1. Acids and Bases Review A game by Taylor Shupe and Mallory Mac

2. Arrhenius Acids Bronsted- Lowery Color Indictors Percent Ionization pHNeutralization 100 200 300 400

3. What produces H + in a solution What is an Acid

4. What type of solution has [OH - ]> 10 -7 and [OH - ]> [H + ]. What is Alkaline Solutions

5. Fill in the blank: H+H+ OH - Type of solution 1.0x 10 -3 ?? H+H+ OH - Type of solution 1.0x 10 -3 1.0x 10 -11 acidic

6. This particular case could not be an Arrhenius base. What is NH 3 ammonia

7. What is a base What is a proton acceptor?

8. What is a base When an acid loses a hydrogen ion it becomes a...

9. Conjugate base Fill in the blank:

10. Some substances, such as water, are amphoteric, what is another name for amphoteric? What is amphiprotic

11. Color indicators are organic compounds that establish equilibrium between their ________ form and ionic form in solution. What is molecular

12. The pH at which the color change occurs is called the ?. What is the end point

13. What type of indicator is this... What is phenolphthalein

14. A solution is tested: methyl red= yellow and bromothymol blue = yellow. What is the concentration of the sample? What is six

15. HCl is a strong acid. In an aqueous solution it will ionize % What is 100

16. H2SO4(aq) + HOH(l)  H3O+(aq) +HSO4-(aq) How many ionisable hydrogen(s) does this equation contain What is two

17. Find the percent ionization of 0.100M solution of formic acid if it’s [H + ] = 4.22x10 -3 M What is 4.22x10 -3 x 100 = 4.22% 0.1

18. A 0.40 M solution of HClO 3 is 0.027% ionized. Find the K a for this acid. [H + ] = 0.027 (0.40) = 1.08 x 10 -4 M 100 HClO 3(aq)  H + (aq) + ClO 3 - (aq) K a = [H + ][ClO 3 - ] [HClO 3 ] K a = (1.08 x 10 -4 )(1.08 x 10 -4 ) (0.3999) K a = 2.9 x 10 -8

19. Acids taste sour, bases taste ? What is bitter

20. An unknown acid has a H + of 3.9x10 -3, what is the OH - ? What is 2.6x10 -12

21. Find the pOH of a solution with a [H + ] of 6.7x10 -3 What is 11.8

22. Acid + Base  + water What is salt

23. Calculate the volume of seawater with a pH of 7.80 that contains 1.0 mol of hydroxide ions. pH = 7.8 = pOH = 6.2 = [OH - ] = 6.3 x 10 -7 M 6.3 x 10 -7 mol = 1 L 1 mol = ?L = 1.58 x 10 6 L

24. A is a technique for finding an unknown concentration of one chemical from the known concentration of a second chemical. What is titration

25. Find the concentration of an HF solution if 15.0 mL of 0.200 M KOH just neutralized 20.0 mL of HF. HF + KOH → KF + H 2 O Step 1n = MV = (0.200 mol / L)(0.0150 L) = 0.00300 mol KOH Step 2 x mol HF = 0.00300 mol KOH x 1mol HF = 0.00300 mol HF 1 mol KOH Step 3M = n = (0.00300 mol) = 0.150 mol = 0.150 M V (0.0200 L) L

26. A titration shows that 242 mL of 0.500 M NaOH will just neutralize all of the acetic acid that is present in 150.0 mL of vinegar. Find the % by mass of acetic acid in vinegar. NaOH + HC 2 H 3 O → NaC 2 H 3 O 2 + H 2 O Step 1 n = MV = (0.500 mol) (0.242 L) = 0.121 mol NaOH L Step 2 x mol HC 2 H 3 O 2 = 0.121 mol NaOH x 1 mol HC 2 H 3 O 2 = 0.121 mol HC 2 H 3 O 2 1 mol NaOH Step 3 x g HC 2 H 3 O 2 = 0.121 mol HC 2 H 3 O 2 x 60 g HC 2 H 3 O 2 = 7.26 g HC 2 H 3 O 2 1 mol HC 2 H 3 O 2 Step 4 % mass = 7.26 g x 100 = 4.84% acid 150.0 g assumed