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Just view Basic Concepts

Just view Basic Concepts. No note taking here. You can view PPT again online if needed before test. Everyday stuff. Household cleaners are acidic or basic. Everyday uses. Foods and medicines are acidic or basic. pH Indicators. U sed to test pH of soil and swimming pools.

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Just view Basic Concepts

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  1. Just view Basic Concepts No note taking here. You can view PPT again online if needed before test.

  2. Everyday stuff • Household cleaners are acidic or basic.

  3. Everyday uses • Foods and medicines are acidic or basic.

  4. pH Indicators • Used to test pH of soil and swimming pools.

  5. Common Indicators • Red cabbage juice and grape juice can be used as a pH indicator.

  6. pH of soil • Some plants may change flower color due to the pH of the soil.

  7. Basic Concepts – Environmental effects • Acid rain can have economic and aesthetic effects on lakes and structures.

  8. Vocabulary 8.3/8.4 You should know these terms for these sections. Be sure to define these words in your notes for homework. See page 240 and 246. • acid • base • neutralization • pH

  9. Acids

  10. What juices might contain acid? Orange juice Tomato juice Lemon juice

  11. Acid in your body?

  12. Hydronium ions • Hydronium ion is a water molecule with an extra hydrogen ion attached to it. H2O + H+ ---> H3O+ • It usually used to determine the acidity of a chemical compound.

  13. How H3O+ is made • When a compound is put into water solution, the more the hydronium ion is produced , the higher the acidity is. HCl + H2O ----> Cl- + H3O+ • The Hydrogen ion is transferred to water molecule.

  14. Common acids.

  15. What do they all contain?

  16. Did you know? • Acids taste sour • Are corrosive to metals • Change blue litmus paper red • Become less acidic when mixed with bases.

  17. Bases

  18. Hydroxide ions • A base is a compound that produces hydroxide ions (OH−) when dissolved in water. NaOH ---> Na+ + OH- • When sodium hydroxide dissolves in water, it dissociates into sodium ions and hydroxide ions.

  19. Common bases

  20. What do they all contain?

  21. Did you know? • Bases taste bitter • Feel slippery • Change red litmus paper blue • Become less basic when mixed with acids.

  22. Indicators

  23. Indicators • An indicator is any substance that changes color in the presence of an acid or base. • Common indicators are litmus, phenolphthalein and universal indicator. • Lab: Red Cabbage Juice

  24. Neutralization

  25. Neutralization • Negative ions in an acid combine with the positive ions in a base to produce an ionic compound called a salt. • At the same time, the hydronium ions from the acid combine with the hydroxide ions from the base to produce water. 

  26. Neutralization • The neutralization reaction of an acid with a base will always produce water and a salt, as shown below: AcidBaseWaterSalt HCl   +  NaOH   H2O   +  NaCl

  27. Think about this • What would happen if a hydrogen ion (H+) from an acid reacted with a hydroxide ion (OH-) from a base? 

  28. Water • What would happen if a hydrogen ion (H+) from an acid reacted with a hydroxide ion (OH-) from a base?  Water would be produced. 

  29. Neutralization reaction • If the ions (other than H+ and OH- ions) from the acid and the base are put back into the equation, it would read, showing that an acid reacts with a base to make water plus an ionic compound called a salt.  This acid-base reaction is called a neutralization reaction. 

  30. Neutralization • Another example: AcidBaseWaterSalt HBr   +  KOH   H2O   +  KBr

  31. Salts are made by reacting an acid with a base

  32. pH scale

  33. pH scale • Scale from 0 - 14 • Describes the concentration of hydronium ions (H3O+) in a solution. • The pH of a solution is a measure of its hydronium ion concentration. • A pH of 7 indicates a neutral solution. • Acids have a pH less than 7. • Bases have a pH greater than 7.

  34. Water = 7 • Water is neutral because it contains small but equal concentrations of hydronium ions (H3O+) and hydroxide ions (OH−) .

  35. If you add an acid to water… • The concentration of H3O+ increases and the concentration of OH− decreases. • Suppose you have a hydrochloric acid solution in which the concentration of H3O+ is 0.10 M (or 1.0 × 10−1 M). • The solution has a pH of 1.   • The lower the pH value, the greater the H3O+ ion concentration in solution is.

  36. If you add a base to water….. • The concentration of OH− increases and the concentration of H3O+ decreases. • Consider a sodium hydroxide solution in which the concentration of OH− is 0.10 M. The concentration of H3O+ in this solution is 1.0 × 10−13 M, which corresponds to a pH of 13.   • The higher the pH value, the lower the H3O+ ion concentration is.

  37. pH e End The End Get it?

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