Chemistry Semester 2 Final Exam Study Guide – Flashcards
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Mole
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The amount of a substance whose mass is equal to the atomic mass in grams
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Avogadro's number.
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6.022 * 10^23
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Calculate molar mass.
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Skill Question
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Calculate how many moles of a sample you have from its mass and molar mass.
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Skill Question Equation: #mol= mass/ m.m.
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Solve a gram to gram problem.
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Equation: #mol= mass/ m.m. ratio mole bridge g-m-m-g
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Limiting reactant.
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The reactant in a chemical reaction that limits the amount of product that can be formed
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Excess reactant
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The reactant in a chemical reaction that is in excess.
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Identify limiting and excess reactants in a reaction
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Skill Question
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pressure
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Force per unit of area on a surface
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STP
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Standard Temperature and Pressure (0 celsius and 1 atm)
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State molar volume at STP
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22.414 Liters
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Solve problems using the ideal gas equation.
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Skill Question PV = nRT R = 0.082 Latm/molK P - Pressure, measured in atm. V - volume, measured in L. n - number of moles, measured in mol. R - ideal gas constant, measured in 0.082Latm/molK T- temperature, measured in K
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Solution.
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A homogeneous mixtures of 2 or more substances in the same phase
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Colloid.
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Medium sized particles - shows the Tyndall effect - particles do not settle
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Suspension.
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Larger particles - does show the Tyndall effect - particles do settle out eventually
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Explain Tyndall effect.
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Particles that are dissolved do not scatter light. Particles that are suspended do.
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Explain the difference between homogeneous and heterogeneous.
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The difference between heterogeneous and homogeneous mixtures is the degree at which the materials are mixed together.
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Solute.
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The substance dissolved in the solution
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Solvent.
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The dissolving medium
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Discuss why water is referred to as "the universal solvent."
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Water can break down polar and covalent bonds
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Describe the process of dissociation.
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Define diluted and concentrated solutions.
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Diluted means less solute, concentrated is more solute
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Calculate molarity and molality.
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Molarity: The number of moles of solute in one liter of solution Molality: the number of moles of solute in one kg of solvent
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Explain some of the quantitative concentration (like ppm and ppb)
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Define saturated and supersaturated.
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A solution that contains the maximum amount of solute. A solution that contains more dissolved solute than a saturated solution contains under the same conditions
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Write simple dissociation equations.
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Skill Question
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Use the solubility guidelines to predict whether a compound is soluble.
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Skill Question
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Define precipitate.
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Solid separates from a liquid
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Write net ionic equations.
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Skill Question
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Define spectator ion.
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The Ion that doesn't bond in a reaction
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Define electrolyte.
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An Ionic Bond that is separated into charged particles when dissolved. The ions will carry charge, conducting electricity
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Define colligative property.
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Properties that depend on the concentration of solute particles but not their identity
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List some colligative properties
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Freezing point, boiling point
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Calculate boiling point elevation
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Skill Question
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Calculate freezing point depression
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Skill Question
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Define volatile.
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Evaporates easily and has a low boiling point
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Define nonvolatile.
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Does not evaporate easily or have a low boiling point
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Define colligative.
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Describe how a nonvolatile solute interferes with the boiling of a solvent.
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Non-volatile solute particles are like prison guards. It takes a lot to get past them. A Non-volatile solute has a higher boiling point than the solute you put it in
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Discuss some of the relevant details about acid rain.
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Acid Rain is harmful to the world and our resources.
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Define indicator.
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A substance that changes color in the presence of an acid or base
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Describe properties of acids.
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Taste sour, Strong acids can be corrosive to flesh, Change the color of indicators, Produce hydrogen gas when they react with active metals, Neutralizes bases, Conduct electricity
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Describe properties of bases.
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Taste bitter, Strong bases can burn flesh, Change the color of indicators, Feel slippery, Neutralizes acids, Conduct electricity
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Name binary Acids and oxyacids.
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Skill Question
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Describe the Arrhenius concept of acids and bases.
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A chemical compounds that increases the concentration of hydrogen ions in an aqueous solution
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Describe the Bronsted Lowry concept of acids and bases.
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A molecule or ion that is a proton donor
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Describe what makes an acid or base strong.
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The amount of hydronium or hydroxide in the acid or base respectively.
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Describe the process by which hydronium is formed.
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Formed during the creation of all acids ever. Opposite of hydroxide which is found in bases.
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Describe neutralization reactions
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The two compounds create a salt
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Predict the products of neutralization reactions.
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Skill Questions
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Calculate [H3O+] and [OH-].
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Skill Question
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Calculate pH.
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Skill Question
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Oxidation.
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Decrease in oxidation number
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Define reduction.
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Increase in oxidation number
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Identify the oxidized ion and the reduced ion in a reaction.
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Skill Question
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Recognize examples of electrochemical applications (like the ones on the test you just took).
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Skill Question
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What is the freezing point of phenol if it has 30g of MgCl2 dissolved in 2kg of phenol? ∆Tf = imkf
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i = 3 m = #mol solute / kg solvent #mol = mass / m.m. = 30g / 95.205 = .315mol m = .315mol / 2kg = .158m kf = -7.40 c/m plug everything into equation ∆Tf = 3(.158)(-7.40) ∆Tf = -3.5 question asks for the actual freezing point, so add -3.5 to the original temperature, 40.9 40.9 + (-3.5) = 37.4c
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What is the hydronium concentration and hydroxide concentration of 1.3 x 10-3M H2SO4, and what is the pH?
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[H3O+] = 2 x 1.3 x 10-3M = 2.6 x 10-3M 2.6 x 10-3M = [H3O+] Hydronium Concentration 1 x 10-14M2= [H3O+][OH-] 1 x 10-14M2 = [2.6 x 10-3M][OH-] / 2.6 x 10-3M 3.85 x 10-12M = [OH-] Hydroxide Concentration pH = -log[H3O+] = -log[2.6 x 10-3M] = 2.59 pH
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Process in which hydronium dissociates
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When it dissociates there are lots of hydrogen protons in the solution and since hydrogen is just a proton, which are positively charged, then that proton is attracted to anything negative: it gets attracted to the negative pole of water making it H3O+
