Notes

1. Which. of the following is considered a heterogeneous mixture?
D. Both colloids and suspensions

2. When sunlight strikes a cloud, the light is scattered by the cloud due to which of the following reasons?
A. The Tyndall effect caused by the colloidal particles in the cloud

3. Why is it necessary to shake an oral suspension medicine before administering it?
B. To mix the active ingredient because particles settle at the bottom

4. Which of the following illustrates a solid solution?
A. Brass

5. Which of the following is a characteristic of an electrolyte solution?
A. It consists of many molecules when dissolved in water, leading to the light. buyld glowing brightly.

6. At 60 °C, 71 g of KBr are dissolved in 100g of water. This solution is considered to be:
C. Supersaturated

7. Which salt is the least soluble at 20 degrees C?
A. KNO3

8. A chemist studied a supersaturated solution of NaClO₃ in a beaker containing 100 grams of water. Starting at 20 °C, the chemist added enough NaClO₃ to produce a saturated solution. Then, more NaClO₃ was added until the solution reached 60°C. If the chemist cools the solution back to the original 20°C, how much of the solute will crystallize at the bottom of the beaker?
C. 60grams

9. Which of the following best describes a saturated solution in terms of solution equilibrium as shown in the illustration on the right?
C. A solution in which the solute concentration is exactly at its solubility limit, with dissolution and crystallization occurring at equal rates.

10. Which of the following factors does NOT affect the rate of dissolution/dissolving?
D. Density of the solvent

11. Which solution is most concentrated?
A. Solution A

12. Glucose is a sugar that is found abundantly in nature. What is the percent by mass of glucose in a solution made by dissolving 163 g of glucose in 755 g of water?
A. 21.6%

13. How many mL of hydrogen peroxide are needed to make an 8.5% solution by volume of hydrogen peroxide if you want to make 450 mL of solution?
B. 38.25 mL

14. What is the proper way to prepare 250 mL of a 0.1 M dilute solution from a 1 M stock solution in a laboratory?
B. Measure 25 mL of the 1 M stock solution using a pipet, transfer it to the 250 mL volumetric flask, and dilute by adding distilled water until it reaches the mark.

15. What is the mass of NaCl in 1 liter of a 2.5 M NaCl solution?
D. 146.1 g

16. Which color does blue litmus paper turn when dipped in an acidic solution?
A. Red

17. What color change can be expected when phenolphthalein is introduced to an acidic or basic solution?
D. Both B and C are correct

18. How does bromothymol blue indicator behave in an acidic environment?
C. It turns yellow

19. In a particular experiment, a student aims to determine whether the solution is acidic or basic. If the pH paper registers a pH of 6, what conclusion can be drawn regarding the solution?
B. The solution is slightly acidic.

20. Which of the following is NOT a typical property of acids?
C. Feels slippery

21. Which of the following is a binary acid?
A. HBr

22. What is the correct name for the base Fe(OH)₂?
A. Ferrous hydroxide

23. Which statement is TRUE about acids and bases?
A. They react to form salts and water in a neutralization reaction.

24. Which of the following is an Arrhenius base?
D. Ca(OH)₂

25. According to the Bronsted-Lowry definition, what defines an acid?
A. It donates a proton (H⁺).

26. Which of the following chemical equations represents a reaction involving a weak acid?
B. CH₃COOH + H₂O ⇌ CH₃COO⁻ + H₃O⁺

27. In the reaction involving CH₃COOH + H₂O ⇌ CH₃COO⁻ + H₃O⁺, which substance acts as a strong acid?
D. H₃O⁺ (hydronium ion)

28. In the reaction, HF + H₂O ⇌ F⁻ + H₃O⁺, which of the following act as bases?
D. H₂O and F⁻

29. Which of the following statements highlights the main difference between a strong acid and a strong base?
A. Strong acids and bases dissociate completely in water.

Which of the following chemical reactions represents a weak base?
A. NH₃ + H₂O ⇌ NH₄⁺ + OH⁻