solution formation. A hydrophilic substance is polar and often contains O—H or N—H groups that can form hydrogen bonds to water. For example, glucose with its five O—H groups is hydrophilic. In contrast, a hydrophobic substance may be polar but usually contains C—H bonds that do not interact favorably with water, as is the case with naphthalene and n-octane. Hydrophilic substances tend to be very soluble in water and other strongly polar solvents, whereas hydrophobic substances are essentially insoluble in water and soluble in nonpolar solvents such as benzene and cyclohexane.

The difference between hydrophilic and hydrophobic substances has substantial consequences in biological systems. For example, vitamins can be classified as either fat soluble or water soluble. Fat-soluble vitamins, such as vitamin A, are mostly nonpolar, hydrophobic molecules. As a result, they tend to be absorbed into fatty tissues and stored there. In contrast, water-soluble vitamins, such as vitamin C, are polar, hydrophilic molecules that circulate in the blood and intracellular fluids, which are primarily aqueous.

Water-soluble vitamins are therefore excreted much more rapidly from the body and must be replenished in our daily diet. A comparison of the chemical structures of vitamin A and vitamin C quickly reveals why one is hydrophobic and the other hydrophilic. Because water-soluble vitamins are rapidly excreted, the risk of consuming them in excess is relatively small.

Eating a dozen oranges a day is likely to make you tired of oranges long before you suffer any ill effects due to their high vitamin C content. In contrast, fat-soluble vitamins constitute a significant health hazard when consumed in large amounts. For example, the livers of polar bears and other large animals that live in cold climates contain large amounts of vitamin A, which have occasionally proven fatal to humans who have eaten them. Using what you know of hydrophilic and hydrophobic solutes, classify each as water soluble or fat soluble and predict which are likely to be required in the diet on a daily basis.

Asked for: classification as water soluble or fat soluble; dietary requirement. Based on the structure of each compound, decide whether it is hydrophilic or hydrophobic. If it is hydrophilic, it is likely to be required on a daily basis. These compounds are consumed by humans: caffeine, acetaminophen, and vitamin D. Identify each as primarily hydrophilic water soluble or hydrophobic fat soluble , and predict whether each is likely to be excreted from the body rapidly or slowly.

Caffeine and acetaminophen are water soluble and rapidly excreted, whereas vitamin D is fat soluble and slowly excreted. Solutions are not limited to gases and liquids; solid solutions also exist.