1. What is the acid concentration if 0.4 moles is dissolved in 150 cm 3 ? Molarity Check

2. What is an ACID?

3. What is an BASE?

4. What is an acid? What is a base? NaOH + HCl NaCl + H 2 O MgCO 3 + 2CH 3 COOH (CH 3 COO) 2 Mg + H 2 O + CO 2 NH 3 + HCl NH 4 Cl

5. Bronsted-Lowry Acids and Bases

6. Objectives 1. Define Bronsted-Lowry acids and bases 2. Identify Bronsted-Lowry acids and bases in equations 3. Explain the difference between monoprotic and diprotic acids

7. “A substance which donates protons in a reaction. A proton donor.” Bronsted-Lowry Acid

8. “A substance which accepts protons in a reaction. A proton acceptor.” Bronsted-Lowry Base

9. “Involve proton transfer from acid to base.” Bronsted-Lowry Acid-Base reactions

10. Example: The reaction between sodium carbonate and hydrochloric acid. Na 2 CO 3 + 2HCl 2NaCl + CO 2 + H 2 O In ionic form, this is written as:

11. Example 1 The reaction between sodium carbonate and hydrochloric acid. Na 2 CO 3 + 2HCl 2NaCl + CO 2 + H 2 O In ionic form, this is written as: CO 3 2- (aq) + 2H + (aq) CO 2 (g) + H 2 O(l)

12. H 2 SO 4 (aq) + HNO 3 (aq) ↔ H 2 NO 3 + (aq) + HSO 4 - (aq) H 2 SO 4 = Bronsted-Lowry acid (H + donor) HNO 3 = Bronsted-Lowry base (H + acceptor) HSO 4 - = Bronsted-Lowry base H 2 NO 3 + = Bronsted-Lowry acid Acid 1 Base 1 Acid 1Base 2 Acid 2 Identify the acid and base in the forward & backward reactions

13. H 2 O(aq) + NH 3 (aq) ↔ NH 4 + (aq) + OH - (aq) H 2 O = Bronsted-Lowry acid (H + donor) NH 3 = Bronsted-Lowry base (H + acceptor) OH - = Bronsted-Lowry base NH 4 + = Bronsted-Lowry acid Acid 1 Base 1 Acid 1Base 2 Acid 2

14. H 2 O(aq) + H 2 O(aq) ↔ H 3 O + (aq) + OH - (aq) H 2 O = Bronsted-Lowry acid (H + donor) H 2 O = Bronsted-Lowry base (H + acceptor) OH - = Bronsted-Lowry base H 3 O + = Bronsted-Lowry acid Acid 1 Base 1 Acid 1Base 2 Acid 2

15. Monoprotic vs Diprotic Acids