Acids and Bases

1. Acids and Bases

2. ACIDS • Substance that produces Hydronium (H30)+ ion in solution. • Properties: tastes sour corrosive litmus turns red Common: citrus acid --found in juices Acids lactic acid – found in yogurt and buttermilk acetic acid – found in pickled foods hydrochloric acid – found in stomach used in industry

3. Common Acids

4. Bases • Any substance that produces a hydroxide ion (OH) - in solution. • Also—any substance that will accept a Hydrogen ion (H)+. • Properties: Many are crystalline solids feels slippery bitter taste turns litmus blue some are corrosive

5. Common Bases

6. Dissociation of Acids • When acids come into contact with water molecule attracts the hydrogen atom to form a hydronium ion (H3O)+. • Ex: When HCl dissolves in water, a H3O + ion and Cl- are produced. • hen hydrogen chloride dissolves in water, a hydronium ion and a chloride ion are produced.

7. Dissociation of Bases • When bases that contain –OH dissolve in water, the negative areas of nearby water molecules attract the positive ion in the base. • The positive areas of nearby water molecules attract the –OH of the base. • The base dissociates into a positive ion and a negative ion a hydroxide ion (OH). • n bases that contain –OH dissolve in water, the negative areas of nearby water molecules att (OH). • positive ion in the base.

8. Ammonia • Ammonia is a common household cleaner. • However, products containing ammonia never should be used with other cleaners that contain chlorine (sodium hypochlorite), such as some bathroom bowl cleaners and bleach. • Breathing these gases can severely damage lung tissues and cause death.

9. Ammonia • Ammonia is a base that does not contain –OH. • In a water solution dissociation takes place when the ammonia molecule attracts a hydrogen ion from a water molecule, forming an ammonium ion (NH4+). This leaves a hydroxide ion (OH-).

10. Strong and Weak Acids • The strength of an acid or base depends on how many acid or base particles dissociate into ions in water. • Strong Acids - nearly all acid molecules dissociate into ions good electrolyte Ex: • Weak Acids – small fraction of acid molecules dissociate into ions poor electrolyte Ex:

11. Strong and Weak Bases • Strong Bases dissociate completely in solution. Ex: • Weak Bases does not dissociate completely in solution. Ex:

12. pH of a Solution • 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 acidic or basic a solution is. • pH Scale: 0---7 Acidic H+ 7 Neutral H+ and OH- are equal 8-14 Base OH-

13. Ways to Indicate pH • Use Universal indicator 1) This paper undergoes a color change in the presence of H3O+ ions and OH‾ ions in solution 2) The final color of the pH paper is matched with colors in a chart to find the pH. • Use pH meter • This meter is operated by immersing the electrodes in the solution to be tested and reading the dial.

14. Blood pH • Blood pH range: 7.0 – 7. 8 • Enzymes cannot operate effectively outside this range. • Your blood contains compounds called buffers that enable small amounts of acids or bases to be absorbed without harmful effects. • Buffers are solutions containing ions that react with additional acids or bases to minimize their effects on pH.

15. Neutralization • Double Replacement Reaction • Occurs when Acids react with Bases Acid + Base = Salt + water Ex:

16. Salts • Essential for life---you lose salt to perspiration

17. Titration • Process in which a solution of known concentration (standard solution ) is used to determine the concentration of another solution. • The standard solution is carefully to a solution of unknown concentration to which an acid/base indicator has been added. • If the solution of unknown concentration is a acid, a standard basesolution is used. • If the solution of unknown concentration is a base, a standard acid solution is used.

18. Titration • To find the concentration of an acid solution, first, you would add a few drops of an indicator, such as phenolphthalein (fee nul THAY leen), to a carefully measured amount of the solution of unknown concentration. • Then, you would slowly and carefully add a base solution of known concentration to this acid-and-indicator mixture. • Toward the end of the titration you must add base drop by drop until one last drop of the base turns the solution pink and the color persists. • The point at which the color persists is known as the end point, the point at which the acid is completely neutralized by the base.

19. Other Indicators • Indicator – litmus which comes from lichens • Lichens – combination of fungus and cyanobacteria • Hydrangeas- Blue flowers with acidic soil Pink flowers with basic soil

20. Soaps and Detergents • Soaps are organic salts • Soaps contain a nonpolar organic chain of carbon atoms on one end and either a sodium or potassium salt of a carboxylic acid (karbahk SIHL ihk), –COOH, group at the other end. • Good Soaps contain 12-18 C atoms

21. Soap Scum • One problem with all soaps, however, is that the sodium and potassium ions can be replaced by ions of calcium, magnesium, and iron found in some water known as hard water. • When this happens, the salts formed are insoluble. • They precipitate out of solution in the form of soap scum.

22. Detergents • Similar to Soaps • Does not contain carboxyl group • Contains sulfonic group instead • Problems: 1) Some contain Phosphates—causes water pollution 2) Excess sulfonic acid—causes foaming of water

23. Esters • Made from alcohols • Contains OH- group • BUT they are not bases • Usage: Soaps (glycerine) Perfumes foods clothing

24. Polyesters • Synthetic fiber • Contain many esters=== polyesters • They are made from an organic acid that has two –COOH groups and an alcohol that has two –OH groups • Strong material because of the long chain that is close together