Name: ______Date: ______Period: ______

HONROS Chemistry Second Semester Final Exam Study Guide

For any problems involving calculations you MUST show all work with units.

Study guide will be checked on a daily basis for completion grade and is due on the day of the final exam.

1 mole = 22.4 Liters
1 mole = 6.02 x 1023 particles
1 mole = (molar mass) g
___ mole A = ___ mole B /

[H+1] x [OH-1] = 1 x 10-14 / pH = - log [H+]
pOH = - log [OH-1]
pH + pOH = 14
[H+1] = 10-pH
[OH-1] = 10-pOH
  1. Nomenclature: for each of the following compounds below write the chemical name or the chemical formula.

  1. hydroiodic acid
  2. manganese(II) oxide
  3. chromium(II) chlorite
  4. hydrofluoric acid
  5. nitrous acid
  6. lead(IV) nitride
  7. aluminum peroxide
/
  1. cobalt(III) sulfate
  2. strontium sulfide
  3. dinitrogen trioxide
  4. barium hydroxide
  5. tetrarsenicdecoxide
  6. bromine trioxide
  7. barium nitrate
/
  1. Mg(SO3)2
  2. NaClO3
  3. Sn(ClO2)4
  4. Hg3(PO4)2
  5. SrCO3
  6. PCl5
  7. P2O5
/
  1. HBr
  2. HCl
  3. HNO3
  4. S2Cl2
  5. BaCl2
  6. NaBr
  7. Fe2O3

  1. Six Types of reactions: combination (synthesis), decomposition, combustion, single replacement, double replacement, neutralization
  2. the substance(s) created by a chemical reaction are call the ______
  3. the substance(s) that start a chemical reaction are call the ______
  4. state 4 observation thatare evidence a chemical reaction (change) has occurred?
  5. Describeeach of the 6 major types of reactions?
  6. Give an example for EACH of the 6 types of reactions.
  1. Balance the following chemical reactions and identify the type of reaction occurring. If names are given you MUST FIRST balance charges to writhe the chemical formulas.

a)___CaCO3(s) + ___HCl(aq) → ___H2O(l) + ___CO2(g) + ___CaCl2(aq)

b)___ HBr + ___ Al(OH)3 ___ H2O + ___ AlBr3Type of reaction: ______

c)___Mg (s) +__ HCl(aq) → ___MgCl2 (aq) + ___H2(g)Type of reaction: ______

d)___ NaBr + ___ Ca(OH)2 ___ CaBr2 + ___ NaOHType of reaction: ______

e)___SO2(g) +___ O2(g) → ___SO3(g)Type of reaction: ______

f)___ NH3+ ___ H2SO4 ___ (NH4)2SO4Type of reaction: ______

g)___Fe(NO3)2(aq) + ___H2S(g) → ___FeS(s) + ___HNO3(aq)Type of reaction: ______

h)___ C5H9O + ___ O2 ___ CO2 + ___ H2OType of reaction: ______

i)___ Pb + ___ H3PO4___ H2 + ___ Pb3(PO4)2Type of reaction: ______

j)___NH4OH(aq)→___ NH3(g) + ___H2O(l)Type of reaction: ______

k)barium chloride(aq) and silver nitrate (aq) are mixed to form solid silver chloride and aqueous barium nitrate Type of reaction: ______

l)Hydrogen gas and oxygen gas react to make hydrogen peroxide.Type of reaction: ______

m)Sulfuric acid and calcium hydroxide react to make water and calcium sulfate. Type of reaction: ______

  1. Predict the productsof the following reactions, and identify the type of reaction
  2. NaOH(aq) + H2SO4(aq) →Type of reaction: ______
  3. Zn (s) + HCl(aq)→Type of reaction: ______
  4. AgNO3(aq) + BaCl2(aq) →Type of reaction: ______
  5. Fe2(SO4)3(aq) + Ba(OH)2(aq)→Type of reaction: ______
  6. KNO3(aq) + BaCl2(aq) →Type of reaction: ______
  7. H2O (l) →Type of reaction: ______
  8. Hg + O2→Type of reaction: ______
  1. Stoichiometry [SHOW ALL calculations with units and chemical formulas]
  2. Calculate the theoretical yield in grams of iron in the reaction of 687.5 g of iron (III) oxide with excess carbon, according to the equation: 2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g)
  3. If 167g of Fe3O4 is reacted with excess CO, what mass of CO2 will be produced, according to the equation Fe3O4(s) + 4CO(g) → 4CO2(g) + 3Fe(s)
  4. What mass of Silicon Nitride [Si3N4]is produced from 35.0 g of Nitrogen given the following equation? 3 Si + 2 N2 → Si3N4
  5. What mass of Iron (III) Bromide [FeBr3] is produced from 78.9 g of Bromine given the following equation? 2Fe + 3 Br2 2 FeBr3
  6. What mass of Silicon Nitride [Si3N4] is produced from 35.8 g of Silicon given the following equation? 3 Si + 2 N2 → Si3N4
  7. If I start the following reaction with 63.4 grams of magnesium and an excess of nitric acid, how many grams of hydrogen gas will I produce? 2 HNO3 + Mg  Mg(NO3)2 + H2
  8. If 48.5 grams of carbon dioxide gas is produced in this reaction, how many grams of sodium hydroxide should be produced? NaHCO3 CO2 + NaOH
  1. Percent Yield [SHOW ALL calculations with units and chemical formulas]
  2. If the actual yield of Iron in problem 5a is 102.5 g what is the percent yield?
  3. If the actual yield of Silicon Nitride [Si3N4] in problem 5c is 64.4 g what is the percent yield?
  4. If the actual yield of Iron (III) Bromide [FeBr3] in problem 5d is 120.5 g what is the percent yield?
  1. Limiting reactant [SHOW ALL calculations with units and chemical formulas]
  2. how can you determine which reactant is limiting in a problem?
  3. determine thelimiting reagent if 26.5g ofAl2(SO3)3is reacted with 26.5 g NaOH? Al2(SO3)3+ 6NaOH --> 3 Na2SO3 + 2 Al(OH)3
  4. What is the limiting reactant if you have 68.5 of Al(NO4)3 and 35.3 g of KCl?Al(NO4)3 + 3 KCl AlCl3 + 3 KNO4
  5. determine the limiting reagent if 26.5g of Al2(SO3)3 and 68.4g of NaOH Al2(SO3)3 + 6 NaOH --> 3 Na2SO3 + 2 Al(OH)3

Acid and Bases

  1. List 3 properties of just ACIDS:
  1. List 3 properties of just BASES:
  1. List 3 properties of BOTH acids & bases:
  1. In a neutral solution the
  2. pH = ______c. pOH = ______
  3. [OH-1] = ______d. [H+] = ______
  1. Acid/Base definitions
  2. Arrhenius acid:
  3. Arrhenius base:
  4. Bronsted-Lowery acid:
  5. Bronsted-Lowery base:
  6. Lewis acid:
  7. Lewis base:
  1. Define and give an example for each of the following:
  2. Monoprotic acids
  3. Diprotic acids
  4. Triprotic acids
  1. Complete the table

Base / Conjugate acid / Acid / Conjugate base
SO4–2 / HNO2
F-1 / HC2H3O2
HO1- / HSO4–1
NO3-1 / HCO3–1
HSO4-1 / H2S
CO3–2 / H2CO3
  1. Are the following conjugate acid/base pairs? Why or why not?

a)SO3-2 and SO2
b)CN-1 and OH-1
c)H3O and H2
d)NH4+1 and NH3 / e)H2O and OH-1
f)H2SO4 and HSO3-1
g)CO3-2 and HCO3-1
h)CO3-2 and CO
  1. Identify the acid, base, conjugate acid, conjugate bases in the following reactions
  2. NH4+1 + HSO4-1 → H2SO4 + NH3
  3. HNO3 + OH- H2O + NO3-
  4. CH3NH2 + H2O  CH3NH3+ + OH-
  5. OH- + HPO4-2 H2O + PO4-3
  6. NH3 + H2O → OH-1 + NH4+1
  7. H2O + H2PO4-1 → OH-1 + H3PO4
  1. Calculations with pH, pOH, [OH-], or [H+]and determine if the substance is Acidic, basic or neutral!! [SHOW ALL calculations]
  2. Calculate the [OH-] and pOH in a solution that has a pH of 7.30.
  3. Calculate the pH and [OH-1] if [H+1]= 7.48 x 10-2
  4. Calculate the [H+] and [OH-] in a solution that shows a pOH of 12.07.
  5. Calculate the pH, pOH, and [OH-] of 1.0 x 10-3 M H+1.
  6. Calculate the pH if [OH-1] = 3.68 x 10-7
  7. Calculate the pH pOH, and[H+] of a solution that has [OH-] = 3.58 x 10-8 M?
  8. Calculate the pOH, pH and [OH-1 if [H+1]= 9.28x 10-10
  1. Complete the following table

pH / pOH / [H+1] / [OH-1] / Acid/Base/Neutral
8.25
1 x 10-7
3.53 x 10-11
5.14
2.35 x 10-6
  1. Molarity: [SHOW ALL calculations with units and chemical formulas]
  2. Define molarity
  3. Find the molarity of a solution made with 559 mL and 35.6 g of HC2H3O2
  4. What is the mass of H3PO4 used to make 98 mL of a 3.14 M solution?
  5. What is the volume needed to make 1.25 M solution with 25.5 g of NaOH?
  6. Define concentrated solution
  7. Define dilute solutions.
  8. How do concentrated and dilute solutions they differ from each other.
  9. What are the three thing that you can do to dissolve a solid faster in a solvent?
  10. What are the three thing that you can do to dissolve a gas faster in a solvent?
  1. Using the chart what are different types of solutions (saturated, unsaturated or super saturated) formed when the following mass of potassium chloride (KCl) is dissolved at 450C
  2. 40 grams
  3. 50 Grams
  4. 30 grams
  1. How many grams of KClO3 can dissolve at 40°C in the following amounts of water?
  2. 300 g H2O
  3. 25 g H2O
  4. 5500 g H2O