<p> Acids, Bases, and Salts Chapter 19</p><p>I. Properties of Acids A. Acids give foods a tartar, . Example: vinegar (acetic acid), lemons (citric acid) B. Aqueous solutions of acids are . Electrolytes conduct electricity (car battery). There are strong and weak electrolytes. C. Acids cause certain chemical dyes called, to change color. Example: Litmus paper will turn red. D. Acids taste sour, will change the color of an acid-base indicator, and can be a strong or weak electrolyte. E. Some Common Acids 1. Hydrochloric acid (HCl) 2. Nitric acid (HNO3) 3. Sulfuric acid (H2SO4) 4. Phosphoric acid (H3PO4) 5. Acetic Acid (CH3COOH)</p><p>7. Carbonic acid (H2CO3)</p><p>II. Properties of Bases A. and hazardous. Exception: Stomach antacids (Milk of Magnesia) are bases used to treat excess stomach acid. B. . Example: Soap C. Aqueous solutions of bases are electrolytes and will cause an indicator to change color. D. Some Common Bases 1. Potassium hydroxide (KOH) 2. Sodium hydroxide (NaOH) 3. Calcium hydroxide Ca(OH)2 4. Magnesium hydroxide Mg(OH)2 III. Hydrogen Ions from Water. </p><p>A. Water molecules are highly and in constant motion. B. The collisions between water molecules are energetic enough to a hydrogen ion from one molecule to another. This is called . 1. Water molecule that a hydrogen ion becomes (-) charged and (OH-). 2. Water molecule that a hydrogen ion becomes (+) and + + (H3O ) or (H ). C. The self-ionization of water occurs to a extent. In chemically pure water, the number of H+ and OH- ions are . Certain chemical substances, when dissolved in water can change the amounts of H+ and OH- IV. Hydrogen Ions from Water A. -A substance that the amount of H+ (and decreases the amount of OH-) B. Base -A substance that the amount of OH- (and decreases the amount of H+ C. Neutral Substance- A substance that the amounts of H+ or OH- (so H+ remains to OH-) V. The pH Concept A. pH is a scale used to determine how a solution is.</p><p>B. pH scale goes from </p><p>C. pH = </p><p>D. pH than 7 = </p><p>E. pH than 7 = </p><p>F. pH 7 = </p><p>VI. Strong and Weak Acids and Bases A. Strong acids are in aqueous solution. + - HCl (aq) + H2O (l)  H3O (aq) + Cl B. Weak acids in aqueous solution. + - CH3COOH (aq) + H2O (l)  H3O (aq) + CH2COO</p><p>VII. Acid, Base Dissociation A. Every acid and base has a dissociation that tells you have much the acid or base separates into when dissolved in water. The . the constant the more the acid forms ions and the the acid. VIII. Salts in Solution. A. Salts form as a result of a reaction between an and a . B. Salts that produce acidic solutions contain ions that release , H+, to water. C. Salts that produce basic solutions contain ions that attract to water. IX. pH and pOH .</p><p>A. pH determines how acidic a solution is. A pH means you have a very solution. pH 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14</p><p>Acidic Basic pOH 14 13 12 11 10 9 8 7 6 5 4 3 2 1 0</p><p>B. pOH determines how acidic a solution is. A pOH means you have a very solution. C. pH + pOH = 14 D. Working with pH</p><p>1. What is the pH of a solution that has an [H+] = 0.1 M or 1 x 10-1M? pH = -log [H+] pH = 2. What is the pH of a solution that has an [H+] = 0.01 M or 1 x 10-2M? pH = </p><p>3. What is the pH of a solution that has an [H+] = 0.001 M or 1 x 10-3M? pH = </p><p>4. Which has a greater concentration of [H+]? [H+] = </p><p>5. What is the difference between pH = 1 and pH = 2 in terms of [H+]? A factor of </p><p>6. What is the difference between pH = 1 and pH = 3 in terms of [H+]? A factor of </p><p>7. What is the pOH if the pH = 2? pOH = </p><p>8. What is the pOH if the pH = 6? pOH = </p><p>9. What is the pH, pOH and is this acidic or basic if [H+] = 1 x 10-6 M? pH = , pOH = , </p>