Chapter 8 Solutions.

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Presentation transcript:

Chapter 8 Solutions

Solutions and Other Mixtures Heterogeneous Mixtures: Does not have a fixed composition (Particles not distributed evenly) Suspensions: particles are large and settle out Pulp in orange juice Particles may be filtered out

Solutions and Other Mixtures Some mixtures of two liquids will separate Oil, vinegar, and flavoring can be shaken together to make salad dressing. But the dressing is a heterogeneous mixture. When the dressing stands for a few minutes, two layers form. The two liquids separate because they are immiscible, which means they do not mix Oil floats to the top since it is less dense The process of pouring a less dense liquid off a denser liquid is called decanting

Solutions and Other Mixtures

Solutions and Other Mixtures

Solutions and Other Mixtures Colloid: particles are too small to settle out The color in Latex paint comes from solid particles of colored pigments that are dispersed in water Particles small enough to pass through filter Even though particles are small they still scatter light that passes through he colloid (Tyndall effect)

Solutions and Other Mixtures

Solutions and Other Mixtures Other colloids: Dispensing gas in a liquid Whipped cream Dispensing gas in a solid Marshmallows Dispensing of water droplets in air Fog Dispensing of small particles in air smoke

Solutions and Other Mixtures Some immiscible liquids can form colloids Mayonnaise is a colloid made up of tiny droplets of oil suspended in vinegar Egg yolk coats the oil droplets so that they do not join together and form a separate layer Cream is a mixture of oil, proteins, and carbohydrate dispersed in water. The lipid is coated with protein that acts as an emulsifier therefore spread throughout the mixture Emulsion: colloid in which liquids that usually do not mix are spread throughout each other One liquid is dispersed in the other

Solutions and Other Mixtures

Solutions and Other Mixtures

Solutions and Other Mixtures Homogeneous mixtures: look uniform because the individual components of the mixture are too small to be seen Are solutions: all homogeneous mixtures are also solutions Solute: substance that dissolves Solvent: substance in which the solute dissolves Example: salt water

Solutions and Other Mixtures Two or more liquids that form a single layer when mixed are miscible (one liquid is water) Alcohol Beer Drinking alcohol

Solutions and Other Mixtures Liquid solutions that do not contain water Nail polish remover Crude oil Distillation: process that separates miscible liquids

Solutions and Other Mixtures

Solutions and Other Mixtures

Solutions and Other Mixtures Alloys: homogeneous mixture that is usually composed of two or more metals (solids can dissolve in other solids) Metals melted to a liquid and mixed Have properties that the individual metals do not Brass: solution of zinc dissolved in copper metal Bronze: solution of tin in copper metal Steel: metal solution that contains some non-metals (carbon)

How Substances Dissolve

Water Is V-shaped Two hydrogen atoms are located at the same end of the molecule, and oxygen is at the opposite end This arrangement allows oxygen to pull the shared electrons toward itself and away from the two hydrogen atoms The electron pairs are NOT shared equally, but spend more time in the vicinity of oxygen Because electrons are negatively charged, the oxygen end of the molecule is slightly more negative and the hydrogen end slightly more positive Because water has two poles of charge, it is a polar molecule, or dipole

COVALENT BONDS

Polar and Nonpolar Molecules Polar molecules orient themselves toward other dipoles or toward charged particles (such as ions and some proteins), and they play essential roles in chemical reactions in body cells

Polar and Nonpolar Molecules Different molecules exhibit different degrees of polarity, and we can see a gradual change from ionic to nonpolar covalent bonding Extremes: Ionic bonds: complete electron transfer Nonpolar covalent bonds: equal electron sharing There are various degrees of unequal sharing in between

IONIC/POLAR/NONPOLAR

Hydrogen Bonds Weak attractions that form between partially charged atoms found in polar molecules Hydrogen bonds form when a hydrogen atom, already covalently linked to one electronegative atom (usually nitrogen or oxygen), is attracted by another electron-hungry atom, and forms a bridge between them Common between dipoles such as water molecules, because the slightly negative oxygen atoms of one molecule attract the slightly positive hydrogens of the other molecules

HYDROGEN BOND

Hydrogen Bonds Surface tension is due to hydrogen bonds between water molecules Although hydrogen bonds are too weak to bind atoms together to form molecules, they are important as Intramolecular bonds, which bind different parts of a single large molecule together into a specific three-dimensional shape Some large biological molecules, such as proteins and DNA, have numerous hydrogen bonds that help maintain and stabilize their structures

How Substances Dissolve Like dissolves like: means that a solvent will dissolve substances that have molecular structures that are like the solvent’s structure Polar dissolve polar Many substance dissolve in water (universal solvent) +/- charges attract charges of solute Nonpolar dissolves nonpolar Nonpolar substances usually do not dissolve in water Nonpolar molecules do not have partially negative and positively parts because the electrons are distributed evenly over the whole molecule Nonpolar solvents must be used to dissolve nonpolar materials Oil based paint must be dissolved by nonpolar solvent

How Substances Dissolve

How Substances Dissolve The dissolving process: Kinetic theory of matter states that molecules are always moving The energy transferred from the solvent to the solute, as well as the attractive forces between the solvent and solute molecules, causes molecules at the surface of the substance to dissolve

How Substances Dissolve The dissolving process: Solutes with a larger surface area dissolve faster Small pieces of a solid dissolve faster than large pieces of the same solid (small pieces have a larger surface area) Cube of 1 cm on each edge Each face has an area of 1 cm2 6 surfaces= total surface area of 6 cm2 Large Cube broken down to smaller cubes of 0.1 cm on each edge Each face has an area of 0.01 cm2 6 surfaces= total surface area of 0.06 cm2 Total surface of 1,000 cubes is 1,000 x 0.06cm2 = 60 cm2 Which is 10 times the surface area of the larger cube

How Substances Dissolve Surface area to volume ratio SA/Vol

How Substances Dissolve

How Substances Dissolve The dissolving process: Stirring or shaking helps solids dissolve faster Solids dissolve faster when the solvent is hot

How Substances Dissolve Solutes affect the physical properties of a solution Boiling point of water is 1000C and the freezing point is 00C If you add salt (NaCl) the boiling point will increase and the freezing point will decrease Cooking and melting winter ice Ethylene glycol (antifreeze) in car Raising boiling point and lowers freezing point

Solubility and Concentration Solubility of a substance is the maximum mass of a solute that can dissolve in 100 g of solvent at a certain temperature and standard atmosphere pressure Different substances have different solubilities in water Depends on the on the strength of the forces acting between the solute particles and the strength of the forces acting between water molecules and solute particles

Solubility and Concentration

Solubility and Concentration How much of a substance is in a solution? Concentration: the amount of a particular substance in a given quantity of a mixture, solution, or ore: Not quantitative terms: Concentrated: large amount of solute Dilute: small amount of solute Saturated: dissolved solute is in equilibrium with undissolved solute. So, if you add more solute, it just settles to the bottom of the container Heating can dissolve more solute (supersaturated) Unsaturated: least than the maximum amount of solute

Solubility and Concentration Temperature and pressure affect the solubility of gases Temperature: Unlike solids, gases are less soluble in warmer water Fish??? Pressure: High: more gas dissolves Low: less gas dissolves Example: Carbonated drink Scuba diver (bends)

Solubility and Concentration Concentration of solutions Terms concentrated, dilute, saturated, and unsaturated do not reveal the quantity of dissolved solute One of the most common ways of expressing the concentration of a solution is molarity Molarity is expressed as moles of solute per liter of solution

Solubility and Concentration Molarity = moles of solute/liters of solution M = mol/L Example: a 1.0 M is read as one molar solution A 1.0 M solution of NaCl contains 1.0 mol of dissolved NaCl in every 1.0 L of solution

Solubility and Concentration Calculate the molarity of sucrose, C12H22O11, in a solution of 124 g of solute in 0.500 L of solution Moles C12H22O11 = mass C12H22O11/molar mass C12H22O11 Molarity = moles C12H22O11 / liters of solution Molar mass C12H22O11= 342 g Moles C12H22O11= 124 g / 342g/mol = 124g x 1mol/342g = 0.362 mol Molarity of solution=0.362 molC12H22O1 1 / 0.500 L solution=0.724 M