AP Chemistry Unit 1 Practice Test 2014-2015 - Section I and II

Sep 30, 2026

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AP Chemistry Unit 1 practice test covering core chemistry concepts through multiple-choice and free-response problems. Section I tests solution behavior, solubility and precipitate formation, stoichiometry, net ionic equations, atomic structure, molarity and ion concentration, oxidation numbers, empirical to molecular formula possibilities, reaction coefficient balancing, and redox identification. Section II includes quantitative molarity dilution, balanced net ionic equations for several acid-base reactions, and an acid-base neutralization requiring identification of acid and base and calculation of mass needed for complete neutralization.

LanguageEnglish

CategoryExam

FormatPDF

Pages7

Reading Time18 min

AccessFree to download

Section I: Multiple Choice

1-15

Section II: Free Response

1-3

XXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXX AP Chemistry Unit 1 Practice Test 2014-2015 Section I: Multiple Choice Name: Directions: You have 20 minutes to complete Section I. NO CALCULATORS PERMITTED. Each set of lettered choices below refers to the numbered questions or statements immediately following it. Select the one lettered choice that best answers each question or best fits each statement and bubble in the corresponding letter on the scantron. 1. Which of the following compounds will form a solution with water that is a good conductor of electricity? A) C2H6 C) HBr B) HF D) NH3 2. The mass of CuSO4 (molar mass 160. g/mol) in 20.0 milliliters of 3.00 molar solution is A) 0.0375 grams C) 9.60 grams B) 4.50 grams D) 320. grams 3. When silver nitrate solution was added to a solution containing two ions, a precipitate formed with one ion but the other ion was soluble. The solution could have contained: A) chlorate ion & copper (II) ion B) potassium ion & barium ion C) lead(II) & iodide ion D) barium ion & acetate ion 4. 2N2H4(g) + N2O4(g) Æ 3N2(g) + 4H2O(g) When 8.0 g ofN2H4 (MM = 32 g/mol) and 92 g ofN2O4 (MM = 92 g/mol) are mixed together and react according to the equation above, what is the maximum mass of H2O that can be produced? A) 9.0 g B) 18 g C) 36 g D) 72 g E) 144 g 5. What is the net ionic equation for the reaction of calcium chlorate(aq) with potassium sulfate(aq)? A) Ca2+(aq) + 2 K+(aq) o CaK2(s) B) CaCl2(aq) + KSO4(aq) o 2KCl(aq) + CaSO4(aq) C) K+(aq) + ClO3- (aq) o KClO3(s) D) Ca2+(aq) + SO42- (aq) o CaSO4(s) XXXXXXXXXXXXXXXXXXXXXXXXXXXXXXX Unit 1 Practice Test XXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXX XXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXX AP Chemistry Unit 1 Practice Test 2014-2015 6. A species with 11 protons and 10 electrons is A) Ne C) F B) Na+ D) Mg2+ 7. If 87 grams ofK2SO4 (molar mass 174 grams) is dissolved in enough water to make 250 milliliters of solution, what is the molar concentration of the resulting solution? A) 0.020 M C) 2.0 M B) 1.0 M D) 4.0 M 8. What is the molar concentration of nitrate ions in a 3.0 M Ba(NO3)2 solution? A) 3.0 M C) 9.0 M B) 6.0 M D) 12 M 9. Potassium sulfide has a molar mass of 103 g/mol. How many moles of potassium sulfide are in a 51.5 g of potassium sulfide? A) 0.25 mol B) 0.50 mol C) 1.0 mol D) 2.0 mol E) 6.0 x 1023 mol 10. The net ionic equation for the reaction that occurs when solutions of hydrofluoric acid and sodium hydroxide are mixed is A) HF(aq) + OH- (aq) o H2O(l) + F- (aq) B) HF(aq) + NaOH(aq) o H2O (l) + Na+(aq) + F- (aq) C) Na+(aq) + F- (aq) o NaF(s) D) H + (aq) + OH- (aq) o H2O(l) 11. The permanganate ion produces a purple color in solution. A stock solution of KMnO4 with a concentration of 1 M is prepared. Several dilutions are performed and the resulting solutions areplaced into a colorimeter to measure the absorbance of light. Which solution will absorb the most light? A) 5 mL of stock solution + 5 mL of water B) 8 mL of stock solution + 2 mL of water C) 5 mL of stock solution + 15 mL of water D) 10 mL of stock solution + 10 mL of water XXXXXXXXXXXXXXXXXXXXXXXXXXXXXXX Unit 1 Practice Test XXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXX XXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXXX AP Chemistry Unit 1 Practice Test 2014-2015 12. What are the oxidation numbers for each element in KClO3? A) +1, +2, -2 C) +1, +5, -2 B) +1, +2, -4 D) +1, +7, -2 13. The empirical formula for a compound is N2O. Which of the following could be a molecular formula for the compound? A) N3O C) N4O3 B) N2O3 D) N8O4 14. What is the coefficient for KNO3(aq) when the following equation is balanced with lowest integers? K3PO4(aq) + Fe(NO3)2(aq) —> Fe3(PO4)2(s) + KNO3(aq) A) 1 B) 2 C) 4 D) 6 E) 12 15. In th

FAQs

What is the time limit and calculator rule for Section I?

Section I provides 20 minutes. No calculators are permitted.

How do you find the volume of 6.0 M AgNO3 needed to prepare 250.0 mL of 2.00 M AgNO3?

Use the dilution relationship M1V1 = M2V2 to solve for V1 with the given molarities and final volume.

In Section II question 3, what are you asked to identify and calculate in the acid-base reaction?

You name the base and acid used, then calculate the grams of NaHCO3 required to completely neutralize a specified volume and molarity of HClO4.

Sep 30, 2026

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