1 Chapter 19 Objectives: 1) Differentiate between acids and bases. 2) Explain the following three acid-base theories: Arrhenius, Bronsted-Lowry, Lewis. 3) Be able to name and write formulas for binary and ternary acids. 4) Be able to name and write formulas for hydroxide bases. 5) Differentiate between strong and weak acids and bases (with examples of each). 6) Explain pH.

2 7) Know the pH scale with a few examples. 8) Define salt. 9) Define neutralization reaction. 10) Describe using an illustration what titration is and what it is used for. 11) Be able to use molarity and volume to solve titration problems.

3 CH. 19 Acids, Bases, and Salts I) Acids vs. Bases * ______: any substance which produces __________ ions, ____, in water solutions; is a proton _______; is an electron pair __________; and tastes _____. * ______: any substance which produces ___________ ions, ____, in water solutions; is a proton __________; is an electron pair _______; and tastes ________.

4 A) Arrhenius Theory: *Observed that some solutions conducted electricity (demo conductivity). 1) Svante Arrhenius concluded that acids were substances that ionized in water to form hydrogen ions, ___. HCl 

5 Bases ionized in water to form hydroxide ions, _____. NaOH  B) Bronsted-Lowry Theory: 1) During a chemical reaction, any substance that donates a _______ is an acid and any substance accepting a proton is a _______.

6 a) conjugate_________: the substance formed after a base acquires a proton, ___. b) conjugate_________: the substance formed after an acid loses a proton, ___.

7 2) “Is it possible for a substance to be both an acid and a base (at different times of course)?” a) ___________: example is H 2 O.

8 C) Lewis Theory: 1) The focus is on the transfer of electrons! a) ______: electron pair donor. b) ______: electron pair acceptor.

9 II) Naming Acids: A) ______Acids: acids containing only two elements. B) _________Acids: (also known as oxyacids) acids containing three elements.

10 1) The most common form of the 3 element combination is given an “ic” ending. 2) If a second acid is formed using the same 3 elements, but with fewer oxygens, the acid is given an “ous” ending.

11 3) If a third acid is formed using the same 3 elements, but with more oxygens, the acid is given a “per” prefix and an “ic” suffix.

12 III) Naming Bases: * Most bases are composed of a metal cation and a hydroxide anion. They are named by adding the word “hydroxide” to the name of the metal ion.

13 IV) Strong vs. Weak Acids and Bases: A) Acids: 1) Strong acids ionize completely! 2) Weak acids ionize partially!

14 3) ____________ Acids: any acids containing more than one ionizable hydrogen. B) Bases: 1) Strong and weak bases are defined the same as acids, but with the hydroxide ion.

15 V) Neutralization Reactions: A) ___: percent hydronium ion. 1) pH: a measure of the hydronium ion [ _____ ] concentration in a solution. 2) pH Scale:

16 B) _______: a crystalline compound made from the (-) ion of an acid and the (+) ion of the base. 1) _________________ Reaction: the reaction of an acid with a base to form salt and water.

17 *neutralization occurs when the product of the MOLARITY (concentration: how strong) and VOLUME for both the acid and base are equal; or in other words, when the moles of acid equal the moles of base.

18 C) TITRATION!!!!! 1) Titration: A method for determining the molarity (concentration) of a solution (acid or base) by reacting it with another solution (acid or base) of known molarity until the reaction neutralizes.

19 2) Example Problem: What is the molarity of NaOH if it took 15 mL of the NaOH to neutralize 25 mL of 0.30 M acetic acid?