Chapter 8 Solutions, Acids, and Bases

8-1 Formation of Solutions Substance can dissolve in water three ways-by ___________, ____________, and_________ A ____________ is a substance whose particles are dissolved in a solution. The substance in which the solute dissolves is called the __________. Ex: Seawater Solute = is the_________ Solvent = is the___________

Solutes/Solvents Solutes and solvents can take the form of a _________, ________ or ______ The solution takes the_________ of the solvent.

Dissociation of Ionic Compounds ______________ is the process in which an ionic compound separates into ions as it dissolves. For a solute to dissolve in water, the solute and solvent particles must________ one another. Before a _________ can form, the attractions that hold the solute together and the solvent together must be ___________

Dispersion of Molecular Compounds Sugar dissolves in water by _______, or breaking into small pieces that spread throughout the water. Ex: piece of ________ disperses throughout your mouth _______ in saliva dissolves the________ and flavoring in the candy.

Process of Dispersion When enough ________molecules surround a sugar molecule, the attractions between them are great enough to overcome the attractions holding the _______ molecule to the surface of the crystal. The sugar molecule ________ free, and is pulled into solution by the water molecules, then another layer if sugar molecules is exposed to the water

Ionization of Molecular Compounds The process in which neutral molecules gain or lose electrons is known as _____________. Dissolving by ionization is a _________ change. The solution that results contains______ substances. When a solute dissolves by ionization, the ions in solution are formed by the reaction of _______ and _________ particles.

Example of Ionization When _______ and____________form a solution, two molecular compounds react to form two ions. Ions formed are H 3 O + and Cl - Drawing

Answer the following Questions 1.What are three ways that substances can dissolve in water? 2.How does sugar dissolve in water?

8-1 Continued Properties of Liquid solutions Three physical properties of a solution that can differ from those of its solute and solvent are: 1._____________ 2._____________ 3._____________

Conductivity _______ sodium chloride is a _______ conductor of electricity Sodium chloride _________ in water and the ions formed can move freely enabling them to_________ electricity

Freezing Point The __________ point of water at sea level is 0 degrees Celsius Example : icy roads are salted with magnesium chloride, the resulting solution can have a freezing point as low as __________degrees Celsius

Boiling Point A _________ can raise the boiling point of the solvent Example: the __________ used in most car radiators is a solution containing water and ethylene, which raises the boiling point. This helps the engine from ____________.

Heat of Solution During the formation of a solution, energy is either _________ or __________. In order for a solution to form, both the attractions among the _______ particles and the attractions among the _______ particles must be_________ _________ attractions________ energy.

Heat of Solution Continued As the solute dissolves, new attractions _________ between solute and solvent particles. The___________ of attractions __________energy. The difference between these energies is known as____________

Factors Affecting Rates of Dissolving Factors that affect the rate of dissolving include: _________ __________

Surface Area The ________ the surface area of a solid solute, the more frequent the __________ are between solute and solvent particles. More collisions result in________ rate of dissolving

Stirring __________ moves dissolved particles away from the surface of the solid, and allows for more collisions between the solute and solvent particles

Temperature _________ the temperature of the solvent _________ up the dissolving rate. This causes its particles to move faster. As a result, both the number of collisions and the __________ of these collisions with solute particles increase. The ________ goes into the________ more quickly.

Section 8-1 Review Using your book complete the following questions: Page 257 Numbers 1,2,3,4,5

Section 8-2 The maximum amount of a solute that dissolves in a given amount of solvent at a constant temperature is called___________ Ex: _______ in lemonade Knowing the solubility of a substance can help you classify solutions based on how much _________ they contain.

Solubility Solutions are described as: ___________, ___________ depending on the amount of______ in solution.

Saturated Solutions Table sugar is very _________ in water A _________ solution is one that contains as much solute as the solvent can hold at a given temperature. When a solution is saturated, the solvent is “_________” with solute. If you add more solute, it will___dissolve.

Unsaturated Solutions A solution that has______ than the maximum amount of solute that can be dissolved is called an _________ solution. Example: many_________ you drink are unsaturated solutions of sugar in water. As long as the amount of solute is less than the___________at that temperature, the solution is _________

Supersaturated Solutions A____________ solution is one that contains more solute than it can normally hold at a given temperature. Supersaturated solutions are very __________. Ex: Carrying a stack of________

Review Questions What terms are used to describe solutions with different amounts of solute. How does a supersaturated solution differ from a saturated solution?

How Cold Packs Work Read page 233 in your book Discussion

8-2 Continued Factors Affecting Solubility Three factors that affect the solubility of a solute are: 1._________________ 2._________________ 3._________________

Polar and Nonpolar Solvents Oil does not dissolve in water because oil molecules are_______ and water molecules are ________ A common guideline for predicting solubility is “like ________like” __________ formation is more likely to happen when the solute and solvent are either both polar or both nonpolar

Temperature In general, the solubility of solids________ as the solvent temperature ___________. Example: sugar added to______tea verses _____tea _______usually become less soluble as the temperature of the solvent increases

Pressure _______ the _______ on a gas________ its solubility in a liquid Carbonated beverages, uses pressure to force CO 2 to dissolve in the liquid The _______ of CO 2 in a sealed 12-ounce can of soda at room temp can be two to three times atmospheric__________.

Concentrations of Solutions The __________ of a solution is the amount of solute ________in a specified amount of solution Concentrations can be expressed as percent by ________, percent by________, and________.

Percent by Volume Percent by Volume = Volume of solute x 100% Volume of solvent Example the volume of the solute is 10 L and the volume of the solvent is 30 L. What is the percent by volume?

Percent by Mass Concentration expressed as a percent by mass is ________ useful when the solute is a solid. Percent by mass = Mass of solute x 100% Mass of solution Example: Suppose you have 100grams of a solution of sugar in water. After allowing the water to evaporate, 15 grams of sugar remains. What is the percent by mass?

Molarity ________ is the number of moles of a solute dissolved per liter of a solution. Molarity = moles of solute x 100% Liters of solution

Example of Molarity To make 1-molar (_____) of solution of sodium chloride in water 1.First calculate the molar mass of the solute (NaCl) = _________ 2.If 58.5 grams of sodium chloride is mixed with enough water to make_________ of solution, the resulting solution is 1-molar.

Complete the following Questions Page 239 questions 1,2,3,4

8-3 Properties of Acids and Bases There are several differences among _______solutions, ______solutions, and solutions that have properties________ an acid or nor a base

Identifying Acids An ________is a compound that produces hydronium ions (_____) when dissolved in water. Ex: HCl + H 2 O  H 3 O + + Cl - Some general properties of acids include _________, ________ with metals, and ability to produce ________________

Sour Taste Foods that taste _______ often contain acids Ex: ________, grapefruits, limes, and ________ all contain________acid. _______contains ________ acid. _______ products that have______contain ______ acid

Reactivity with Metals When you use _______ foil to cover a bowl of leftover spaghetti sauce or other foods containing________ the foil often turns_______. ________contain _______acid, which _________ with metals such as aluminum

Reactivity with Metals The reaction between an acid and a metal is an example of _______ replacement reaction. Ex: ______ is added to hydrochloric acid. Zn +2HCl  H 2 + ZnCl 2 As zinc replaces hydrogen in hydrochloric acid, ________ gas and____________ is produced

Color Changes in Indicators An __________ is any substance that changes color in the presence of an _____ or_______. One of the most common indicators used is________, a kind of_______ derived from plants called lichens. Litmus________is made by coating strips of paper with litmus. _______litmus paper turns________in the presence of an _____.

Testing Acids on litmus paper Observations Vinegar – HCl – Sulfuric Acid- Acetic Acid -

Identifying Bases Sodium hydroxide, ________ is an example of a base. A _______ is a compound that produces hydroxide (_____) when dissolved in water. _______  Na + + OH -

Bases ______ have certain______ and ________ properties that you can use to identify them. Some general properties of bases include ________, _______, and ability to produce ___________ in indicators

Properties of Bases ____________ _____________________

Bitter Taste ______ chocolate (without the sugar) Cough___________ and other liquid medicines

Slippery Feel Bases feel ______. Wet ________ and many___________products that contain bases are slippery to the touch. When wet, some ________ feel slippery because water dissolves compounds trapped in the rocks, producing a basic solution.

Color changes in Indicators Bases turn_____litmus paper_____. Observations of bases NaOH – Ba(OH) 2- NH 4 OH-

Flowers Hydrangeas color changes based on whether they are grown in acidic or basic soil Acidic – flowers are bluish-purple Basic – flowers are pink

End of 8-3 Neutralization and Salts _______contains bases that can leave a bitter taste. Lemon juice contains an______called citric acid. Squeezing lemon juice on fish makes it taste ________bitter The reaction between an acid and a base is called _____________

Neutralization During neutralization, the_________ ions in an ______ combine with the_________ions in a ________to produce an ionic compound called a ______ The hydronium ions from the acid combine with the hydroxide ions from the base to produce__________. The neutralization reaction between an acid and a base produces a________and__________.

Example of neutralization (H 3 O + + Cl - ) + Na + + OH - )  2HOH + (Na + + Cl - ) _____ _______ _______ _____ Other common salts that are produced during neutralization are: 1.Potassium chloride – ______ – salt substitute 2.Potassium iodide – ______- added to table salt to prevent iodine deficiency 3.Magnesium Chloride –_______ – De-icer for roads

Proton Donors and Acceptors Acids lose or “_______” protons Bases “_______” protons, forming water, a neutral molecule. ______can be defined as proton _____, and _______ can be defined as proton _________. Example_______can act either as an acid or base depending on the compound with which it reacts.

Water acting as an acid and a base Complete the following examples from the board.

8-4 Strengths of Acids and Bases Chemists use a number scale from _______ to______to describe the concentration of __________ ions in a solution. It is known as the_____________. The _______of a solution is a measure of its hydronium ion concentration.

pH scale A pH of _____indicates a ______ solution. ______ have a pH______ than 7 _______have a pH______than 7 See Figure 22

pH scale ______ is neutral because it contains small but ________ concentrations of hydronium ions and hydroxide ions. The _______the pH value, the_______ the H 3 O + ion concentration in solution is. The ________ the pH value, the______ the H 3 O + ion concentration is.

Strong Acids and Bases When certain acids and bases dissolve in water, the formation of ions from the solute______ goes to ________. Such acids and bases are classified as _______.

Strong Acids When strong ________ dissolve in water, they ionize almost completely. Ex: _______= hydrochloric acid _______ = sulfuric acid _______ = nitric acid

Strong Bases Strong________ dissociate almost completely in water. Examples of strong bases: ________ – sodium hydroxide ________ - calcium hydroxide ________ – potassium hydroxide

Beaker Breaker 1.Acids have a pH range from ________to ___________ 2.Name one property of a base _______________ 3.Compare the pH values of acids, bases, and pure water.

Weak Acids and Bases Weak ______ and_______ ionize or dissociate only ________ in water The citric acid in orange ________and the acetic acid in_________ are_________acids. __________and________ contain weak ________.

Concentration verses strength ___________ is the amount of solute dissolved in a given amount of solution. _________ refers to the solute’s tendency to form ions in water.

Weak Acids A weak acid forms ________ hydronium ions than a strong acid of the same concentration. A weak acid has a ________ pH than a strong acid of the same concentration.

Weak Bases Follows the same concept as weak acids. Example is NH 3 (ammonia) because when it dissolves in water, very little of it_________.

Buffers Weak acids and bases can be used to make ___________. A ________ is a solution that is ___________to large changes in pH. Buffers can be prepared by_______ a _______acid and its______or a ________ base and its _______.

Electrolytes An __________ is a substance that ionizes or dissociates into ions when it dissolves in water. The resulting solution can conduct__________ current. Electrolytes in sports drinks help _____________the balance of ions in your body.

Electrolytes Strong acids and bases are strong electrolytes because they dissociate or ionize almost__________ in water. Ex: sodium hydroxide (______) is a strong ___________ that produces many ions in water. Acetic acid is a weak electrolyte because it only________ ionizes.

Examples of Electrolytes _____________ and other portable devices that produce electricity also contain electrolytes. _______batteries use lead plates in combination with the electrolyte sulfuric acid to produce _________. Space shuttles use devices called________ Fuel cells use the strong _______ potassium hydroxide as an electrolyte.

Testing strong weak acids verses strong weak bases on litmus paper Observations Test #1 Test #2 Test# 3 Test#4