Georgia GACE Chemistry (6-12) Assessment Practice Test
The Georgia GACE Chemistry (6-12) Assessment practice page covers chemical principles and quantitative problem solving relevant to secondary chemistry. The question bank samples ionic compounds, solution preparation, precipitation reactions, stoichiometry, acids and bases, nuclear decay, and electrochemistry, including interpreting equations and connecting particle-level behavior to observable properties.
Exam overview
About the Georgia GACE Chemistry (6-12) Assessment Exam
Chemistry questions call for translating among formulas, balanced equations, particle descriptions, and measured quantities. Practice may involve identifying ionic formulas from charges, writing net ionic equations for precipitates, calculating theoretical yield or limiting reactants, and using concentration and volume information in solution work. Other items examine how ion mobility explains electrical conductivity, how hydronium concentration relates to pH, and why strong and weak acids differ in ionization. Radioactive decay questions use parent-to-daughter proportions to infer elapsed half-lives, while electrolysis questions distinguish reduction at the cathode from oxidation at the anode. For secondary teaching, these concepts also support explaining calculations and chemical models clearly, checking units and significant figures, and diagnosing whether an answer is consistent with conservation of atoms and charge.
Sample Practice Questions
Review a selection from this exam's published US Practice Tests practice bank.
Which formula represents the compound formed from magnesium ions and nitride ions?
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Correct answer: CMagnesium forms Mg²⁺ and nitride is N³⁻. The smallest whole-number ratio that balances the charges is three magnesium ions to two nitride ions, giving Mg₃N₂.
A student dissolves 5.0 g of potassium chloride in water and transfers the solution quantitatively to a 250 mL volumetric flask, then fills to the calibration mark. What is the main purpose of filling precisely to the mark?
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Correct answer: AA volumetric flask is designed to prepare a solution at a specified final volume. Knowing that volume, together with the amount of solute, makes it possible to determine the solution concentration accurately.
A student mixes aqueous silver nitrate and sodium chloride. Which net ionic equation represents the formation of the solid product?
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Correct answer: ASilver chloride is insoluble in water and precipitates when Ag⁺ and Cl⁻ ions meet. Sodium and nitrate ions remain dissolved as spectator ions.
Which description best explains why a salt solution can conduct electricity while solid crystalline salt generally does not?
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Correct answer: BIonic solids contain charged ions, but those ions are fixed in the crystal lattice and cannot carry charge through the solid. When dissolved, many ions become mobile and can transport electrical charge.
A reaction uses 1 mol of nitrogen gas and 3 mol of hydrogen gas to form ammonia according to N₂ + 3H₂ → 2NH₃. What is the theoretical amount of ammonia produced?
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Correct answer: BThe balanced equation shows that 1 mol of N₂ reacts with 3 mol of H₂ to produce 2 mol of NH₃. The given reactant amounts are in the exact stoichiometric ratio.
A radioactive parent isotope decays into a stable daughter isotope. If a rock contains 25% parent isotope and 75% daughter isotope, and initially contained no daughter isotope, how many half-lives have elapsed?
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Correct answer: BAfter one half-life, 50% of the parent remains; after two, 25% remains. The remaining 75% has decayed into daughter isotope, so two half-lives have elapsed.
What is the pH of a solution whose hydronium-ion concentration is 1.0 × 10⁻³ mol/L?
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Correct answer: BpH = −log₁₀[H₃O⁺]. Substituting 1.0 × 10⁻³ mol/L gives pH = 3.
How to use this practice test
The free practice session presents up to 20 random questions from the 50-question bank. Work through the calculations and explanations implied by each prompt, then use the results shown after the session to identify which concepts or problem-solving steps need more attention.
Preparation tips
- Practice writing ionic formulas by balancing cation and anion charges, then check that the resulting compound is electrically neutral.
- For reaction calculations, balance the equation first, compare available reactants with mole ratios, and identify the limiting reactant before finding theoretical yield.
- Distinguish complete ionic equations from net ionic equations by canceling spectator ions; verify that atoms and total charge balance.
- Connect solution measurements to calculations: convert volume to liters for molarity work and use pH = −log[H₃O⁺] when hydronium concentration is given.
- Review redox conventions in electrolysis and isotope decay: reduction occurs at the cathode, and each half-life halves the remaining parent isotope.