Chemistry Fundamentals Examination Bank Revision 01 (PDF)

Chemistry Fundamentals Examination Bank Revision 01 (7/2/24) It is best practice to provide approximately two exam items per enabling objective (EO) for assessments. It is up to the instructor to create the test for the final exam. Do not use any of the questions in...

Chemistry Fundamentals Examination Bank Revision 01 (7/2/24) It is best practice to provide approximately two exam items per enabling objective (EO) for assessments. It is up to the instructor to create the test for the final exam. Do not use any of the questions in this bank for the informal assessments throughout the course, these are specifically to be used to create the final exam for the course. A minimum of 50 questions is expected for a final exam. Chapter 1 Terminal Objective (TO) TLO-0100 Without references, DESCRIBE the characteristics of matter, by achieving 80% or better on a written examination. Enabling Objectives (EO) EO-0101 DEFINE the Chemistry term “matter.” 1. What is matter? o A. Anything that does not have mass but occupies space o B. Anything that has mass and does not occupy space o C. Anything that has mass and occupies space o D. None of the above 2. What does “occupies space” mean in the context of matter? o A. Matter can be seen o B. Matter can be felt o C. Matter has volume o D. Matter has color 3. What does “has mass” mean in the context of matter? o A. The color of the substance o B. The texture of the substance o C. The amount of space a substance takes up o D. The amount of material in a substance EO-0102 IDENTIFY the properties of the three (3) common phases of matter. 4. What are the characteristics of matter in the solid phase? o A. No definite shape and no definite volume o B. Definite shape but no definite volume o C. Definite shape and definite volume 1 | Page  o D. No definite shape but definite volume 5. How are the particles in a solid arranged? o A. Not closely packed and not in fixed positions o B. Closely packed but not in fixed positions o C. Closely packed and in fixed positions o D. Not closely packed but in fixed positions 6. What is a characteristic of liquids? o A. Definite shape and definite volume o B. No definite shape but definite volume o C. Not closely packed o D. No definite shape and no definite volume 7. How are the particles in a liquid arranged? o A. Definite shape and definite volume o B. Closely packed and in fixed positions o C. Closely packed but not in fixed positions o D. Not closely packed and not in fixed positions 8. What are the characteristics of gases? o A. Definite shape and definite volume o B. No definite shape but definite volume o C. Definite shape but no definite volume o D. No definite shape and no definite volume EO-0103 DEFINE the following Chemistry terms: a. Melting b. Freezing c. Boiling d. Evaporation e. Condensation f. Sublimation 9. What happens during the process of melting? o A. A liquid changes into a solid o B. A gas changes into a liquid o C. A solid changes into a liquid o D. A liquid changes into a gas 10. What is a melting point? o A. The temperature at which a liquid changes into a gas o B. The temperature at which a gas changes into a liquid o C. The temperature at which a solid changes into a liquid o D. The temperature at which a liquid changes into a solid 11. What happens during the process of freezing? o A. A solid changes into a liquid o B. A gas changes into a liquid 2 | Page  o C. A liquid changes into a gas o D. A liquid changes into a solid 12. What is a freezing point? o A. The temperature at which a liquid changes into a gas o B. The temperature at which a liquid changes into a solid o C. The temperature at which a solid changes into a liquid o D. The temperature at which a gas changes into a liquid 13. What happens during the process of boiling? o A. A solid changes into a liquid o B. A liquid changes into a solid o C. A liquid changes into a gas (vapor) o D. A gas changes into a liquid 14. What is a boiling point? o A. The temperature at which a liquid changes into a solid o B. The temperature at which a solid changes into a liquid o C. The temperature at which a liquid changes into a gas (vapor) o D. The temperature at which a gas changes into a liquid 15. What is it called when a substance changes from a liquid to a gas (vapor) state below the boiling point? o A. Boiling o B. Condensation o C. Evaporation o D. Freezing 16. What is condensation in the context of phase changes? o A. The change from solid to liquid o B. The change from liquid to gas o C. The change from solid to gas o D. The change from gas to liquid 17. What is the process called when a substance changes from the solid phase directly to the gas phase? o A. Condensation o B. Evaporation o C. Sublimation o D. Melting 18. Which of the following is an example of a substance that undergoes sublimation? o A. Water o B. Dry ice (frozen carbon dioxide) o C. Iron o D. Gold EO-0104 DISCRIMINATE between physical and chemical change (i.e., DESCRIBE the changes and GIVE AN EXAMPLE of each). 19. What is a physical change? 3 | Page  o A. A change that forms a new substance o B. A change that alters a substance’s chemical properties o C. A change that alters any of a substance’s physical properties o D. A change that alters a substance’s state of matter 20. Which of the following is an example of a physical change? o A. Burning wood o B. Cutting a piece of wood o C. Rusting iron o D. Baking a cake 21. What is a chemical change? o A. A change that alters a substance’s state, i.e. solid to liquid. o B. A change that alters any of a substance’s physical properties o C. A change that forms a new substance o D. A change that alters a substance’s shape 22. Which of the following is an example of a chemical change? o A. Melting ice o B. Boiling water o C. Combining hydrogen and oxygen to form water o D. Cutting a piece of paper 23. What happens when hydrogen and oxygen combine under the right circumstances? o A. They form a colorless gas o B. They form a solid substance o C. They undergo a chemical change and form water o D. They undergo a physical change and form a new gas EO-0105 DEFINE the following Chemistry terms: a. Mixture b. Solution c. Pure Substance 24. What is a mixture? o A. A substance made of elements and compounds. o B. Two or more pure substances that are physically combined in variable proportions o C. A substance that undergoes a chemical reaction when combined with another substance o D. A change that forms a new substance 25. What is a solution in the context of mixtures? o A. A mixture of two solids o B. A mixture of a liquid and a gas o C. A homogeneous mixture where the molecules of the substances blend evenly but are not bound together by intermolecular bonds o D. A mixture where a chemical reaction occurs between the substances 4 | Page 26. What is a pure substance? o A. A substance that can be separated into different substances by physical means o B. A substance that changes its composition depending on its source o C. A homogeneous sample of matter that has the same composition and properties, whatever its source o D. A substance that forms new substances when combined with other substances EO-0106 DEFINE the following Chemistry terms: a. Solute b. Solvent c. Solubility 27. Which of the following is considered the solute in a solution of sugar and water? o A. Water o B. Sugar o C. Both are solutes o D. Neither are solutes 28. In the atmosphere, which gas is considered the solute? o A. Oxygen o B. Nitrogen o C. Both are solutes o D. Neither are solutes 29. Which of the following substances is insoluble in water? o A. Salt o B. Sugar o C. Silicon Dioxide (Sand) o D. All of the above EO-0107 DEFINE and GIVE EXAMPLES of the following: a. Atom b. Element c. Molecule d. Compound 30. *What is the smallest unit of bonded atoms that can exist independently? o A. Element o B. Compound o C. Atom o D. Molecule 31. *What are the two types of molecules? o A. Molecules of a compound and molecules of a mixture o B. Molecules of an atom and molecules of a compound 5 | Page  o C. Molecules of an element and molecules of a compound o D. Molecules of a substance and molecules of a mixture 32. What is a compound? o A. The smallest unit of bonded atoms that can exist independently o B. A pure substance composed of two or more different elements chemically combined in fixed proportions o C. A pure substance composed of the same element chemically combined in fixed proportions o D. Anything that occupies space 6 | Page  Chapter 2 Terminal Objective (TO) TLO-0200 Without references (except where noted), EXPLAIN the characteristics of atoms and molecules, by achieving 80% or better on a written examination. Enabling Objectives (EO) EO-0201 DESCRIBE the model of an atom. 33. What are the two regions of an atom? o A. Molecules and compounds o B. Groups and Periods o C. Nucleus and electron cloud o D. Protons and Neutrons 34. Where are the protons and neutrons located in an atom? o A. In the electron cloud o B. In the nucleus o C. Outside the atom o D. In the atomic shell 35. What determines the element of an atom? o A. The number of electrons o B. The number of neutrons o C. The number of protons o D. The total number of particles EO-0202 STATE one (1) sub-atomic particle that differs among the following: a. Elements b. Isotopes c. Ions 36. What gives atoms their identity? o A. Neutrons o B. Electrons o C. Protons o D. Ions 7 | Page  37. What is an atom with 1 proton in its nucleus? o A. Helium o B. Oxygen o C. Hydrogen o D. Carbon 38. What are atoms of the same element with different numbers of neutrons called? o A. Ions o B. Isotopes o C. Molecules o D. Compounds 39. *What is an atom or molecule called when the total number of electrons is not equal to the total number of protons? o A. Isotope o B. Compound o C. Molecule o D. Ion EO-0203 DEFINE the Chemistry term “atomic number”. 40. What is the atomic number of an element determined by? o A. Number of molecules o B. Number of neutrons o C. Number of protons o D. Number of isotopes 41. What is the atomic number of uranium? o A. 1 o B. 2 o C. 238 o D. 92 EO-0204 DETERMINE the atomic mass number for any given element. 42. What does the atomic mass number of an atom represent? o A. The sum of protons and electrons o B. The sum of neutrons and electrons o C. The sum of protons and neutrons o D. The sum of isotopes 43. What is the atomic mass number of a normal hydrogen atom? o A. 0 o B. 1 o C. 2 o D. 3 8 | Page  EO-0205 DEFINE the Chemistry term “valence.” 44. The innermost shell of any atom will hold a maximum of how many electrons? o A. 0 o B. 5 o C. 2 o D. 8 45. *What is another meaning of the word ‘valence’ in chemistry? o A. Atomic number o B. Atomic mass o C. Ionic charge o D. Isotope number EO-0206 IDENTIFY chemically active electrons and DESCRIBE the reason for their activity. 46. Which electrons are chemically active? o A. Electrons in the innermost shell o B. Electrons in the middle shell o C. Electrons in the outermost shell o D. Electrons in the nucleus 47. *What is the result of the reactions undergone by elements that have an excess or deficiency of electrons in the outer shell? o A. The reacting elements strive to empty their outer shell of electrons o B. The reacting elements strive to achieve an outer shell that is half full of electrons o C. The reacting elements strive to achieve an outer shell that is full of electrons o D. The elements want to gain another neutron EO-0207 DEFINE the Chemistry terms “ion” and “ionization” and GIVE EXAMPLES of ions. 48. What is the process called when electrons are gained or lost by an atom or a group of atoms? o A. Electrification o B. Ionization o C. Polarization o D. Magnetization 49. What happens when a neutral atom gains electrons? o A. It has a net positive charge 9 | Page  o B. It remains neutral o C. It has a net negative charge o D. It becomes a compound EO-0208 DESCRIBE how positive and negative ions are formed. 50. What type of ions are formed when atoms lose electrons? o A. Neutral ions o B. Positive ions o C. Negative ions o D. Isotopes 51. What type of ions are formed when atoms gain electrons? o A. Neutral ions o B. Positive ions o C. Negative ions o D. Isotopes EO-0209 Using a Periodic Table of the Elements, IDENTIFY the following: a. Periods of the periodic table b. Groups of the periodic table 52. How are the elements in the periodic table organized? o A. Alphabetically o B. Based on their atomic number o C. Based on their ionization o D. Based on their physical state at room temperature 53. What is each column in the periodic table called? o A. A period o B. A group o C. A family o D. A class 54. How many columns are there in the periodic table? o A. 8 o B. 12 o C. 18 o D. 20 EO-0210 Using the Periodic Table of Elements, DETERMINE the following for any element: a. Chemical symbol or name b. Atomic Number 10 | Page  c. Classification Use the periodic table for the following questions: 55. *Boron would be considered a _______________. a. None of these choices b. Non-metal c. Metal d. Metalloid 56. Select the phrase that correctly completes the following statement: Metals ________________________. a. Include chlorine, fluorine, and bromine b. Include iron, copper, silver, and gold c. Are chemically unreactive d. Are located in the upper right area of the periodic table 11 | Page 57. Lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, and neon form a ______________. a. Atom b. Compound c. Period d. Group 58. Match each group on the periodic table to its name _e___Group 1 a. Noble Gases _c___ Group 2 b. Transition Metals _b___ Groups 3-12 c. Alkaline Earth Metals _d___ Group 17 d. Halogens _a___ Group 18 e. Alkali Metals EO-0211 STATE why elements in the same group on the periodic table share certain chemical and physical characteristics. 59. Why do elements in the same group (family) of the Periodic Table have similar chemical and physical characteristics? o A. Because they have the same atomic number o B. Because they have the same atomic weight o C. Because their valence shells have the same electron configuration o D. Because they are in the same period 60. *How does the atomic number influence the chemical properties of elements within the same group in the Periodic Table? o A. Elements with higher atomic numbers have more protons o B. Elements with higher atomic numbers have more neutrons o C. Elements with higher atomic numbers have more energy levels, placing their valence electrons further from the nucleus, which influences their reactivity o D. Elements with higher atomic numbers have fewer energy levels EO-0212 Using a Periodic Table of the Elements, DETERMINE relative chemical reactivity of elements. 61. Why are Group VIII elements (the Inert or Noble Gases) unreactive? o A. Because they have the highest atomic numbers o B. Because they are gases o C. Because their valence (outermost) shell is full o D. Because they are located on the right side of the periodic table 12 | Page 62. How does the reactivity of Group I & II elements change as one progresses down the column? o A. Reactivity decreases o B. Reactivity remains the same o C. Reactivity increases o D. There is no specific pattern EO-0213 EXPLAIN the chemical notation 63. What does the “A” represent for the following notation ? a. The atomic number b. The number of protons c. The number of neutrons d. The atomic mass EO-0214 Given the standard or the X-A notation for a particular item, DETERMINE the atomic structure, i.e.: a. Number of protons b. Number of neutrons c. Number of electrons 64. *When using notation to determine the atomic structure, what information about the atom can be obtained? o A. The electronic structure o B. The ionic charge or valence o C. The number of protons, electrons, and neutrons o D. The atomic weight 65. What is the ionic charge (valence) of an atom that has one more electron than it has protons? o A. +1 o B. +2 o C. 0 o D. -1 66. What is the ionic charge (valence) of an atom that has the same number of electrons and protons? o A. +1 o B. -1 o C. 0 13 | Page o D. +2 14 | Page  EO-0215 Using a Periodic Table of the Elements, IDENTIFY the “atomic weight” and DETERMINE its value for any given element. 67. Select the atomic weight of nitrogen. a. 14.007 g/mol b. 16.00 g/mol c. -3 g/mol d. 7.01 g/mol EO-0216 DEFINE the Chemistry term “molecular weight” and CALCULATE the molecular weight for any given molecule or compound. 68. *What does the term “molecular weight” refer to? o A. The weight of the heaviest atom in the molecule o B. The average weight of all the atoms in the molecule o C. The total mass of the individual atoms in the molecule o D. The weight of the lightest atom in the molecule 69. *How is the molecular weight of a molecule determined? o A. By adding the atomic weights of the heaviest and lightest atoms in the molecule o B. By finding the average atomic weight of all the atoms in the molecule o C. By adding the atomic weights of all the atoms in the molecule o D. By multiplying the atomic weights of all the atoms in the molecule EO-0217 DEFINE the Chemistry term “mole” and RECALL the value of Avogadro’s number. 70. What is the counting term used in chemistry? o A. Dozen o B. Mole o C. Pair o D. Score 71. What does a mole represent in chemistry? o A. 12 items o B. 6.022 x 1023 items o C. 20 items o D. The atomic weight EO-0218 DEFINE the Chemistry term “gram atomic weight” and DETERMINE its value for any given element. 15 | Page 72. *What is the gram atomic weight (gaw) of an element? o A. The number of protons in an atom of the element o B. The number of neutrons in an atom of the element o C. The mass in grams of a mole of atoms of the element o D. The number of electrons in an atom of the element 73. *How many atoms does a gram atomic weight of any element contain? o A. 6022 atoms o B. 6.022 x 1023 atoms o C. 6.022 x 10-24 atoms o D. 6.022 x 10 atoms 16 | Page  Chapter 3/4 Terminal Objectives (TO) TLO-0300 Without references, DESCRIBE how atoms chemically bond together to form different molecules and compounds, by achieving 80% or better on a written examination. TLO-0400 Without references, EXPLAIN how chemical solutions and their concentration are affected by various mechanisms, by achieving 80% or better on a written examination. Enabling Objectives (EO) EO-0301 DESCRIBE the basic mechanism for ionic bonds. 74. How are ionic bonds formed? o A. By sharing electrons between atoms o B. By one atom losing electrons and another atom gaining electrons o C. By atoms exchanging protons o D. By atoms sharing protons 75. What force holds ions together in an ionic bond? o A. Gravitational force o B. Magnetic force o C. Electrostatic attraction between oppositely charged particles o D. Nuclear force EO-0302 DESCRIBE the basic mechanism for covalent bonds. 76. What is the method by which atoms bond when they share electrons to fill their outer shells? o A. Ionic bonding o B. Covalent bonding o C. Metallic bonding o D. Hydrogen bonding 77. What force holds atoms together in covalent bonds? o A. The attraction between protons and electrons o B. The repulsion between electrons o C. The attraction between neutrons and protons o D. The overlapping (intertwined) electron clouds of the atoms 17 | Page  EO-0303 DESCRIBE the basic mechanism for metallic bonds. 78. What is the third type of bonding, in addition to ionic and covalent? o A. Hydrogen bonding o B. Metallic bonding o C. Van der Waals bonding o D. Dipole-dipole bonding 79. What is the mechanism of metallic bonding? o A. Each atom contributes its core electrons into a region surrounding the atoms o B. Electrons are localized and belong to one atom o C. Electrons form a “sea” in which only core electrons are shared by many atoms o D. Each atom contributes its valence electrons into a region surrounding the atoms, these electrons are delocalized and do not belong to any one atom, but are free to move around, forming a “sea” in which all valence electrons are shared by many atoms. EO-0304 EXPLAIN the significance of a balanced chemical equation. 80. What does a balanced chemical equation show? o A. It shows the ratio of volumes of gases involved in a chemical reaction o B. It indicates the physical states of reactants and products o C. The amounts of reactants and products involved, and the mole ratio of reactants and products o D. It provides the actual mass of reactants and products EO-0305 DESCRIBE the change in energy that takes place in the following chemical reactions/processes: a. Endothermic reaction/process b. Exothermic reaction/process 81. What is an exothermic reaction? o A. A reaction in which energy is absorbed o B. The minimum amount of energy required to start a chemical reaction o C. A reaction in which energy is given off or released o D. A reaction in which no energy change occurs 82. Which of the following is an example of an endothermic process? o A. Burning a candle o B. A chemical reaction where the heat content of the products is less than the heat content of the reactants o C. Melting ice cubes o D. A reaction where energy is released 18 | Page  EO-0306 DEFINE the following Chemistry terms: a. activation energy b. catalyst 83. What is activation energy in the context of a chemical reaction? o A. The energy released during a chemical reaction o B. The total energy of the products of a chemical reaction o C. The minimum amount of energy required to start a chemical reaction o D. The energy difference between the reactants and products 84. What does the reaction rate describe in a chemical reaction? o A. The amount of energy required to start a reaction o B. The reaction in which energy is given off or released o C. How rapidly a chemical reaction progresses, and whether the reaction is speeding up or slowing down as it progresses o D. The energy difference between the reactants and products EO-0307 DESCRIBE how the following factors can affect the reaction rate: a. The nature of the reactants b. The surface area of the reactants c. The concentration of the reactants d. The temperature of the environment e. The presence of a catalyst 85. What are the factors affecting the rate of chemical reactions? o A. The nature of the products o B. The volume of the reactants o C. The nature of the reactants, surface area, concentration, temperature, and presence of a catalyst o D. The mass of the reactants 86. What is the concentration in the context of a chemical reaction? o A. The number of reactants in a given volume of material o B. The number of atoms, molecules, or ions contained in a given volume of material o C. The number of products in a given volume of material o D. The total mass of reactants in a given volume of material 87. Where do chemical reactions take place when solids react with other substances? o A. Inside the solid o B. In the air surrounding the solid o C. On the surface of the solid o D. In the core of the solid 88. What is the role of a catalyst in a chemical reaction? o A. A catalyst is a substance that gets permanently consumed during the reaction 19 | Page  o B. A catalyst is a substance that changes the nature of the reactants o C. A catalyst is a substance that changes the rate of a chemical reaction but doesn’t get permanently consumed during the reaction o D. A catalyst is a substance that changes the volume of the reactants EO-0308 DEFINE the Chemistry term “Chemical Equilibrium.” 89. What is chemical equilibrium? o A. The state in which the rate of the forward reaction is greater than the reverse reaction o B. The state in which the rate of the reverse reaction is greater than the forward reaction o C. The state in which the rate of the forward and reverse reactions are exactly equal o D. The state in which the amount of product is limited to a certain quantity 90. What does it mean when a reaction reaches equilibrium? o A. It means that the amount of product is limited to that quantity o B. It means that the reaction has stopped o C. It means that the reaction can no longer be shifted to favor either the forward or the reverse reaction o D. It means that the rate of the forward and reverse reactions are exactly equal, but it does not mean that the amount of product is limited to that quantity 91. What is a reversible reaction? o A. It means the products can react to re-form the reactants o B. It means reactants are not reversible o C. It means changing the state of the reaction from equilibrium to non-equilibrium o D. It means stopping the reaction EO-0401 EXPLAIN how the following affect the solubility of solids, liquids, and gases. a. Temperature change b. Pressure change 92. What does it mean if a compound is soluble? o A. It means a solution has the maximum amount of a dissolved substance at a given temperature o B. It means that the compound is able to break apart into fragments too small to be caught by any filter o C. It means that a substance can rapidly have a chemical reaction o D. It means that heat is in a solution 20 | Page  EO-0402 DEFINE the following Chemistry terms: a. Saturated solution b. Super saturated solution 93. What is a saturated solution? o A. A solution that contains the minimum amount of dissolved solute o B. A solution that contains the maximum amount of dissolved solute o C. A solution that contains more dissolved solute than a saturated solution under the same conditions o D. A solution that contains less dissolved solute than a saturated solution under the same conditions 94. What is a super saturated solution? o A. A solution that contains the minimum amount of dissolved solute o B. A solution that contains the maximum amount of dissolved solute o C. A solution that contains more dissolved solute than a saturated solution under the same conditions o D. A solution that contains less dissolved solute than a saturated solution under the same conditions EO-0403 DEFINE the following Chemistry terms: a. Chemical concentration b. Concentrated solution c. Dilute solution 95. What is the chemical concentration of a solution? o A. The measurement of the amount of solute present in a given amount of solvent or solution o B. The amount of solute in a solution o C. The amount of solvent in a solution o D. The measurement of the amount of solvent present in a given amount of solute 96. Which of the following best describes a dilute solution? o A. A solution with a relatively large amount of solute as compared to the amount of solvent o B. A solution with a relatively small amount of solute as compared to the amount of solvent o C. A solution with an equal amount of solute and solvent o D. A solution with no solute EO-0404 DESCRIBE the following solution processes: 21 | Page  a. Concentration Process b. Dilution Process 97. What is the concentration process? o A. The process by which the concentration of a solution is decreased o B. The process by which the amount of solvent in a solution is increased o C. The process by which the concentration of a solution is increased o D. The process by which the amount of solute in a solution is decreased 98. What best describes the dilution process? o A. The process by which the concentration of a solution is increased o B. The process by which the amount of solvent in a solution is decreased o C. The process by which the concentration of a solution is decreased o D. The process by which the amount of solute in a solution is increased 22 | Page  Chapter 5 Terminal Objective (TO) TLO-0500 Without references, DESCRIBE the components that make up acids and bases, and the units used to measure these components, by achieving 80% or better on a written examination. Enabling Objectives (EO) EO-0501 DEFINE the following Chemistry terms: a. Acid b. Base c. Salt 99. What are acids? o A. Substances that produce hydroxide ions (OH-) when dissolved in water o B. Ionic compounds composed of both positive and negative ions o C. Substances that produce hydrogen ions (H+) when dissolved in water o D. Substances that do not dissolve in water 100. What are salts? o A. Ionic compounds composed of both positive and negative ions o B. Substances that produce hydroxide ions (OH-) when dissolved in water o C. Substances that produce hydrogen ions (H+) when dissolved in water o D. Substances that do not dissolve in water EO-0502 DESCRIBE what happens when acids and bases are mixed in a solution, and IDENTIFY the resulting products. 101. What happens when acids and bases are mixed in a solution? o A. They tend to increase each other’s concentration o B. They tend to decrease each other’s concentration o C. They tend to neutralize each other, and the resulting products are salts and water o D. They tend to form more acids and bases 102. What is neutralization in the context of acids and bases? o A. The reaction of hydrogen ions (H+) and hydroxide ions (OH-) to form more acids and bases 23 | Page  o B. The reaction of hydrogen ions (H+) and hydroxide ions (OH-) to form only water (H2O) o C. The reaction of hydrogen ions (H+) and hydroxide ions (OH-) to form only a salt o D. The reaction of hydrogen ions (H+) (also known as hydronium ions (H30+), and hydroxide ions (OH-) to form a salt and water (H2O) EO-0503 DEFINE and STATE the formula for pH. 103. What is the definition of pH? o A. The positive logarithm of the hydrogen ion concentration of a solution o B. The negative logarithm of the hydrogen ion concentration of a solution o C. The negative logarithm of the hydroxide ion concentration of a solution o D. The positive logarithm of the hydroxide ion concentration of a solution 104. What value on the pH scale is considered neutral? o A. 0 o B. 7 o C. 14 o D. 10 105. How can you determine if a solution is acidic, basic, or neutral using pH? o A. If the pH of a solution is > 7 the solution is basic; if it is 7 the solution is neutral; if it is 7 the solution is acidic; if it is 7 the solution is basic; if it is