1. No QOTD Today 5/16/14 Please have your HW out to be checked off (p. 71-72) Please pick up the HW key and check your work. We will have time to ask questions after I finish checking off HW. Remember that “chemistry in my life” posters are due Monday!

2. Learning Target 1. You should be able to describe the effect on pH when water is added to an acid, a base or salt water. 2. You should be able to describe the relationship between [H+], [OH-], pH and pOH and perform calculations to determine missing information. QUIZ over acids, bases and pH on Tuesday!

3. Turn and Talk #1: diluting HCl [ HCl ]pH 1.0 M0 0.1 M1 0.01 M2 0.001M3 0.0001 M4 0.00001 M5 0.000001 M6 0.0000001 M7 0.00000001 M? 1.How does diluting acid affect the acidity? 2.If you continue to dilute the solution, will you get a pH above 7? Why or why not? 3.What do you think will happen to the pH if you were to dilute the last solution even more?

4. Diluting HCl [ HCl ]pH 1.0 M0 0.1 M1 0.01 M2 0.001M3 0.0001 M4 0.00001 M5 0.000001 M6 0.0000001 M7 0.00000001 M? 1.How does diluting acid affect the acidity? Acidity decreases (lower H 3 O + concentration) 2.If you continue to dilute the solution, will you get a pH above 7? Why or why not? NO! It will still have some acid in it and acids are never above pH 7! 3.What do you think will happen to the pH if you were to dilute the last solution even more? It will not change. It is already neutral!

5. Turn and Talk #2: diluting NaOH [ NaOH ]pH 1.0 M14 0.1 M13 0.01 M12 0.001M11 0.0001 M10 0.00001 M9 0.000001 M8 0.0000001 M7 0.00000001 M? 1.How does diluting base affect the basicity? 2.If you continue to dilute the solution, will you get a pH above 7? Why or why not? 3. What do you think will happen to the pH if you were to dilute the last solution even more?

6. Turn and Talk #2: diluting NaOH [ NaOH ]pH 1.0 M14 0.1 M13 0.01 M12 0.001M11 0.0001 M10 0.00001 M9 0.000001 M8 0.0000001 M7 0.00000001 M? 1.How does diluting base affect the basicity? Basicity decreases (lowers OH - concentration) 2.If you continue to dilute the solution, will you get a pH above 7? Why or why not? NO! Bases are always above pH 7 3. What do you think will happen to the pH if you were to dilute the last solution even more? The pH will stay at 7 (it is already neutral)

7. Turn and Talk #3: diluting NaCl [ NaCl ]pH 1.0 M7 0.1 M7 0.01 M7 0.001M7 0.0001 M7 0.00001 M7 0.000001 M7 0.0000001 M7 0.00000001 M? 1.How does diluting NaCl affect the pH? Why? There is no effect! NaCl is neither an acid nor a base! Therefore, you don’t change either [H 3 O + ] or [OH - ] when you add water.

8. Activity Turn to page 68-69. Fill in the tables and answer the questions. We will debrief these in about 15 minutes. If you finish early, ask me for the homework!

9. Answers p. 68 SubstanceAcid? Base? pH[H + ] decimal[H + ] scientific notation? 1 M HClAcidic01 M1.0 x 10 0 0.1 M HClAcidic 10.1 M1.0 x 10 -1 Clear sodaAcidic30.001 M1.0 x 10 -3 Rain waterAcidic60.000001 M1.0 x 10 -6 Distilled water Neutral70.0000001 M1.0 x 10 -7 AlcoholNeutral70.0000001 M1.0 x 10 -7 Salt waterneutral70.0000001 M1.0 x 10 -7 Washing soda Basic80.00000001 M1.0 x 10 -8 AmmoniaBasic100.0000000001 M1.0 x 10 -10 0.1 M NaOHBasic130.0000000000001 M1.0 x 10 -13 1 M NaOHbasic140.00000000000001 M1.0 x 10 -14

10. Answers p. 68 1.If you know [H + ] in decimal form, how do you find the pH? pH = decimal place the 1 is in (0.1 has the digit in the 1 st decimal place and has pH = 1) 2.If you know [H + ] in scientific notation, how do you find the pH? pH = the exponent number (without the – sign). But the only works if you have 1.0 as the coefficient! Ex: 1.0 x 10 -4 would have pH = 4 3.As the value of pH increases, what happens to [H + ] ? It decreases 4. As the value of pH decreases, what happens to [H + ] ? It increases

11. Answers p. 68 5.Solution A has a pH of 5. Solution B has a pH of 9. a)What is [H + ] for each solution? A = 1.0 x 10 -5 M B = 1.0 x 10 -9 M b) Identify if they are acidic or basic A = acidic B = basic (hey, those match the letter numbers! c) How many times more acidic is the acid than the base? A is 10 4 times more acidic (10,000 times more!)

12. p. 69 table (HCl) WellpH[H + ][OH - ]pOH A11.0 x 10 -1 M1.0 x 10 -13 M13 B21.0 x 10 -2 M1.0 x 10 -12 M12 C31.0 x 10 -3 M1.0 x 10 -11 M11 D41.0 x 10 -4 M1.0 x 10 -10 M10 E51.0 x 10 -5 M1.0 x 10 -9 M9 F61.0 x 10 -6 M1.0 x 10 -8 M8 G71.0 x 10 -7 M 7 H7 7 I7 7

13. p. 69 table (NaOH) WellpH[H + ][OH - ]pOH R71.0 x 10 -7 M 7 Q7 7 P7 7 O81.0 x 10 -8 M1.0 x 10 -6 M6 N91.0 x 10 -9 M1.0 x 10 -5 M5 M101.0 x 10 -10 M1.0 x 10 -4 M4 L111.0 x 10 -11 M1.0 x 10 -3 M3 K121.0 x 10 -12 M1.0 x 10 -2 M2 J131.0 x 10 -13 M1.0 x 10 -1 M1

14. p. 69 answers 1.What does [OH - ] stand for? Molar concentration of hydroxide ions 2. What can you say about [OH - ] in solutions with high acidity? [OH - ] will be very low 3.How is the value of pH related ot the value of pOH for each concentration? If pH is 1, then pOH is 13. THEY ALWAYS ADD UP TO 14! pH = pOH = 14

15. p. 69 answers 4.If you know the value of pH, how do you determine pOH? Subtract pH from 14 to get pOH 5. If you know the value of pOH, how do you find pH? Subtract pOH from 14 to get pH

16. pH equations ( you’ll want these for the HW ) pH is an example of a “p function”: p(stuff) = - log(stuff) pH = - log [H + ] = - log [H 3 O + ] pOH = - log[OH] pH + pOH = 14 So to find the pH of a base, find pOH and subtract from 14

17. Practice Problems (use calculator!) pH = -log[H + ] pOH = - log[OH - ] pH + pOH = 14 1. What is the pH of a 0.25 M HCl solution? pH = - log(0.25) = 0.6 2. What is the pH of a 12 M HCl solution? pH = - log(12) = -1.08 (yes, it CAN be negative!) 3. What is the pH of a 0.5 M NaOH solution? (hint: find pOH first since this is a base) pOH = -log(0.5) = 0.3 pH = 14-pOH = 14 – 0.3 = 13.7

18. Homework Answer HW Qs 1-6 on p. 70