1. Acid, Base, and Salt What I know?

2. The name for HBr is _____ acid. Hydrobromic Acid

3. I feel slippery; therefore, I am a _________. BASE

4. Can I get burned by a base? Yes

5. Which reactant acts as a Brønsted- Lowry acid in this equation? HCl (g) + H 2 O (l)  H 3 O 1+ (aq) + Cl 1- (aq) HCL

6. Name the following: NaOH CaSO 4 NaC 2 H 3 O 2 sodium hydroxide calcium sulfate Sodium acetate

7. The [ ] around H+ in the pH formula mean this. Molar Concentration A substance that has both acid and base qualities is called this.

8. Sulfuric Acid Nitric Acid Hydrochloric Acid

9. I have a pH of 3 so I am an ___________. Acid A substance that has both acid and base qualities is called this.

10. Amphoteric

11. What method is used to visually detect the end of a titration? Addition of an indicator that will turn color at a given pH

12. pOH measures this. The concentration of the hydroxide ion(OH - )

13. What is the pH of a 0.00001M solution of HCl? pH 5

14. The type of reaction that occurs when an acid reacts with a base to form salt and water. Neutralization

15. HF + Ca(OH) 2 → F - + H 2 O Identify the acid and base in the reaction above. HF acid Ca(OH) 2 base

16. Would LiOH or C 6 H 12 O 6 be a stronger electrolyte? LiOH

17. What is the pH of a solution having a hydrogen ion concentration, [H 1+ ], of 0.010 mole/liter? pH = 2

18. What is the pH of a solution having a solution of NaOH with a concentration of 3.5 x 10 -3 M? pH is 11.5

19. If I am bitter, I am a ___________. BASE

20. KOH + H 2 SO 4 → H 2 O + SO 4 2- Identify the conjugate acid and conjugate base in the reaction above. H 2 O conjugate acid SO 4 2- conjugate base Recall a Bronsted-Lowrey acid dontates a proton.

21. Can I get burned by acids? Yes

22. I turn litmus paper red, so I would be classified as ________________ Acid

23. If 20 mL of NaOH are titrated with 45 mL of 0.01M HCl, what is the concentration of the NaOH? 0.02M NaOH

24. pH = 7

25. Which reactant acts as a Brønsted- Lowry acid in this equation? HBr (g) + H 2 O (l)  H 3 O 1+ (aq) + Br 1- (aq) HBr

26. Which solution, when placed in the beaker, will cause the bulb to glow the brightest? deionized water, sugar, acetic acid or HCl HCl

27. The value of pH is defined as the negative log of the _____. Hydrogen ion concentration or [H + ]

28. If the pOH of a sodium hydroxide solution is 5, what would be the pH of the solution? pH 9

29. Using the chart below, select the best indicator to use when the end point and equivalence point of a titration are at pH = 7. indicatorpH range of indicator Methyl orange3.3 – 4.5 Bromthymol blue6 – 7.6 phenolphthalein8 - 10 Bromthymol blue