CHEMISTRY CP Name: _______KEY_____________________ Period: ________

CHEMISTRY SPRING FINAL REVIEW SHEET

REMEMBER: In addition to a Periodic Table, Ion Chart, and Scientific Calculator, you may have one 4 x 6” card (BOTH SIDES) with any notes, formulas, or constants you may need. UNIT 5 – STOICHIOMETRY DEFINITIONS AND PRACTICE PROBLEMS: Mole Concept 1. Know the definition of a mole. Avogadro’s number of particles; 1Mole = 6.02 × 1023 particles = gram formula mass of an element/compound 2. Know Avogadro’s Number. 6.02 × 1023 3. Be able to calculate the molar mass for a compound. As an example: Calculate the molar masses of MgCO3

and HNO3. MgCO3 = 84.3 g/M HNO3 = 63.01 g/M 4. Make the following conversions:

a. What is the number of moles of CaS in 120 grams of the compound? Ca: 40.1 g 120 g / 72.2 g = 1.66 moles S: + 32.1 g CaS = 72.2 g/M

b. What is the mass in grams of 18.06×1023 molecules of CO2?

18.06×1023mol 1 Mole 44.0g/M = 132g

6.02×1023 mol 1 Mole C: 12.0 g × 1 = 12.0 g O: 16.0 g × 2 = 32.0 g CO2 = 44.0 g/M

c. How many molecules of CO2 are in .50 moles?

0.5 M CO2 6.02×1023 mol = 3.01×1023 molecules

1 M Stoichiometry 5. Given the equation: ____ Zn + _2___ HCl ____ ZnCl2 + ____ H2

a. How many moles of hydrogen will be formed when 4 moles of HCl are reacted? Mole Ratio: H2 = 1 = x Moles H2 x = 2 Moles H2

HCl 2 4 Moles HCl b. How many moles of Zn will be reacted to form 3 moles of ZnCl2?

Mole Ratio: Zn = 1 = x Moles Zn x = 3 Moles Zn ZnCl2 1 3 Moles ZnCl2

c. How many moles of HCl will be needed to react completely with 3 moles of Zn? Mole Ratio: Zn = 1 = 3 Moles Zn x = 6 Moles HCl

HCl 2 x Moles HCl 6. Given the equation: __2_ Na + __2__ H2O _2___ NaOH + ____ H2

According to the following reaction, calculate the number of grams of sodium hydroxide that will be produced if 8.215 grams of sodium are reacted with excess water.

Step 1: Convert grams to Moles 8.215 g Na × 1 Mole Na = 0.357 Moles Na

23.0 g Na Step 2: Mole Ratio Na = 2 = 0.357 Moles Na = x = 0.357 Moles NaOH NaOH 2 x Moles NaOH Step 3: Convert Moles to grams 0.357 Moles NaOH × 40 g NaOH = x = 14.28 grams NaOH 1 Mole

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7. Given the equation: __2__ CO + ____ O2 __2___ CO2 How many grams of carbon monoxide are required to produce a total of 44 grams of oxygen?

Step 1: Convert grams to Moles 44 g O2 × 1 Mole O2 = 1.375 Moles O2

32.0 g O2

Step 2: Mole Ratio O2 = 1 = 1.375 Moles = x = 2.75 Moles CO CO 2 x Moles Step 3: Convert Moles to grams 2.75 Moles CO × 28.0 g CO = x = 77 grams CO 1 Mole

Limiting Reactant 8. Given the equation: ____ C6H12O6 + _ 6 ___ O2 _ 6 ___ CO2 + __ 6 __ H2O

If 35 grams of C6H12O6 react with 40 grams of O2, how many grams of CO2 will be produced? What is the limiting reactant?

Step 1: Balance the equation Step 2: Convert grams of reactants into Moles and compare 35 g C6H12O6 × 1 Mole C6H12O6 = 0.194 Moles C6H12O6 **Limiting Reactant** 180 g C6H12O6

40 g O2 × 1 Mole O2 = 1.25 Moles O2

32 g O2

Step 3: Use Limiting Reactant to solve for Moles of CO2 C6H12O6 = 1 = 0.194 Moles = x = 1.164 Moles CO2 CO2 6 x Moles Step 4: Convert Moles to grams 1.164 Moles CO2 × 44 g CO2 = x = 51.2 grams CO2

9. Given the equation: ____Mg(s) + _2___ HCl(aq) ____ MgCl2(aq) + ____ H2(g)

A 1.4 g sample of magnesium is treated with 8.1 g of hydrochloric acid to produce magnesium chloride and hydrogen gas.

a. What is the limiting reactant? Step 1: Balance the equation Step 2: Convert grams of reactants into Moles and compare

1.4 g Mg × 1 Mole Mg = 0.0576 Moles Mg **Limiting Reactant** 24.3 g Mg

8.1 g HCl × 1 Mole HCl = 0.235 Moles O2

34.5 g HCl b. What is the excess reactant? HCl c. How many grams of hydrogen are produced?

Step 3: Use Limiting Reactant to solve for grams of H2 Mg = 1 = 0.0576 Moles = 0.0576 Moles H2 x 2 g/M = 0.1152 g

H2 1 x Moles Percent Yield 10. Given the equation: ____ Mg + _2___ HNO3 ____ Mg(NO3)2 + ____ H2

a. If 40 grams of magnesium (Mg) are reacted with excess nitric acid (HNO3), how many grams of hydrogen are produced.

Step 1: Convert grams to Moles 40 g Mg × 1 Mole Mg = 1.646 Moles Mg

24.3 g Mg

Step 2: Mole Ratio Mg = 1 = 1.646 Moles = x = 1.646 Moles H2

H2 1 x Moles Step 3: Convert Moles to grams 1.646 Moles H2 × 2.02 g H2 = x = 3.29 grams H2 1 Mole

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b. If 1.7 grams of hydrogen was actually produced, what was the percent yield? (Hint: Use your answer from part a)

(Actual yield / Theoretical Yield) x 100 = (1.7 g / 3.29 g) x 100 = 51.7%

11. The amount of product in a given reaction turns out to be only 2.34 grams although the theoretical amount was calculated to be 3.12 grams. What is the percentage yield?

(Actual yield / Theoretical Yield) x 100 = (2.34 g / 3.12 g) x 100 = 75%

12. Given the balanced equation: NaHCO3 + HCl NaCl + H2O + CO2 In the reaction of 10 grams of NaHCO3 with excess HCl, 4.5 grams of NaCl is actually produced. What is the percentage yield from this reaction?

Step 1: Convert grams to Moles 10 g NaHCO3 × 1 Mole = 0.119 moles NaHCO3

84.01 g

Step 2: Mole Ratio NaHCO3 = 1 = 0.119 Moles = x = 0.119 Moles HCl HCl 1 x Moles Step 3: Convert Moles to grams 0.119 Moles H2 × 58.5 g NaCl = x = 6.96 grams NaCl 1 Moles

(Actual yield / Theoretical Yield) x 100 = (4.5 g / 6.96 g) x 100 = 64.5%

Empirical and Molecular Formula 13. What is the empirical formula for fructose, C6H12O6? CH2O 14. Determine the empirical formula for succinic acid that is composed of 40.60% carbon, 5.18% hydrogen, and

54.22% oxygen. C: 40.60 g = 3.38 moles H: 5.18 g = 5.18 moles O: 54.22 g = 3.38 moles 12.0 g 1.00 g 16.00 g 3.38 / 3.38 = 1 5.18/3.38 = 1.5 3.38/3.38 = 1 EF = C2H3O2 15. A sample of a compound is composed of 12.8 grams of copper and 3.5 grams of chlorine. What is the

empirical formula of the compound? Cu: 12.8 g = 0.202 moles Cl: 3.5 g = 0.10 moles 63.5 g 35.5 g 0.202 / 0.099 = 2 0.099 / 0.099 = 1 EF = Cu2Cl

16. The empirical formula of a compound is CH2O and the molar mass is 150 g/mol. What is the molecular formula of the compound?

MM CH2O: 12 + 2 +16 = 30 g 150 g / 30 g = 3 MF = C3H6O3 UNIT 6 – States of Matter, Kinetic Molecular Theory, Gas Laws DEFINITIONS AND PRACTICE PROBLEMS: 17. Know the three common states of matter in terms of particle motion. Gas: particles move randomly and independent of one another; indefinite shape and volume Liquid: particles vibrate around a moving point; indefinite shape and definite volume Solid: particles vibrate about a fixed point; definite shape and volume 18. Be able to draw a picture of what the particles look like in each of the three states of matter.

19. What is plasma? Give two examples of where plasma is found. State of matter consisting of free electrons and positive ions- no atoms in plasma state; most common form of matter Examples of where plasma can be found: lightning, neon signs, aurora borealis, sun and stars

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20. What are the three assumptions of the Kinetic Theory? (1) all matter consists of small particles (2) these particles are in constant motion (3) collisions between particles are perfectly elastic 21. What does STP stand for and what are its numerical values (i.e., give five for pressure and two for

temperature)? STP: Standard Temperature and Pressure

Pressure units are 101.3 KPa, 760 mmHg, 760 torr, 1 atm, and 14.7 psi Temperature units are 0°C and 273 K 22. At what temperature does all molecular motion stop? What is the name for this temperature? 23. Convert the following temperatures from Celsius to Kelvin and Kelvin to Celsius:

a. 22°C 295 K c. 220 K -53°C b. 474°C 747 K d. 390 K 117°C

24. Convert the following pressure units to the indicated pressure units: a. 2.6 atm = _1976___ mmHg b. 120 mmHg = __15.99___ KPa

Gas Law Constants R = 0.0821 R = 8.315 R= 62.4 25. There is a mixture of three gases in a closed container. Gas A exerts a pressure of 15 psi, Gas B a pressure of 6.5 psi, and the total pressure is 25.7 psi. What is the partial pressure of Gas C? Ptotal = PA + PB + PC 25.7 psi = 15 psi + 6.5 psi + PC 25.7 psi = 21.5 + PC

PC = 4.2 psi 26. Which of the following gases would diffuse most rapidly: N2, O2, He, Cl2? 27. What is the ratio of the rate of diffusion of H2 to He?

𝑹𝒂𝒕𝒆  𝑨𝑹𝒂𝒕𝒆  𝑩

= 𝑴𝒐𝒍𝒂𝒓  𝑴𝒂𝒔𝒔  𝑩𝑴𝒐𝒍𝒂𝒓  𝑴𝒂𝒔𝒔  𝑨

     𝑹𝒂𝒕𝒆𝑯𝒚𝒅𝒓𝒐𝒈𝒆𝒏      𝑹𝒂𝒕𝒆𝑯𝒆𝒍𝒊𝒖𝒎

 =   𝟒.𝟎𝟎  𝒈𝟐.𝟎𝟎  𝒈

= 1.41

28. A sample of gas occupies 200 cm3 at STP. Calculate the volume this same amount of gas would occupy at pressure of .75 atm and a temperature of 10°C.

P1 × V1 = P2 × V2 T1 T2

(1atm)(200 cm3) = (.75 atm)(V2) 273 K 283 K V2 = 276 cm3 29. Know that at STP, one mole of any gas is equal to 22.4 L. 1 mole = 22.4 Liters at STP for any gas a. Determine the volume, in liters, occupied by 0.030 moles of CO2 gas at STP.

0.030 moles x 22.4 Liters = 0.672 liters b. How many moles of argon atoms are present in 44.8 L of argon gas at STP? 44.8 Liters / 22.4 Liters = 2 moles 30. Given the reaction at STP: ____ N2 + __3__ H2 ___2__ NH3 How many liters of H2 will be required to react with 56 grams of N2?

Step 1: Convert grams to Moles 56 g N2 × 1 Mole = 2 moles N2

28.0 g Step 2: Mole Ratio

N2 = 1 = 2 Moles = x = 0.6 Moles Hydrogen

H2 3 x Moles Step 3: Convert Moles to liters 2 Moles H2 × 22.4 L = x = 44.8 liters 1 Mole

31. Given the reaction at STP: __2__ H2 + ____ O2 __2__ H2O What is the total volume water vapor produced if 40 liters of hydrogen gas are consumed in the reaction

above? Step 1: Liter Ratio H2 = 2 moles = 40 liters of water vapor

H2O 2 moles

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32. According to Boyle’s Law, what type of relationship do pressure and volume have? INVERSE or INDIRECT 33. A gas sample occupies 450 cm3 at STP. Calculate the volume this gas would occupy at a pressure of 45

KPa and a temperature of 30° C. P1 × V1 = P2 × V2

T1 T2

(101.3)( 450) = (45)(V2) 273 K 303 K V2 = 1127.1 cm3

34. What pressure in atm is required to compress 1.0 L of gas at 760 mm Hg to a volume of 50.0 L? P1 × V1 = P2 × V2

(760 mmHg) (1.0 L) = x (50.0 L) P = 15.2 mmHg or 0.02 atm 35. A 200 mL sample of air at STP is heated at constant volume until its pressure increases to 1500 mm Hg. What is the new temperature of the sample? P1 = P2

T1 T2

(760mmHf) = (1500mmHg) 273 K x K T2 = 539 K

36. What is the molecular mass of a gas if .150 L have a mass of 4.22 g at 100° C and 1.05 atm? MM = (.422 g) (0.0821) (373 K’) (1.05 atm) (.150 L) MM = 81.90 g

37. What is the density of a gas at STP that has a molar mass of 44.0 g/mol? d = MM·P/RT d = (44g/M)(1atm) / (0.0821)(273K) d = 1.96 g/L 38. A large balloon sits at the surface of the sea. After being lowered under the surface the balloon has its temperature tripled and its pressure halved. What will happen to its volume? P1 × V1 = P2 × V2

T1 T2

(1atm)( 1L) = (0.5 atm)(V2) 1 K 3 K V2 = 6 Volume increases by a factor of 6

USE THE GRAPH BELOW TO ANSWER QUESTIONS 39-40.

UNIT 7 – Reaction Rates, Equilibrium, and ThermochemistryDEFINITIONS AND PRACTICE PROBLEMS: Rates of Reaction 41. Know what the rate of a chemical reaction can be measured by. Decrease in concentration of reactants or increase in concentration of products over time. 42. Know what factors affect the rate of a reaction and how they affect the rates of reaction. For example,

what would happen to the rate of reaction if the following actions were performed? FACTORS THAT AFFECT RATE OF RxN: Temperature, Concentration, Surface Area and Catalyst a. Removing an enzyme Decreases rate of reaction b. Decreasing temperature Decreases rate of reaction c. Increasing surface area Increases rate of reaction d. Diluting a solution Decreases rate of reaction e. Adding heat Increases rate of reaction

39. What gas law is described by the graph? Charles’ Law: graph shows Temperature and Volume 40. According to the graph, what type of relationship do the variables volume and temperature have? Direct relationship, as temperature increases, volume increase

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f. Adding an enzyme Increases rate of reaction g. Breaking a reactant into smaller pieces Increases rate of reaction 43. Know what conditions are true of a chemical reaction at equilibrium. (1) rates of forward and reverse reactions are equal. (2) The concentrations of all substances involved stop

changing (3) reactants and products are both present but concentrations are not necessarily equal (4) The system is a dynamic one, still an ongoing inter-conversion of reactants and products.

Le Chatelier’s 44. What does Le Chatelier's Principle say? Le Châtelier's principle states that if a system in equilibrium is subjected to a stress by changes in determining factors, such as temperature, pressure, and concentration of components, the system will tend to shift its equilibrium position so as to counteract the effect of the stress 45. What are three kinds of stresses that can be placed on a system? temperature, pressure, and concentration of components 46. Use the following reaction at equilibrium answer the questions:

A(g) + 3 B(g) 2 C(g) + heat a. What direction will the reaction shift if heat is added? left b. What direction will the reaction shift if pressure is increased? right c. What will happen to the concentration of A if the temperature decreases? decreases d. What will happen to the concentration of C if more A is added? increases e. What direction will the reaction shift if more C is added? left

47. Use the following reaction at equilibrium answer the questions: A(g) + B(aq) ⇄ C(s) + heat �Hrxn= -453 kJ/mol a. The pressure of A in the reaction chamber is increased. The reaction will shift right to favor products b. The temperature of the reaction is increased by 200 C. Shift left c. A catalyst is added to the system. No change

48. At 1000oC, container has an equilibrium mixture consisting of 0.102 mol/L of ammonia, 1.03 mol/L of nitrogen, and 1.62 mol/L of hydrogen. Calculate the Keq for the equilibrium system.

2 2 3N (g) + 3H (g) 2NH (g)Ä Keq = (0.102)2 / (1.03)2 (1.62)3 = 0.00231 49. The equilibrium constant for the equilibrium reaction CO(g) + H2O(g) ⇌CO2(g) + H2(g) is 302 at 600K. What is the

value of the equilibrium constant for the reverse reaction at the same temperature? Keq‘= 1/302 = 0.00331 POTENTIAL ENERGY DIAGRAMS

PHASE DIAGRAMS

Use the potential energy diagram to the left to answer the following questions? 50. Which curve (A or B) represents the catalyzed reaction? B – lowers activation energy 51. According to the diagram above, is the forward chemical reaction endothermic or exothermic?

Use the potential energy diagram to the right to answer the following questions. 52. Is the forward reaction endothermic or exothermic? 53. Which letter represents the activation energy? A 54. Which letter represents the potential energy of the products? F 55. Which letter represents the heat of reaction? C 56. Which letter represents the activation energy of the reverse reaction? E

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USE THE DIAGRAM TO THE LEFT FOR QUESTIONS 57-60. 57. According to the diagram, at which point are the solid, liquid and gas phases in equilibrium (exist at the same temperature and pressure)? POINT D 58. What is this point called? TRIPLE POINT 59. Which temperature and pressure correspond to the critical point? CRITICAL POINT IS POINT E (304.25 K, 73 atm) 60. At a constant pressure of 60 atm, which phase change occurs from 250 K to 200 K? FREEZING (LIQUID TO SOLID)

HEATING/COOLING CURVES 61. Use the diagram below: ENERGY CALCULATIONS

                               𝐄𝐪𝐮𝐚𝐭𝐢𝐨𝐧  𝟏:𝐂𝐚𝐥𝐜𝐮𝐥𝐚𝐭𝐢𝐧𝐠  𝐇𝐞𝐚𝐭 𝐄𝐪𝐮𝐚𝐭𝐢𝐨𝐧  𝟐:𝐂𝐚𝐥𝐜𝐮𝐥𝐚𝐭𝐢𝐧𝐠 ΔHfus 𝐄𝐪𝐮𝐚𝐭𝐢𝐨𝐧  𝟑:𝐂𝐚𝐥𝐜𝐮𝐥𝐚𝐭𝐢𝐧𝐠 ΔHvap 𝑄 = 𝑚𝑎𝑠𝑠  ×  ∆𝑇  ×𝐶𝑝                                                                                𝑄 = ΔHfus  ×  𝑚𝑎𝑠𝑠                                                                                            𝑄 = ΔHvap  ×𝑚𝑎𝑠𝑠                                              

Constants: Heat of fusion = 334 J/g Heat of vaporization = 2260 J/g Specific heat for solid water (ice) = 2.06 J/g°C Specific heat for liquid water = 4.18 J/g°C

Specific heat for gaseous water (steam) = 2.02 J/g°C Boiling point of water = 100°C Freezing point of water = 0°C

62. How many joules of heat energy are absorbed when 200.0 grams of water are heated from 10.0°C to

40.0°C? Q = m x T x Cp Q = 200 x 30°x 4.18 = 25080 J 63. What is the total amount of heat energy released when 125 grams of water is cooled from 50.0°C to 25°C? Q = m x T x Cp Q = 125 x (-25°) x 4.18 = -13062.5 J 64. How much energy is needed to heat 87g of ice at -10°C to water vapor at 120°C? Step 1: Q = m x T x Cp(solid) (87g) x (10) x (2.06) = 1792.2 J Q total = 267351 J Step 2: Q = m x Hfus (87g) x (334 J/g) = 29058 J Step 3: Q = m x T x Cp(liquid) (87g) x (100) x (4.18) = 36366 J Step 4: Q = m x Hvap (87g) x (2260 J/g) = 196620 J Step 3: Q = m x T x Cp(gas) (87g) x (20) x (2.02) = 3514.8J

A

B

C

D

E Label the solid, liquid and gas phases on the diagram to the left. (A) Which of the letters on the diagram correspond to the liquid phase only? B (B) Which of the following letter(s) correspond to when a phase change is occurring? D and C (C) Could this substance be water based on the melting point/boiling point of water? Yes, it could be water

LIQUID

SOLID

GAS

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65. The boiling point of ethanol is 78°C. How much heat is required to heat 100 grams of ethanol from 25°C to its boiling point and then to turn it into a vapor? Cp = 2.44 J/g °C ∆Hvap = 855 J/g

Q = m x T x Cp Q = m ∆Hvap Qtotal = 98432 J Q = 100 x (53°) x 2.44 = 12932 J Q = 100 x 855 = 85500 J UNIT 8 – Solutions, Solubility, Units of Concentration, Acids & Bases 66. What gives water its unique properties such as lower density in solid state, low vapor pressure, high specific

heat, and high surface tension? Hydrogen bonding between individual water molecules 67. What causes high surface tension in water? Hydrogen bonding and surface molecules which tend to exert

an inward force resulting unbalanced forces and a smooth surface 68. Why is water considered the universal solvent? It has the ability to dissolve many other substances due to its

polarity 69. Know the definition of a solution, solute and solvent. Given an example of a solution.

SOLUTION: a homogeneous mixture where one substance is dissolved inside of another. SOLVENT: the substance that does the dissolving SOLUTE: the substance that is dissolved Examples of solutions include steel, Kool-Aid, and air. A mixture that is not a solution is oil and water.

70. Give an example of a solid, liquid, and gas solution. Identify the solute and solvent. Solid: Steel. Solute-carbon, Solvent-iron Liquid: Soda. Solute-sugar, CO2, etc. Solvent-water Gas: Air. Solute-O2, CO2, etc. Solvent-N2

71. What happens to ionic compounds such as NaCl when they dissolve in water? Complete dissociation into its ions - Na+ and Cl- forming electrolytes which can conduct electricity 72. Why does a covalent compound like sugar (C12H24O12), dissolve in water? Because sugar is polar and water

is polar; like dissolves like 73. What is the difference between unsaturated, saturated and supersaturated solutions?

SATURATED: a solution where the maximum of solute is added to solvent SUPERSATURATED: a solution where there are more solute particles than are needed to form a saturated solution

UNSATURATED: a solution where there are less solute particles than are needed to form a saturated solution 74. A glass of water has 10g of sugar dissolved in it. If more sugar can be added to dissolve in the water, is the solution unsaturated, saturated, or supersaturated? UNITS OF CONCENTRATION COMMON CONVERSIONS: 1 g = 1 mL for water 1 kg = 1000 g 1 L = 1000 mL 75. If 8.7 g of Na2CO3 is dissolved in 800 mL of water, what is the molarity of the solution? What is the answer in PPM? 8.7 g / 106 g = 0.0821 moles Molarity = 0.0821moles / 0.800 L = 0.103M 76. How many grams of beryllium chloride, BeCl2, are needed to make 125 mL of a 0.050 M solution? Molarity = moles / Liters 0.00625 moles x 79.9 g/M = 0.499 grams 0.050 M = x moles / 0.125 L x moles = 0.00625 moles 77. How many grams of MgCl2 would be needed to make 1.5 L of a 0.40 M solution? Molarity = moles / Liters 0.5 moles x 95.3g/M = 47.65 grams 0.40 M = x moles / 1.5 L x moles = 0.625 moles 78. Suppose you had 7.00 moles of solute dissolved into 5.80 L of solvent. What's the molality? (1 L = 1 kg) molality = moles / kg solven molality = 7.00 moles / 5.80 kg = 1.21m 79. If I make a solution by adding 83 grams of sodium hydroxide, NaOH, (solute) to 750 mL of water (solvent)…

a. What is the molality of sodium hydroxide in this solution? molality = 2.075 moles / .750 kg = 2.77m b. What is the percent by mass of sodium hydroxide in this solution? [83 g / (750+83)] x100 = 9.96% c. What is the mole fraction of sodium hydroxide in this solution?

XNaOH = 2.075 moles / 43.74 moles = 0.0474 XH2O = 1.00 - 0.0474 = 0.9526

80. If I make a solution by adding water to 35 mL of methanol (CH3OH) until the final volume of the solution is 275 mL, what is the percent by volume of methanol? %Volume = ( 35 mL / 275 mL ) x 100 = 12.7%

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SOLUBILITY

81. Know how temperature affects the solubility of a solid, liquid and gas. Be able to identify how a solubility of a solid, liquid and gas would plot on a curve. Increasing temperature will cause solubility for solids and liquids to increase. Increasing temperature will cause solubility for gases to decrease. Increasing pressure increases the solubility of gases

82. Using the solubility graph below, determine if the following solutions are saturated, unsaturated or supersaturated. If they are anything but saturated, list two things you can do to make them saturated (include numbers).

ACIDS AND BASES 83. What are the properties of acids and

bases? Acids: taste sour, pH < 7, turns blue

litmus red. Bases: taste bitter, slippery, pH > 7, turns red litmus blue.

84. What is an Arrhenius acid and base? How is it different from a Bronsted Lowry acid and base? The two theories are just different ways to describe acids and bases. Bronsted-Lowry definition is generally more inclusive of all acid-bass. Arrhenius acid increases H+ concentration in solution while Arrhenius base increases OH- concentration. Bronsted Lowry acid is defined as a proton donor, while the Bronsted Lowry base is defined as a proton acceptor.

85. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction: NH3 (g) + HOH (l) ⇄ NH4+(aq) + OH-(aq) Base Acid Conj. Acid Conj. Base

86. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction: HCO3 -(aq) + HOH (l) ⇄ CO3 2-(aq) + H3O+ (aq) Acid Base Conj. Base Conj.. Acid 87. If given the hydrogen ion concentration, be able to determine the pH of an aqueous solution. As an example: What is the pH of an aqueous solution with a hydrogen ion concentration of 1×10-4? pH = 4 88. If the hydroxide ion concentration is 1×10-12, what is the pH of the solution? pOH = 12 pOH + pH = 14 12 + x = 14 pH = 2 89. If the pH is 2.37, what is the [H+]? pH = - log[H+] 10-2.37 = [4.27 x 10-2] 90. If the pH is 11.36, what is the concentration of hydroxide ions? pH + pOH = 14 10-2.64 = [2.29 x 10-2] 11.36 + x = 14 pOH = 2.64 91. Given the reaction: NH3 + H2O NH4+ + OH- Be able to identify which reactant acted as an acid and why. Remember: H+ is a proton. Ammonia (NH3) is

a weak base, so this should help you identify water (H2O) as the acid. You can also tell because according to Bronsted- Lowry definition of an acid, H2O donates a proton so it is the acid.

92. What are the products of a neutralization reaction? Predict the products of the following reactions: Remember neturalization reactions result in a SALT and WATER. The salt is an ionic compound made from the positive ion of one reactant bonded to the negative ion of the other reactant

a. HCl + Mg(OH)2 MgCl2 + H2O b. H2CO3 + KOH K2CO3 + H2O

Solution (in 100 mg water)

Saturated, Unsaturated, Supersaturated

+/- how many °C to make saturated

+/- how many grams to make saturated

10 g of KClO3 at 30°C

SATURATED N/A N/A

30 g of NaCl at 40°C

UNSATURATED Beyond this graph

~ 6 g