1. * Name the following acids: * HI * HNO 3 * HCl * Write the formula for the following acids: * Hydrofluoric Acid * Nitrous Acid * Hydrobromic acid

2. Unit 10, Day 2 Kimrey 3 January 2013

3. * Chloric Acid * HClO 4 * Nitric Acid * H 2 C 2 O 4 * Phosphic Acid * HF * Hydroiodic Acid * HBr * Hydrochloric Acid * Perchloric acid * Hydroiodic acid * Sulfic acid / Sulfuric acid * Hydrosulfic acid / Hydrosulfuric acid * OMIT * Carbonic acid * Perbromic acid * Bromic acid * Acetic acid * OMIT * Hydrophosphic acid * HF * HNO 3 * HNO 2 * H 2 CO 3 * HMnO 4 * H 2 Cr 2 O 7 * H 2 SO 3 * H 2 SO 4 * HClO 4 * HClO 2 * HC 2 H 3 O 2 * H 3 PO 4 * 7-14 * No, Bases aren’t sour * Salt + water * Acetic acid- food * H 2 SO 4 - Battery Acid * NaOH- drano * Mg(OH) 2 - antacid

4. * Identify strong and weak acids * Calculate the pH and pOH of an acid given a concentration. * Determine the concentration of an acid given a pH or pOH.

5. * There are two strengths of acids: strong and weak. * Strong acids completely dissociate (break up) in water. * Weak acids do not completely dissociate. * There are 6 strong acids you need to memorize. * HCl * HBr * HI * H 2 SO 4 * HNO 3 * HClO 4

6. * pH is a logarithmic scale that measures the concentration of the [H + ] ion in solution. * Goes from 0 -14 * 0 - 6.99 is acidic * 14 – 7.01 is basic * pH = -log[H + ] * [H+]=10 -pH

7. * Don’t freak over logs and anti-logs, your calculator does them for you! * Ex. Find the pH of a HCl solution with a H+ concentration of 1 x 10 -6. * pH = -log[H + ] * pH = 6

8. * Find the pH of a 0.03 M solution of HBr. * pH = -log[H + ] * pH = 1.5

9. * What is the concentration of a HCl solution that has a pH of 3? * [H+]=10 -pH * [H+] =.001M

10. * Same as pH, but opposite. * Goes from 0 -14 * 0 - 6.99 is basic * 14 – 7.01 is acidic * pOH = -log[OH - ] * [OH-]=10 -pOH

11. * Calculate the pOH for a solution of NaOH with a concentration of 1 x 10 -4 M. * pOH = -log[OH - ] * pOH = 4

12. * Calculate the pOH for a solution of KOH with a concentration of 0.45 M. * pOH = -log[OH - ] * pOH =.35

13. * What is the concentration of a solution the has a pOH of 13.5? * [OH-] = 10 -pOH * [OH-] = 3.16 x 10 -14 M

14. * Remember that both the pH and pOH scale go from 0-14. * As the concentration of [H+] or [OH-] goes up the other must go down. * These two relationships allows us to assume that: * pH + pOH = 14

15. * What is the pH of a solution that is found to have a pOH of 10? * pH = 4

16. * What is the pH of a.067 M solution of LiOH? * pOH = 1.17 * pH = 12.8

17. * What is the pOH of a 0.0056 M solution of HCl? * pH = 2.25 * pOH = 11.75

18. * What is the pH of a solution HI with a concentration of.0089 M? * What is the concentration of a strong acid with a pH of 3.45? * What is the pH of a solution of a NaOH with a concentration of 5.67 x 10 -4 M?