1. Chapter 25 Acids, Bases, and Salts
Section 1-Acids and Bases

2. An acid is a substance that produces hydrogen ions in a water solution.
The ability to produce ions is what gives their characteristic properties.
When an acid dissolves in water, H⁺ ions interact with water molecules to form H₃0⁺ ions, which are called hydronium ions.
Properties of Acids

3. Common Acids Citric Acid is found in citrus fruits.
Lactic Acid is found in yogurt and buttermilk.
Vinegar is also known as acetic acid.
Your stomach uses hydrochloric acid to help you digest your food.
Common Acids

4. Common Acids Name, Formula Use Other Information Acetic Acid
Food Prep and Preservation
When in solution with water it is known as vinegar
Acetylsalicyclic Acid
Pain Reliever, Fever reducer
Known as aspirin
Ascorbic Acid
Antioxidant, Vitamin
Called Vitamin C
Carbonic Acid
Carbonated Drinks
Involved in cave, stalactite, and stalagmite formation and acid rain
Hydrochloric Acid
Digestion as gastric juice
Commonly called Mariatic Acid
Phosphoric Acid
Makes detergents, fertilizers, and soft drinks
Sour but pleasant taste, detergents containing phosphates polute water
Sulfuric Acid
Car batteries, fertilizers
Dehydrating agent, causes burns by removing water from cells
Nitric Acid
Makes fertilizers
Colorless, but yellow when exposed to light
Common Acids

5. A substance that forms hydroxide ions, OH⁻, in a water solution is a base.
A base is also any solution that accepts H⁺ from acids.
Think of bases as the opposite of acids.
Properties of Bases

6. In pure and undissolved state many bases are crystalline solids.
In a solution bases feel slippery and have a bitter taste.
Strong bases are like strong acids as they are corrosive and can burn the skin.
Properties of Bases

7. Common Bases Name, Formula Use Other information Aluminum Hydroxide
Color-fast fabrics, antacid, water purification
Sticky gel that collects clay ad dirt particles on surface
Calcium Hydroxide
Leather-making, mortar and plaster, lessen acidity of soil
Called caustic lime
Magnesium Hydroxide
Laxative, antacid
Called milk of magnesia
Sodium Hydroxide
To make soap, oven cleaner, drain cleaner, textiles, and paper
Called lye and caustic soda; generates heat when combined with water, reacts with metals to form hydrogen
Ammonia
Cleaners, fertilizer, to make rayon and nylon
Irritating odor that is damaging to nasal passages and lungs
Common Bases

8. Acids & Bases Ammonia is a popular household cleaner.
Never combine products containing ammonia with other cleaners that contain chlorine such as toilet bowl cleaners and bleach. The reaction produces poisonous gases.
Solutions of both acids and based produce some ions that are capable of carrying electric current to some extent. They are considered to be conductors.
Acids & Bases

9. Chapter 25 Acids, Bases, and Salts
Section 2- Strengths of Acids and Bases

10. Strong Acids and Weak Bases
The strength of an acid or base depends on how completely a compound separates into ions when dissolved in water.
An Acid that ionizes almost completely in solution is a Strong Acid. ex. Hydrochloric Acid
A weak acid is an acid that only partly ionizes in a solution. Ex. Acetic and Carbonic Acids
Strong Acids and Weak Bases

11. The pH of a solution is a measure of the concentration of H⁺ ions in it.
The greater the H⁺ concentration is, the lower the pH is and the more acidic the solution is.
The pH measures how acid or basic a solution is. pH

12. To indicate pH, a scale ranging from 0 to 14 has been devised.

13. pH Solutions with a pH lower than 7 are described as acidic.
Solutions with a pH greater than 7 are described as basic.
A pH of exactly 7 indicates that the concentration of H⁺ ions and OH⁻ ions are equal. These solutions are neutral. Ex. Pure water at 25 degrees has a pH of 7. pH

14. One way to determine pH is by using pH indicator strips
One way to determine pH is by using pH indicator strips. The final color of the pH paper is matched with colors on a chart to find the pH. pH

15. The blood that circulates through your body has a pH of between 7
The blood that circulates through your body has a pH of between 7.0 and 7.8
Your body can not work outside of this pH range.
Does your Blood pH change when you eat spicy/acidic foods?
Blood pH

16. You would think that your pH in your blood changes when you eat spicy/acidic foods but it does not.
Your blood contains compounds called Buffers that enable small amounts of acids or bases to absorbed.
Buffers are solution containing ions that react with additional acids or bases to minimize their effects on pH.
Blood pH

17. Chapter 25 Acids, Bases, and Salts
Section 3-Salts

18. Neutralization is a chemical reaction between an acid and a base that takes place in a water solution.
Antacid Tablets are an example of a product that a person suffering from indigestion cant take to “neutralize” the effects of acid reflux.
Neutralization

19. A salt is a compound formed when the negative ions from an acid combine with the positive ions from a base.
Name
Common Name
Uses
Sodium Chloride
Salt
Food Prep
Sodium Hydrogen Carbonate
Sodium bicarbonate baking soda
Food Prep and antacids
Calcium Carbonate
Calcite, Chalk
Making paint and tires
Potassium Nitrate
Saltpeter
Fertilizers
Potassium Carbonte
Potash
Making soap and glass
Sodium Phosphate
TSP
Detergents
Ammonium Chloride
Sal ammoniac
Dry-Cell Batteries

20. If you need to know the concentration of an acid or base in a solution you can determine it through a process called titration.
Titration