CP Physical Science Chemistry: Bell Work, Notes, Study Guides Mr. Banker Fall 2014 ian_banker@charleston.k12.sc.us http://wandohigh.ccsdschools.com/directory/science/banker_ian/physical_science/ Remind101.com CP Reminders: text @MrBankerCP to (442)333-7101 Name: Block: Clicker Number:
Table of Contents Bell Work............. First 4 pages Periodic Table............. Following Bell Work Syllabus........ Following Periodic Table Unit 1A.1: Metric System... 3 Unit 1A.3: The Nature of Science... 5 Unit 1B.1: States / Phases of Matter... 7 Unit 1B.3: Composition of Matter... 9 Unit 1B.4: Chemical vs Physical: Properties and Changes... 11 Unit 1B.5: Density... 13 Unit 2.1: Atomic Structure... 15 Unit 2.2: Isotopes and Ions... 17 Unit 2.3: Electron Arrangement... 19 Unit 3.1: Periodic Table of Elements... 21 Unit 3.2: Oxidation Numbers and Bonding... 23 Unit 3.3: Bonding: Ionic and Covalent Bonds... 24 Unit 4.1: Balancing Chemical Reactions... 26 Unit 4.2: Chemical Reactions: Energy... 28 Unit 4.3: Types of Chemical Reactions... 30 Unit 5.1: Solutions and Saturation Level... 32 Unit 5.2: Acids and Bases... 34 Study Guides: Unit 1 thru Unit 5.... At end of each unit 2 P a g e
Unit 1A.1: Metric System Further Reference: 1.2 The Way Science Works and 1.3 Organizing Data THE BASICS 1. The 7 SI base units and what each measures: a. ( ) a measure of b. ( ) a measure of c. ( ) a measure of d. ( ) a measure of e. ( ) a measure of f. ( ) a measure of g. ( ) a measure of 2. Every measurement will include PREFIXES 1. The prefixes from largest to smallest: a. ( ) : one is equal to 1000 meters b. ( ) : one is equal to 100 liters c. ( ) : one is equal to 10 grams d. ( ) : one is equal to 1/10 meters e. ( ) : one is equal to 1/100 liters f. ( ) : one is equal to 1/1000 grams 2. Remember, these are always added to the 3. Bases in order: a. 4. And to help you remember: a. CONVERTING UNITS 1. When you are converting from on unit to another, you: a. First, b. Then, 3 P a g e
2. If you move to the (aka: to ) the you move the decimal to the 3. If you move to the (aka: to ) the you move the decimal to the PRACTICE PROBLEMS: 1. 1 meter = hectometers K H Da B D C M 2. 2.5 kilograms = grams K H Da B D C M 3. 17.504 deciliters = decaliters K H Da B D C M 4. 2.16 grams = kilograms K H Da B D C M 5. 3.2 liters = centiliters K H Da B D C M 6. 1 meter = centimeters K H Da B D C M 7. 9.3 decameters = millimeters K H Da B D C M PRECISION AND ACCURACY 1. Precision is 2. Accuracy is 3. Draw a picture of the following: Not accurate and not precise Accurate and not precise Not accurate, but precise both accurate and precise 4. Explain a scenario where you can be precise, but not accurate. 4 P a g e
Unit 1A.3: The Nature of Science Further Reference: 1.1 Nature of Science and 1.2 The Way Science Works SCIENCE 1. The goal of science is to 2. Scientists hypothesize in order to in a certain situation a. Long held assumptions 3. Question everything, but make SCIENTIFIC INQUIRY: a. You must be able to create based on that question 1) 2) 3) a. Hypothesis = 4) WITHIN THE EXPERIMENT: a. Independent variable is i. Example: ii. There can be independent variable b. Dependent variable is i. Example: c. Constants are i. Example: d. Control group is i. Example: e. Experimental group is i. Example: 5 P a g e
f. Scientists i. Repeated Trials to ii. Average the results to 5) a. Your data is b. Evidence is NOT c. Evidence can be or d. Quantitative data is i. 4 examples of quantitative data: e. Qualitative data is i. 4 examples of qualitative data: 6) a. Restate your, and state whether your data or your hypothesis. 7) 6 P a g e
Unit 1B.1: States / Phases of Matter Further Reference: 3.2 Changes of State MATTER 1. Matter is 2. The 4 states of matter are: a. b. c. d. i. Each state of matter is designated by the,, and behavior of the 3. Each state of matter has a different: a. b. c. d. 4. determines the kinetic energy ( and thus the ) of a substance. KINETIC THEORY OF MATTER 1. The Kinetic Theory of Matter: (AKA ) 1. 2. 3. STATES / PHASES OF MATTER 1. Solids: a. Energy: 2. Liquids: 3. Gasses: b. Movement: c. Particle Spacing d. Volume Shape: volume, shape a. Energy: b. Movement: c. Particle Spacing d. Volume Shape: volume, shape a. Energy: b. Movement: i. Enough energy c. Particle Spacing d. Volume Shape: volume, shape 4. Plasma is 7 P a g e
a. Created at i. Seen in b. It is the most abundant state of matter i. NOT the most abundant CHANGES IN STATES / PHASES OF MATTER A. Increase in energy: a. b. B. Decrease in energy: a. b. C. Melting point a. Example: D. Freezing point a. Example: E. Boiling point a. Example: F. condensation a. Example: G. Sublimation a. Example: H. Deposition a. Example: PHASE CHANGE DIAGRAM 1. When changing from solid to liquid, the substance isn t entirely until the graph has a slope 2. At point A the substance is 3. At point B the substance is 4. At point C the substance is 5. At point D the substance is 6. At point E the substance is 8 P a g e
Unit 1B.3: Composition of Matter Further Reference: 2.1 Classifying Matter MATTER 1. Matter is 2. The two categories of matter are: a. b. SUBSTANCES 1. The two categories of substances are: a. b. 2. Elements are a. There are known elements, with of them occurring naturally. b. It is only an element if c. Element symbols are written with the 1 st letter, and the 2 nd letter i. Ex: Hydrogen = Carbon = Calcium = d. Atom is i. All atoms for one element are 3. Compounds are a. They are i. Ex: CO 2 H 2 O NaCl C 6 H 12 O 6 b. If you see 2 different written together with no spaces, it is a c. Physical processes separate compounds d. Compounds have a different and than the elements that make them up e. Molecule is i. These atoms do not need to be. 1. Ex: H-H is a. H 2 O is also a ii. Molecules are the form of a compound that can exist and still have the of that compound 9 P a g e
MIXTURES 1. Mixtures contain that IS NOT together. 2. Mixtures can be 3. The two categories of mixtures are: a. b. 4. Heterogenous Mixtures occur when matter is a. Different parts have easily b. Example:,, c. CAN be 5. Homogenous Mixtures occur when matter is a. Example:,, b. Homogenous mixtures are also called a c. CAN be RECAP 10 P a g e
Unit 1B.4: Chemical vs Physical: Properties and Changes Further Reference: 2.1 Properties of Matter and 2.2 Properties of Matter PHYSICAL 1. Physical properties are any observations that can be made the composition of matter a. Examples include: i. ii. iii. iv. 2. Physical changes are a change in. a. The identity of the element or compound b. make or break bonds. 3. Examples include: a. Any ( ) i. Rubbing alcohol ii. A juice box iii. Butter b. Any ( ) i. Aluminum foil ii. Clay iii. Chewing 4. Signs of a Physical Change include: a. Any b. Change in the c. What you started off with is 11 P a g e
CHEMICAL 1. Chemical properties are any observations that are dependent upon of the object a. Examples include: i. ii. 2. Chemical changes: The substances that are present at the beginning of the reaction are. a. make or break bonds. b. The change 3. Examples include: a. Gasoline b. Car c. Milk d. Bread e. Hydrogen peroxide f. Food digesting g. Any ( ) 4. Signs of a Chemical Change include: a. Bubbles b. something. c. A forms (solid appears) d. A e. The changes f. There is a different 12 P a g e
Unit 1B.5: Density Further Reference: 2.2 Properties of Matter DENSITY 1. Density is defined as b. It is a measure of are in an object c. Basically, it is the within Equation in words Equation in Symbols Units: Mass = ( ) Volume (2 ways) Ruler = ( ) Displacement = ( ) Density (2 ways) Ruler = ( ) Displacement = ( ) DIFFERENT OBJECTS HAVE DIFFERENT DENSITIES 1. Each substance a. It does not matter you have, it will have b. Distilled water has a density of c. Objects with different densities will always interact, with the more dense object and the less dense 2. Is Ice or Distilled Water more dense? because a. Objects with more than a density of will in tap water i. Example: b. Objects with less than a density of will in tap water i. Example: 13 P a g e
DETERMINING DENSITY 1. Step 1: 2. Step 2: a. 2 ways to determine volume: i. ii. 3. Step 3: PRACTICE PROBLEMS: Show: the formula, your work, and an answer, include units. 1. If the mass of an object is 35 grams and it takes up 7 cm 3 of space, calculate the density. 2. Osmium is a very dense metal. What is its density in g/cm 3 if 50.00 g of the metal occupies a volume of 2.22cm 3? 3. What is the density (g/cm 3 ) of 48 g of a metal if the metal raises the level of water in a graduated cylinder from 25 ml to 33 ml? 14 P a g e
Unit 2.1: Atomic Structure Further Reference: 4.2 Structure of Atoms THE ATOM 1. The atom is a. It is the basic building block b. The atom is made of the following 3 parts: i.,, 2. The atom is composed of 2 parts: the and the a. The nucleus is charged i. Contains and ii. Protons are charged iii. Neutrons are charged 1. Neutrons act like for the nucleus b. The electrons are charged i. Electrons occupy the around the nucleus ii. Electrons are arranged into or iii. Electrons are moving in around the nucleus. Their movement is iv. The electron cloud give us location Location Charge Mass Special Fact Protons Neutrons Electrons 15 P a g e
PROPERTIES OF ATOMS 1. Atomic number is f. Each element has its g. In a NEUTRAL ATOM, this is also 2. (Average) Atomic Mass is 3. Mass number is the a. It is the sum of the and in the nucleus b. Mass number = + 4. Isotope Notation: PRACTICE WITH ELEMENT PARTS Element Symbol Atomic # Protons Neutrons Mass # Boron 11 B Carbon 12 6 6 Magnesium 23 12 23 Copper 64 29 35 20 16 P a g e
Unit 2.2: Isotopes and Ions Further Reference: 4.2 Structure of Atoms ISOTOPES 1. Isotopes are a. Two isotopes of an element will have the same but different (and ) b. Looking at the carbon atoms to the right: i. What is the mass number of the carbon atom on the left ii. What is the mass number of the carbon atom on the right iii. What is the atomic number of the carbon atom on the left iv. What is the atomic number of the carbon atom on the right 2. Isotope notation you write the with the on the top left and the on the bottom left a. Write an example of carbon-14 14 15 16 7 N 7 N 7 N Protons Neutrons Electrons IONS 1. Ions are atoms or groups of atoms with a or a charge a. Ions differ in the number of i. For neutral atoms are where the number of electrons are to the number of protons ii. For ions, the stay the same and the are different. You can either or electrons. b. Examples of Neutral Atoms:,,, c. Examples of Ions:,,, 17 P a g e
2. Taking away an electron gives an atom a charge because there are now more a. This is called a b. So if the Mg atom loses 2 electrons, it becomes 3. Gaining an electron gives an atom a charge because there are now more a. This is called a b. So if the F atom gains 1 electron, it becomes 39 19 N + 16 8 N -2 41 20 N +2 Protons Neutrons Electrons 18 P a g e
Unit 2.3: Electron Arrangement Further Reference: 4.3 Modern Atomic Theory ENERGY LEVELS 1. Electrons that are closer to the nucleus have energy a. Further away from the nucleus means you have energy 2. Each level (or shell) has a maximum number of that it can hold. a. 1 st level = b. 2 nd level = c. 3 rd level = d. 4 th level = 3. Electrons must occupy the first BOHR DIAGRAMS 1. Bohr diagrams show the of the atom c. They show that an atom has orbiting around it. 2. These electrons are organized into different or d. = 2 electrons e. = 8 electrons f. = 18 electrons 3. Draw the following Bohr Diagrams: H B F Si 19 P a g e
4. Valence electrons are electrons a. Valence electrons determine the b. Each column has a i. Sodium (Na) has valence electrons ii. Boron (B) has valence electrons iii. Chlorine (Cl) has valence electrons iv. Neon (Ne) has valence electrons LEWIS DOT DIAGRAMS 1. Lewis dot diagrams use the symbol and dots to represent a. How to i. Write the of the element ii. Figure out how many it has iii. Each side of the symbol can only hold 1. 1 dot = 2. Each side must get before any side can get iv. Maximum number is dots 2. Draw the following Lewis Dot: H Al Cl Ne 20 P a g e
Unit 3.1: Periodic Table of Elements Further Reference: 5.1, 5.2, and 5.3 Exploring, Organizing, and Families of the PT THREE MAIN CATEGORIES 1. The three main categories of the periodic table are c. d. e. 2. Properties of METALS a. Metals are found on the side of the periodic table i. Except for b. Metals are: i. Good ii. iii. (can be stretched into thin wires) iv. (can be pounded into thin sheets) c. A chemical property of metal is its reaction with which results in 3. Properties of NON-METALS a. Non-Metals are found on the side of the periodic table i. Except for b. Non-Metals are: i. Poor ii. Not iii. Solid nonmetals are and iv. Many non-metals are 4. Properties of METALLOIDS a. Metalloids are located b. Have properties of both and c. Metalloids are: i. Solids can be ii. They are iii. They conduct better than, but not as well as ORGANIZING THE PERIODIC TABLE 1. PERIODS a. Each is called a b. The elements in a period in properties c. Each element in the same period has the same d. The first elements in a period (the far left side of the PT) is always an. The last element in a period (the far right side of the PT) is always an. e. As you travel right across a period, you increase the in the nucleus by 21 P a g e
2. FAMILIES a. Columns of elements are called or b. Elements in each family have c. All elements in a family have the same number of d. As you moved down a family, each new elements has an extra 3. HYDROGEN a. The hydrogen square sits atop, but it is of that family i. Hydrogen is in a class of its own. b. It is a at room temperature c. It has in its one and only energy level. d. Hydrogen only needs to fill up its valence shell 4. SPECIFIC FAMILIES a. Group 1: Alkali Metals have valence electrons i. Hydrogen is not a member; it is a ii. Often react with Halogens because they have valence electrons iii. Very, especially with b. Group 2: Alkaline Earth Metals have valence electrons i. Often reactive with the family c. Group 3-12: Transition Metals have valence electrons i. Valence electrons (and oxidation number) d. Group 13: Boron Family have valence electrons i. Most are ( Boron is a ) e. Group 14: Carbon Family have valence electrons i. Contains,, and f. Group 15: Nitrogen Family have valence electrons i. Contains,, and g. Group 16: Oxygen Family have valence electrons i. Contains,, and ii. Reactive with h. Group 17: Halogen Family have valence electrons i. All are ii. Very reactive: both with elements from i. Group 18: Nobel Gas Family have valence electrons i. Exist as : All of them are ii. with other elements because their is full. 1. in the outer shell means they are full 2. Helium(He) has only in the outer shell to be full. 22 P a g e
Unit 3.2: Oxidation Numbers and Bonding HAPPY ELEMENTS 1. All elements want to be happy Further Reference: 6.2 Ionic and Covalent Bonding 2. An atom wants to make them happy a. Atoms will in order to become stable b. The most stable configuration involves having valence electrons c. 8 valence electrons = d. do not need to transfer/share any electrons because they already have and are ii. OCTET RULE means that atoms will with other atoms in order to have. 1. Atoms can or electrons with other elements 2. Elements will not just electrons. They will give to or take from. OXIDATION NUMBERS 1. The oxidation number indicated how many are going to be or during bonding a. Ranges from to 2. Steps to predicting oxidation numbers: a. First, determine how many the neutral atom has b. Determine if the atom will i. Will it be faster to or c. Count the number of electrons i. If you lose electrons, the charge will be ii. If you gain electrons, the charge will be 3. Practice! a. Lithium = b. Sulfur = c. Aluminum = d. Iodine = e. Phosphorous = f. Carbon = g. Neon = 4. Transition metals have oxidation number 23 P a g e
Unit 3.3: Bonding: Ionic and Covalent Bonds Further Reference: 6.2 Ionic and Covalent Bonding CHEMICAL STABILITY 1. Nobel gases are the elements a. They have valence electrons and don t want to or any electrons CHEMICAL BONDS 1. Involve only. The nucleus. 2. Elements will not just. a. They will OR b. There will always be at least involved in this process c. Binary compound = compound with in it i. Example:,, 3. When atoms bond, they will always form new with a. The final product has than either of the IONIC BONDS 1. Form when one atom and another atom a. One atom their to another atom 2. Occur between and a. Two charged 3. The product of an ionic bond is a a. The oxidation numbers must add up to 4. Properties of Ionic Bonds a. bonds b. melting points c. electricity when d. at room temperature 5. Drawing: a. 1 st Determine the b. 2 nd Draw the for each atom c. 3 rd Draw the being transferred in the d. DOUBLE CHECK: Does each atom have a orbital? Drawing Practice: Draw the ionic bonding structure for Na and Cl Oxidation number Lewis Dot Electrons being Transferred 24 P a g e
COVALENT BONDS 1. Occur between a. Formed when two atoms with one another. 2. Can be between two, or two atoms of a. Covalent Bonds are also called (aka Molecule) 3. Properties of Covalent Bonds a. bonds b. melting points and boiling points c. electricity when d. at room temperature 4. Drawing: a. 1 st Draw the for each atom b. 2 nd Draw the being c. 3 rd Draw each as a between two atoms d. DOUBLE CHECK: Does each atom have a orbital? Drawing Practice: Draw the covalent bonding structure for H and Cl. Lewis Dot Electrons being Shared Bonds as Lines Drawing Practice: Draw the covalent bonding structure for H 2 O Lewis Dot Electrons being Shared Bonds as Lines Drawing Practice: Draw the covalent bonding structure for CH 4 Lewis Dot Electrons being Shared Bonds as Lines 5. DIATOMIC MOLECULES a. Two atoms covalently bonded together. i. Cannot exist as and must bond together ii. Called b. The 7 diatomic molecules are: i. 25 P a g e
Unit 4.1: Balancing Chemical Reactions Further Reference: 7.1 and 7.2 Chemical Equations CHEMICAL CHANGES 1. In a chemical change, you are going to bonds, those atoms, and. 2. All chemical changes are a result of a. Happen when you bonds. b. Involve of atoms c. One set of compounds forms another set of compounds LAW OF CONSERVATION OF MATTER 1. The law of conservation of matter states that matter cannot be or, but it can only. a. The number of each type of atom must be to the number of each type of atom BEFORE WE BALANCE 1. Complete the following figure: a. Coefficient: b. Subscript: PreBalancing Practice: How many of each do you have? 2 H 2 O 3 H = O = 4 Fe 2 O 3 Fe = O = 6 NaCl Na = Cl = NO 2 N = O = BALANCING EQUATIONS 1. on the left, on the right 2. Symbols: a. + means b. means c. g means d. s means e. l means f. aq means 26 P a g e
3. When balancing chemical equations, you are not allowed to change the a. You CAN T 4. You can only change the on each side of the equation a. You CAN 5. Practice: Use the T Chart below to balance the following equation a. Magnesium (solid) + Oxygen (gas) Magnesium Oxide (solid) Balancing Practice: Using the provided T Charts, balance the following equations. 27 P a g e
Unit 4.2: Chemical Reactions: Energy Further Reference: 7.1 and 7.2 and 7.4 Chemical Equations and Reaction Rates ENERGY IN CHEMICAL REACTIONS 1. All chemical reactions involve 2. Every time a bond is or, energy is used a. Breaking bonds energy i. Chemical reactions require energy b. Forming bonds energy 3. Chemical energy is stored inside a. The stronger the bond is, the it is to start the chemical reaction 4. Energy is a. The energy within the and the must be the same as the energy within the HEAT ENERGY IN CHEMICAL REACTIONS 1. Exothermic reactions energy and the temperature a. They heat! b. Examples: i. ii. iii. 2. Endothermic reactions energy and the temperature a. They heat! b. Examples: i. ii. iii. 28 P a g e
PHOTOSYNTHESIS 1. Photosynthesis is a reaction a. Reactants are and b. Products are and 2. Energy from the is being transformed into, which is being stored as Show the formula for photosynthesis (without the coefficients!) + + SPEEDING UP REACTIONS 1. The following actions the rate of reactions because they! a. Increasing b. Increasing c. Increasing d. Increasing e. AND. CATALYST 2. A CATALYST is a substance that a. It does this by lowering the of a chem rxn. b. A catalyst is never and never c. Think of it as a, like a i. Each catalyst has only 3. Enzymes are merely that work a. Just like catalysts, each enzyme has b. Substrate: the an enzyme c. Essentially, the enzyme and substrate are like a 29 P a g e
Unit 4.3: Types of Chemical Reactions Classifying Reactions 1. Synthesis (Addition) Reactions: a. Describe it in your own words: Future Reference: 7.3 Nature of Chemical Reactions b. Write the example using A, B, C, D, X, etc c. Write a real world example found in the notes: 2. Decomposition Reactions: a. Describe it in your own words: b. Write the example using A, B, C, D, X, etc c. Write a real world example found in your in the notes: 3. Single Displacement (Replacement) Reactions: a. Describe it in your own words: b. Write the example using A, B, C, D, X, etc c. Write a real world example found in the notes: 30 P a g e
4. Double Displacement (Replacement) Reactions: a. Describe it in your own words: b. Write the example using A, B, C, D, X, etc c. Write a real world example found in the notes: 5. Acid Base Reactions: a. Describe it in your own words: b. Write the example using A, B, C, D, X, etc c. Write a real world example found in the notes: Q1 What 2 things does an Acid Base Reaction ALWAYS result in? 6. Combustion Reactions: a. Describe it in your own words: b. Write a real world example: c. What are the two products of combustion EVERY TIME? Q2 What is ALWAYS going to be the non chemical product of a combustion reaction? 31 P a g e
Unit 5.1: Solutions and Saturation Level Further Reference: 8.1 Solutions and 8.2 How Substances Dissolve HOMOGENEOUS MIXTURES 1. Solution is a a. Solutions are mixtures 2. 2 parts that make up a solution: a. Solute is i. Examples: b. Solvent is i. Examples: THE DISSOLVING PROCESS Q1 Restate the 3 parts of the kinetic theory that you previously learned: 1) 2) 3) 1. Explain how a sugar molecule is broken down when it is put into water. a. Dissolving works from the 2. Increasing between and will increase the speed molecules dissolve. 3. What are the 3 ways that we can increase the speed that a solute will dissolve into solution? 1) 2) 3) 4. Concentration is the quantity of a quantity of a. Dilute: b. Concentrated 32 P a g e
SATURATED SOLUTIONS 1. Saturated Solution is 2. Unsaturated Solution is 3. Supersaturated Solution is a. Having too much solute means that some will 5. Each substance has a value a. That value tells us how much of a substance will under a certain temperature. b. Raising the temperature the solubility value c. The solute stops dissolving once the solution reaches Fill in the table: Substance (Formula) Solubility in 100ml of Water at 20 o C Solubility in 100ml of Water at 30 o C Table Salt (NaCl) Sugar (C 6 H 12 O 6 ) Baking Soda (NaHCO 3 ) 33 P a g e
Unit 5.2: Acids and Bases Further Reference: 9.1 Chemical Reactions and 9.2 Acids and Bases CLASSIFICATION 1. Nothing itself can be an acid or base until it in water 2. Acids: a. + (ex: ) i. Produce in solution 3. Bases: a. + (ex: ) ACIDS Side Note (H + ) Hydrogen ion (H 3 O + ) Hydronium ion i. Produce in solution 1. Acids form when in solution a. Acids conduct b. Acids corrosive c. Acids taste d. Acids react with 2. List 4 examples of Acids: BASES Hydroxide ion (OH - ) 1. Bases form when in solution a. Bases feel b. Bases conduct c. Bases taste d. 2. List 4 examples of Bases: 34 P a g e
ph OF SOLUTIONS 1. ph indicates the concentration of in solution a. The more in a solution, the more the solution is, the of the solution b. The fewer in a solution, the more the solution is, the of the solution 2. Scale of ph values range from to : a. Neutral ph value Example of Neutral ph b. Acid ph value range Examples of Acid c. Base ph value range Examples of Base 3. The you get from 7, the the acid or base is. a. HCl (ph 1) is much an acid than a banana (ph 5) INDICATORS 1. Litmus paper is an a. An indicator b. When litmus paper turns red, that indicates c. When litmus paper turns blue, that indicates d. When litmus paper stays yellow, that indicates ACID AND BASE REACTIONS 2. If equal and equal are mixed, the acid and basic properties a. The remaining ions form and b. Write me a real life acid base reaction (in the notes) 3. If a strong acid is mixed with a weak base, the resulting solution is a 4. If a strong base is mixed with a weak acid, the resulting solution is a 35 P a g e