Post on 10-Mar-2018
Name:Topic 1: Data Collection
What is chemistry? How do we make accurate and precise observations of our world?Vocabulary
Term Definition
Organic ChemistryInorganic ChemistryAnalytical ChemistryPhysical ChemistryBiochemistry
Qualitative ObservationQuantitative ObservationPrecision
Accuracy
Dependent VariableIndependent VariableScientific MethodMajor prefixes of the Metric System (kilo-milli)SI System
Density
Intensive propertyExtensive propertyDimensional AnalysisConversion FactorSignificant FigureUncertainty
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Name:Topic 1: Data Collection (cont)
What is chemistry? How do we make accurate and precise ob3servations of our world?Objective Practice Problem
Identify the proper names and uses of common laboratory materials.
1. Label the following materials with their proper names and uses
Read laboratory measuring instruments to the nearest degree of precision and record data with correct number of significant figures.
2. Use the picture to the right to answer the following questions.
a. Each mark represents __________ mL.
b. The device shown is precise to what decimal place? ________
c. According to the measuring device, what is the volume of water?____________
Name and use basic SI units.
3. Label each of the following measurements with the proper SI unit.
Length _______________ Volume ______________ Mass ______________
4. Label the values below with the correct metric prefixes
___________1000 ___________1/1000 ___________1/100 ___________1/10
Distinguish between qualitative and quantitative observations.
5. Classify each of the following as either a qualitative or quantitative observation:
________________ The candle weighs 4.00 grams. ________________ The candle is round.
________________ The candle burned brightly. ________________ The candle is 2.00cm.
Perform mathematical operations involving dimensional
6. Convert using proper dimensional analysis: 25.4ft/day = ? cm/min
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Name:analysis.Determine the number of significant figures in measurements.
7. Underline and state the number of significant figures in each of the following values:
1.201 ___________ 12.0 x 104 ___________
0.012 ___________ 1200 ___________
8. Round each of the following numbers to 3 significant figures:
125.32 ________________ 124.500
________________
23.523 ________________ 0.0010101
________________
Perform mathematical operations involving significant figures.
9. Solve the following. Report answers with correct units and significant figures:
6.5 cm / 2.1 cm = _____________________
2.33 K + 18.1 K _______________________
0.00032 m x 12 m =_____________________
44.25 kg – 2.25 kg ________________________
Topic 1: Data Collection (cont)What is chemistry? How do we make accurate and precise ob3servations of our world?
Perform mathematical operations involving significant figures AND use basic SI units.
10. Convert the following (while maintaining the same number of significant figures):
42.1 g = ___________ kg 0.450 L = ___________ mL 2.25 L = ___________ mL
5.4 ft/day =___________ cm/min 3.2 °C = ___________ °F 126 K =___________ C
Perform mathematical operations involving scientific notation.
11. Express the following numbers in scientific notation:
52,000 = 0.000175 =
12. Perform the computations below expressing the answers in scientific notation
(7.1x 109)(55) = 10,500 ÷ (4.0 x 10 -4) =
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Name:Differentiate between a precise and an accurate set of data.
13.
Distinguish between intensive and extensive properties.
14. Label the following as intensive or extensive properties of matter:
Density _________________ Volume _________________
Mass _________________ Temperature_________________
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Name:Topic 2: Chemical and Physical Properties of Substances
What are the characteristics by which matter can be classified?Vocabulary
Term Definition
matter
chemical change
chemical property
physical change
physical property
changes of state (phase change)solid, liquid, gas, plasmapure substance
atom
element
compound
mixture
heterogeneous mixturehomogeneous mixturesolution
solute
solvent
aqueous solution
density
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Name:Topic 2: Chemical and Physical Properties of Substances
What are the characteristics by which matter can be classified?Objective Practice Problem
distinguish between chemical and physical properties; chemical and physical changes.
15. Classify each of the following as either a physical or chemical change or property
Release of Odor _________________ Reactivity _________________
Paper Burning _________________ Crushing Chalk _________________
Color Change _________________ Melting Butter _________________
Cutting Paper _________________ Stirring _________________
distinguish between and classify types of matter
16.
Topic 2: Chemical and Physical Properties of Substances (continued)distinguish between and classify types of matter
17. Complete the following table using the terms element, compound, mixture, heterogeneous, homogeneous, and pure substance.
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Name:18. A group of two or more substances that are physically combined are called a
a. mixture.b. compound.c. element.
19. Mixtures that are not evenly mixed throughout are calleda. pure substances.b. homogeneous.c. heterogeneous.
20. Classify the following substances as a: heterogeneous mixture, solution, compound, or
element.
a. iron shavings (Fe) _________________ c. brewed tea _________________
b. neon gas (Ne) _________________ d. water (H2O) _________________
e. granite _________________ f. nitrogen _________________
g. salt (NaCl) _________________ h. energy drink _________________
describe the characteristics of phase states in terms of particle arrangement and motion.
21. Which of the following has a definite shape? Circle all that applya. Solids b. Liquids c. Gases
22. Which of the following has a low density? Circle all that applya. Solids b. Liquids c. Gases
23. Label each of the following with A-I as given in the diagram to the right_____ Melting _____ Evaporation
_____ Liquid _____ Solid
_____ Gas _____
Condensation _____ Freezing
describe the relationship between energy, particle motion and change of phase.
24. Label A, B, and C with the proper phase states.25. Label 1,2,3,4 with the proper phase changes
26. At point 3 on the graph above,a. the heat added increases and the temperature increases.b. the heat added decreases and the temperature decreases.c. the heat added decreases and the temperature stays the same.
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Name:d. the heat added increases and the temperature stays the same.
Use derived properties to identify substances
Use the diagram below to answer the next three questions27. Which line in the graph above represents lead? The density of lead is 11.4 g/mL. The
density of gold is 19.3 g/mL.e. Line Af. Line Bg. Line A if the piece of lead is larger than the piece of gold.h. Line A if the piece of gold is larger than the piece of lead.
28. Which of the following has the greatest volume?
i. 80 g of substance Aj. 80 g of substance Bk. both have the same volumel. not enough information to tell
29. The independent variable in the graph ism. volume in mL.n. mass in go. line A.p. line B.
Topic 3: Atomic TheoryWhat is all matter made of?
VocabularyTerm Definition
atom
atomic mass
atomic number
isotope
mass number
neutron
proton
nucleus
atomic orbital
electron
photon
Aufbau principle
Hund’s rule
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•••••••••••
020406080
100120140160180200
0 1 2 3 4 5 6 7 8 9 10Volume (mL)
•Line A Line B
Name:Pauli exclusion principleatomic emission spectrum
electromagnetic spectrumcontinuous spectrumline spectrum
quanta
Ground state
Excited state
Topic 3: Atomic TheoryWhat is all matter made of?
Objective Practice ProblemsState the position of protons, neutrons and electrons in the atom.
State the relative masses and relative charges of protons, neutrons and electrons.
30. Draw a bohr model of an atom of Sodium-23, labeling the number of protons, neutrons, electrons and their charges.
Determine the number of protons, neutrons and electrons in atoms and ions from the mass number, atomic number and charge.
31. Complete the following table:Symbol
Atomic # Mass # # Protons # Electrons # Neutrons Ionic Charge
34 80 0
Define the term isotope.Write the symbolic notations used to represent isotopes.Calculate the atomic mass for an element given the mass of its isotopes
32. How many neutrons do each of the following isotopes contain?
(a) chlorine-32 ___ (b) gold- 169 _______ c) lead-182 _______
33. Given the following information for element "X",Isotope Mass (amu) Percent Abundance1 34.97 75.77%2 36.97 24.23%(a) Calculate the atomic mass for element “X” (b) Identify element X :
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Name:and the percent abundance for each.Describe the electromagnetic spectrum.
34. Draw two waves with the wavelengths representing the relative energies of red light and of blue light.Label one “more energetic,” the other “less energetic.”
Describe how the frequencies of light emitted by an atom are a unique characteristic of that atom.Summarize the main features of the Bohr model of the hydrogen atom.
35. Which of the following does the Quantum Mechanical model of the atom propose?a. The atom contains protons and electrons.b. Electrons orbit the nucleus of the atom.c. Electrons orbit the nucleus in specific patterns.d. Electrons emit energy in the form of light.
36. Complete the following table:Principal Energy Level
Total number of sublevels
Total number of orbitals
Total number of electrons
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37. Write labeled orbital diagrams for each of the following elements:Calcium Argon
Apply the Aufbau principle, Hund’s rule and the Pauli Exclusion Principle to write electron configurations for an atom.
Write electron configuration and ion configurations of elements
38. Write the electron configurations for the following elements using noble gas notation.Mn Zn
P Pb
39. Write the full electron configurations for the following ions:P-3 Al 3+
40. Determine which of the following electron configurations represent an atom in theexcited state and identify that element. (Circle choice and name the element)a. 1s22s32p63s23p6 b. 1s22s12p63s23p5 c. 1s23s22s22p63p6
element name_______________________________
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Name:Topic 4: Periodic Trends
What trends are used to identify the properties of elements and compounds?Vocabulary
Term Definition
Diatomic element
Periodicity
Electronegativity
Dimitri Mendeleev
Periodic Law
Group/Family
Period
Valence Shell
Valence Electron(s)
Octet Rule
The shielding effect
Atomic Radius
Ionic Radius
Ionization Energy
Topic 4: Periodic TrendsWhat trends are used to identify the properties of elements and compounds?
Objective Practice ProblemsIdentify the diatomic elements.
41. List the formulas of the diatomic elements: H2 ,
Discuss the relationship between an element's electron configurations its location on the periodic table.
An atom is found to have the electron configuration of [Kr]5s24d105p5
42. Identify this element:
43. How many valence electrons does it have?
44. What family does this element belong to?
45. What charge do all of elements in this family have and why?
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Name:
Compare the periodic trends of atomic and ionic radius, ionization energy, and electronegativity.
Explain how the shielding effect influences atomic radius, ionization energy, and electronegativity.
Classify the phase state of an element as a solid, a liquid, or a gas.
Describe the main features of our modern periodic table.
Locate and name the s, p, d and f- blocks on the periodic table.
Using the periodic table below,46. Circle the only noble gas that does not have a p orbital.47. Number the groups 1A-8A48. Number the periods 1-749. Box and Label the 2-s block, the 3p-block, 5d-block, and the 4-f-block.50. Label the halogens, transition elements, alkaline earth metals, alkali metals, and the noble
gases.51. Label groups 1A, 2A and 7A with their ionic charge52. Put an X through all seven elements that are naturally diatomic.53. Label the arrows to show the trends for electronegativity both along a period and a group54. Label the appropriate arrows to show the trends for atomic radius both along a period and a
group55. Label the appropriate arrows to show the trends for ionization energy both along a period
and a group
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Name:
Topic 5: BondingHow do elements combine to form new matter?
How does the type of bond affect the properties of the compound?
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Name:Vocabulary
Term Definition
Ion
Anion
Cation
Ionic bond
Lattice energy
Metallic bond
Oxidation numberCovalent bond
Lewis structure
Resonance structureVSEPR
Polar covalent
Non-polar covalentDispersion force
Dipole-dipole
Hydrogen bond
Pi bond
Orbital hybridizationBond length
Bond strength
Bond energy
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Name:Topic 5: Bonding
How do elements combine to form new matter?How does the type of bond affect the properties of the compound?
Objective Practice ProblemsProperly write the chemical formulas of ionic compounds when given the name
Properly write the chemical formulas of molecular compounds when given the nameProperly write the chemical formulas of acids when given the name
56. Write the correct formula for the following compounds:
sulfur trioxide____________________ calcium sulfate
____________________
phosphoric acid____________________ hydrofluoric
acid____________________
aluminum fluoride ____________________ lead(II)nitrate
____________________
aluminum hydroxide ____________________ ammonium carbonate
______________
gold(III)chloride dinitrogen pentaoxide
Properly name ionic compounds when given the chemical formula
Properly name molecular compounds when given the chemical formula
Properly name acids when given the chemical formula
57. Write one proper name for each of the following compounds.
PbCl4 _____________________________________________
NCl3 _____________________________________________
S2F10 _____________________________________________
Hg(NO3)2 _____________________________________________
HNO3 _____________________________________________
H2S _____________________________________________
Fe(OH)3 _____________________________________________
Sn3(PO4)4 _____________________________________________PREDICT the type of chemical bond formed using electronegativity differences
58. An ionic bond exists when the electronegativity difference is greater than _________
59. A covalent bond exists when the electronegativity difference is _______
60. A polar covalent bond exists when the electronegativity difference is between _______________
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Name:DESCRIBE the characteristics of ionic and covalent compounds
61. Circle the words that complete the sentence. (Molecular/Ionic) bonds are usually (strong/weak) and (do/ do not) conduct electricity, are volatile and have a low melting point.
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Name:Topic 5: Bonding(Continued)
DRAW Lewis Diagrams of Ionic and Covalent Bonds based on the Octet Rule
Draw resonance structures
DETERMINE the direction of a dipole moment in a polar molecule
PREDICT the molecular geometry of a molecule using the VSERP Model
Predict the polarity of a molecule
62. Lewis Structure
Electro-negativityDifference
Bond Polarity
Molecular Shape(VSEPR)
Shape Name Molecular Polarity
CBr4
H2O
PH3
SO3
NH4+
Brackets!
BH3
Classify the intermolecular forces that exist between atoms and molecules.
Identify the type of bonding that occurs between the atoms/molecules/ions listed below.(Select: Ionic, polar covalent, nonpolar covalent, dipole-dipole, hydrogen bonding, dispersion forces.)
63. ___________________________Between atoms of hydrogen and oxygen in a water
molecule
64. ___________________________Between molecules of water
65. ___________________________Between atoms of bromine in a bromine molecule
66. ___________________________Between molecules of bromine
67. ___________________________Between ions of sodium and chlorine in sodium chloride
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Name:68. ___________________________Between molecules of fluoromethane
Topic 6: The MoleHow do chemists quantify matter?
VocabularyTerm Definition
Empirical Formula
Molecular Formula
Structural Formula
Formula unit
Mole
Molar mass
Avogadro’s principle
Percent Composition
Objective Practice ProblemsDefine mole, Avogadro's number, and molar mass, and state how all three are related.
Calculate the number of atoms in a sample of any chemical element.
Perform mole-mass conversions.
69. How many atoms are in one mole of sulfur? _______________________________
70. How much volume does one mole of any gas at STP occupy? __________
71. Calculate the molar mass of the following compounds:Ca(OH)2 = Sulfur trioxide =
FeCl3 = Iron(III) sulfide=
72. How many moles are in 10.0g of potassium chlorate?
73. How many grams are in 2.2 moles of hydrosulfuric acid?
74. How many molecules are present in 2.50 moles of sulfur dioxide?
75. How many oxygen atoms are contained in 13.5 grams of carbonic acid?
76. What is the mass of 4.32 x 1025 molecules of ammonia (NH3)?
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Name:
Topic 6: The Mole (continued)Calculate the percent composition of a compound.
77. Calculate the percentage composition by mass of C12H22O11.
Determine the empirical formula and molecular formula of a compound.
78. An unknown compound is composed of 71.0% silver, 7.9% carbon, and 21.1% oxygen.Determine the empirical formula for this compound.
79. What is the molecular formula and name of this compound if it has been determined to have the molar mass of 303.8 grams?
Determine the chemical formula of a hydrate.
Experimentally determine the chemical formula of a hydrate.
80. Use the data below to determine the formula and name for the aluminum bromide hydrate, AlBr3•XH2O.
Mass of empty crucible and lid: 4.26 gMass of crucible, lid, and hydrate: 8.60 gMass of crucible, lid, and anhydrate (i.e., after heating): 7.35 g
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Name:
Topic 7: Chemical ReactionsHow do chemists quantify matter?
VocabularyTerm Definition
decomposition (analysis)
combination (synthesis)
single-replacement
double-replacement
combustion of a hydrocarbonneutralization reaction
Precipitate
Activity Series
Topic 7: Chemical ReactionsObjective Practice Problems
STATE the reasons why a chemical reaction must be balanced.
81. A balanced equation verifies the law of conservation of matter becausea. the molar masses of all substances are the sameb. the coefficients on both sides of equation are the samec. the moles of reactants equals the moles of productsd. the mass of reactants equals the mass of products
READ a chemical reaction properly and identify the major parts, such as products, reactants, yields, and phase states.
82. The equation that correctly describes the reaction at right isa. Al2 + 3 Cl2 --> Al2Cl6b. 2 Al + 3 Cl --> 2 AlCl3c. 2 Al + Cl2 --> 2 AlCld. 2 Al + 3 Cl2 --> 2AlCl3
83. Identify the products above:
84. Identify the reactants above:
85. Aqueous solutions of magnesium chloride and sodium hydroxide are mixed together to produce solid magnesium hydroxide. Write a complete balanced equation for this reaction (include phases).
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Cl
ClAl
Al
Al
Al
Cl
Cl
Cl
Cl
Cl
Cl
Cl
Cl
Cl
Cl
Name:86. What type of reaction is this? ________________________________
APPLY the rules for balancing chemical reactions to a given list of chemical reactions.
87. Balance the following equations:a. N2 + H2 NH3
b. Cs + H3PO4 Cs3PO4 + H2
c. MnO2 + HCl MnCl2 + H2O + Cl2
d. C4H10 + O2 CO2 + H2O
IDENTIFY and NAME the major types of chemical reactions- synthesis, single replacement, double replacement, combustion or decomposition.
PREDICT the products or reactants of a chemical reaction when given one or the other.
88. Properly predict the products, balance and name each of the reactions below. Assume all reactions occur (phases not needed)
Reactants Products Reaction Type
Ca(OH) 2 + H2SO4
Mg(ClO3) 2 + O2
K + O2
C7H16 + O2
Li + I2
Al + HCl
CaO
Zn + FeCl3
Al2 SO4)3 + MgCl2
Determine an activity series and predict whether or not a reaction will occur
89. Predict whether a reaction will occur for each of the following. If a reaction takes place, write a balanced chemical equation (including phases). If a reaction does not take place, write No RXN.
a. Cl2 (g) + KBr (aq)
b. NaOH (aq) + AlCl3 (aq)
c. Fe(NO3)2 (aq) + MgCl2 (aq)
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Name:
d. H2CO3 (aq) + Ba(OH)2 (aq) Topic 8: Stoichiometry
How do chemists predict the amount of products that can be produced by a chemical reaction?Vocabulary
Term Definitionstoichiometry
Limiting reactant
Excess reactant
Theoretical yield
Percent Yield
Precipitate
Topic 8: StoichiometryHow do chemists predict the amount of products that can be produced by a chemical reaction?
Objective Practice ProblemsPREDICT the amount of a substance being used or produced by a reaction using the method of stoichiometry
90. Determine the moles of hydrogen gas produced when 50 grams of aluminum are reacted with sulfuric acid.
91. Calculate the volume of hydrogen gas that must be burned with oxygen gas to form 4.0 moles of water at STP.
92. When 234 grams of HgO is heated until decomposition, what mass of mercury will be formed?
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Name:Topic 8: Stoichiometry (continued)
How do chemists predict the amount of products that can be produced by a chemical reaction?DETERMINE the limiting reactant in a chemical reaction
CALCULATE percent yield of a reaction.
93. 2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) + 3H2(g)According to the above balanced chemical equation, if you place 5.00 grams of aluminum into 5.00 grams of sulfuric acid….
a. How many grams of aluminum sulfate can be produced?
b. What is the limiting reactant? ___________________
c. Which reactant is in excess and by how much?
d. If the actual yield of the aluminum sulfate is 5.35 grams, what is the percent yield?
Determine the activity series of a set of reactions.
From the data below, determine the activity series of these six elements:X, Y, Z, H, Ba, and Hg, placing the most active one first in the box provided below.
Reactants Observations
X + HCl Bubbles formY + HCl No ReactionZ + BaCl2 No Reaction
Y + HgCl2 A liquid metal begins to appear
Z + HCl Bubbles formZ + XCl3 A dark substance begins to form on the Z metal
Work space: (if needed)
94. Activity Series:
most active ------------------------------------------------------------------> least active23
Name:
Topic 9: Acids/ Bases/ MolarityHow do acids and bases react in solution?
VocabularyTerm Definition
Solute
Solvent
Saturated Solution
Solution
Solubility
Molarity
Bronsted-Lowry Acid:
Bronsted-Lowry Base:
Titration:
Salt:
Buffer:
pH
Objective Practice ProblemsGiven two of the following values (molarity, mass, and volume), CALCULATE the third value.
95. How many grams of K2SO4 will be required to prepare 250mL of 0.5 M potassium sulfate?
96. How many grams of NaOH will be required to prepare 500mL of 0.25 M sodium hydroxide?
CALCULATE and DESCRIBE how to prepare a solution and perform a dilution
97. Describe how you would prepare 100mL of 0.1 M HCl from 1M HCl?
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Name:DIFFERENTIATE between an Arrhenius acid/base and a Bronsted-Lowry acid/base.
98. Label and connect the conjugate acid-base pairs in the following reactions:
NH4+ + OH- NH3 + H2O_________ _________ _________ _________
C2H3O2- + H2O HC2H3O2 + OH-_________ _________ _________ _________
99. Which reaction(s) above don’t fit Arrhenhius’s definition of an acid/base and WHY?
Topic 9: Acids/ Bases/ Molarity (continued)EXPLAIN the differences among an acid, a base, and a salt, and write balanced chemical equations for neutralization reactions.
100. Complete and balance the neutralization reactions shown below. Include the intermediate acid-base ions. Your completed reactions must be balanced..
HCl + Mg(OH)2
H3PO4 + Ga(OH)3
HNO3 + Ba(OH)2
RELATE the ideas of Ka, pH, and conductivity to acid-base chemistry, and describe the relationship among, Ka, pH and conductivity, and acid-base strength.
Given that HNO3, is a strong acid,
101. Would you expect the Ka value for nitric acid, HNO3, to be large or small?
_______102. Would the equilibrium mixture for nitric acid, HNO3, contain mainly products
or mainly reactants? _______103. When 4 moles of nitric acid dissolve in 1 liter of water, what will be the
approximate concentration of H3O+ ion formed? ________
104. Would HNO3 have a high or a low conductivity? __________
105. Would HNO3 have a high or a low pH value? __________
106. Below you are given three values for the concentration of H+ ions of three
different acids. Based on your knowledge of the relationship between [H+], pH, and conductivity, determine which of the three given pH values and relative
conductivities best matches each of the concentrations of H+.
[H+] pH (9.2, 6.9, or 1.4) Conductivity (high, medium, or low)
5.7 X 10-10M _______________ ___________
1.3 X 10-7M _______________ ___________
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Name:
4.4 X 10-2M _______________ ___________107. A solution has a hydrogen ion concentration of 3.42 x 10-10 M.
What is [OH-] of the solution?
What is the pH of the solution?
Is the solution acidic or basic? __________________EXPLAIN the principles involved in the titration of acids and bases, and use unit analysis to calculate concentrations or volumes in titration problems.
108. What is the molarity of a nitric acid solution if 43.3 mL of 0.100 M KOH solution is needed to neutralize 20.0 mL of the acid?
109. Based on the data gathered below after titrating an solution of sodium hydroxide of unknown concentration, calculate the average concentration of the unknown sodium hydroxide solution. Show all of your work.
Calculation Trial 1:
Calculation Trial 2:
Calculation Trial 3:
Average concentration of unknown NaOH solution:
Concluding questions If you were graded on the overall effort you put into this class, what grade do you think you would deserve? (Please answer this as honestly as possible!)
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Trial 1 Trial 2 Trial 3Initial burette HCl reading 0 15.0 29.2Final burette HCl reading 15.0 29.2 45.5
mL of acid addedVolume of NaOH solution 10.0 mL 10.0 mL 10.0 mL
Concentration of HCl 1.00 1.00 1.00Concentration of Unknown NaOH