CHM1045 Spring 2014 EXAM 2 Dr Bridget A DePrince Chapter 4 1 Define solute a solvent and solution Solute is the substance present in a smaller amount Solvent substance present in a larger amount Solution homogeneous mixture of two or more substances 2 Using Table 4 2 classify common compounds as strong electrolytes weak electrolytes or non electrolytes Soluble or insoluble salts strong or weak acids strong or weak bases 3 Explain why water is often called a universal solvent utilizing the term polar solvent dissociation ionization and hydration Water is a very effective solvent for ionic compounds Although water is an electrically neutral molecules it has a positive region The H atom and a negative region the O atom or POSTIVE AND NEGATIVE POLES This is the reason it is a polar solvent Ionization is used to describe the separations of acids and basis into ions Hydration is the process in witch an ion is surrounded by water molecules in a specific order Hydration helps to stabilize ions in solutions and prevents cations from combing with anions 4 Describe precipitation reactions using the terms solubility and precipitate Precipitation reaction results in the formation of an insoluble product OR PRECIPITATE A precipitate is an insoluble solid that separates from a solution LIKE IN LAB EX Pb NO3 2 aq 2KI aq PI2 s 2KNO3 aq 5 Using tables 4 2 classify common ionic compounds as soluble or insoluble 1 CHM1045 Spring 2014 EXAM 2 Dr Bridget A DePrince 6 Predict the resulting products and write the molecular equation ionic equation and net ionic equation identify spectator ions given the reactants of chemical equations 7 Explain differences between Arrhenius acids and bases and Bronsted acids and bases Arrhenius ACID substance that when added to water increases the concentration of H1 ions present BASE substance that when added to water increases the concentration of OH1 ions present HCl is an example of an Arrhenius acid and NaOH is an example of an Arrehnius Base Bronsted ACID Proton donor BASE proton acceptor 2 CHM1045 Spring 2014 EXAM 2 Dr Bridget A DePrince 8 Predict the product formed by an acid base neutralization reaction Neutralizing reaction is a reaction between an acid and a base Generally aqueous acid base reactions produce water and a salt which is an ionic compound made up of a cation other than H and an anion other than OH or O2 Acid base salt water 9 Describe what factor results in an oxidation reduction reaction Also known as REDOX Electron transfer reactions All occur in aqueous solutions 10 Identify redox reactions and are able to identify what is being oxidized and reduced as well as identify the oxidizing agent and reducing agent Define redox Electron transfer reaction OXIDIZED Accepts Electrons REDUCED donates electrons to oxygen 11 Assign oxidation numbers to elements in a compounds and ions 12 Calculate the molarity of a solution given the mass number of moles of solute and the volume of solution 3 CHM1045 Spring 2014 EXAM 2 Dr Bridget A DePrince 13 Describe the method for preparing a specific molar solution given the volume of a solution required and the solute to be used Table 4 7 Know equation moles of solute molarity x L soln 14 Describe how to prepare a specific dilute solution given a known stock solution using dilution techniques Analyze problem Stabilize data Perform calculations Table 4 9 15 Predict the mass of a precipitate formed using gravimetric analysis methods Gravimetric analysis is an analytical technique based o the measurement of mass The mass of the sample is usually measure extremely accurately due to the technique However is only applicable to reactions that go to completion or have nearly 100 yields 16 Deduce the mass percent of specific ions present in an original solution given the result of a gravimetric anabasis 17 Describe how acid base titrations work to identify the concentration of an unknown acid or base In titration a solution of accurately known concentration called a standard solution is added gradually to another solution of unknown concentration until the chemical reaction between the two solutions is complete If we known the volumes of the standard and unknown solutions used in the titration along with the concentration of the standard solution we can calculate the concentration of the unknown solution 18 Predict the amount mass moles or volume of solution of an acid base required to neutralize a base acid Equivalent point the point at which the acid has completely reacted with or been neutralized by the base Usually indicated by a sharp changed in color 4 CHM1045 Spring 2014 EXAM 2 Dr Bridget A DePrince 19 Predict the volume of an oxidizing reducing agent solution required to oxidize reduce a specific volume of reducing oxidizing agent solution provided that the net ionic equation is given Chapter 5 1 List physical characteristics of gases Gases assume the volume and shape of their containers Fases are the most compressible of the states of matter Gases will mix evenly and completely when confined to the same container Gases have much lower densities than liquid and solids 2 Define the term terms velocity acceleration force newton energy joule kinetic energy pressure and pascal Velocity the speed of something in a given direction Acceleration increase in the rate or speed of something Force strength of energy as an attribute of physical action Newton SI unit of force N Joule SI unit of work or energy Kinetic Energy energy that a body possesses by virture of being in motion Pressure forced applie per unit area pressure force area Pascal one newton per square meter 1Pa 1 N m 2 3 Convert between torr mmHg atomosphere and pascals 5 CHM1045 Spring 2014 EXAM 2 Dr Bridget A DePrince 1 torr 1 mmHg 1 atm 760 mmHg 1 atm 101 325 Pa 4 State the difference between open tube manometers and closed tube manometers and explain how each is used A manometer is a device used to measure the pressure of gases other than the atmosphere Closed tube manometers is normally used to measure pressures below atmospheric pressure Open tube manometers is better suited for measuring pressure equal to or greater than atmospheric pressure 5 Ideal gas law PV nRT 6 Explain the differences between Kelvin and Celsius C plus 273 x Kelvin 20 Celsius 273 293 Kelvin 7 Describe gas constant R 8 Define standard temperature and pressure STP and demonstrate that at STP one mole of gas occupies 22 4 liters 9 Perform calculation involving density the Ideal gas equation and
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