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Acids and Bases

This guide offers a comprehensive overview of acids and bases, including their definitions, properties, and examples. Acids produce hydrogen ions (H+) in solution and have a sour taste, while bases produce hydroxide ions (OH-) and are bitter. Both are good electrolytes. The document also explains how to name acids, including binary acids and oxyacids, and provides insight into neutralization reactions, where acids and bases react to form water and salt, resulting in a neutral solution.

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Acids and Bases

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  1. Acids and Bases And neutralization reactions

  2. Acids and Bases • An acid is a substance that produces hydrogen ions in solution. HCl  H+ + Cl- • A base is a substance that produces hydroxide ions in solution. NaOH  Na+ + OH-

  3. Acids • Substances that releasehydrogen ions (H+) when mixed in water • Physical Properties: • Sour tasting • Wetto the touch when in solution • Water soluble • Good conductors of electricity, therefore electrolytes

  4. Acids • Chemical Properties • React with metals to produce hydrogen gas • Corrosive • Make chemical indicators change colour • React with bases to produce a neutral solution

  5. Acids • Examples:

  6. Bases • Substances that release hydroxide ions (OH-) when mixed in water. Also called alkaline • Physical Properties: • Bitter tasting • Slippery to the touch when in solution • Water soluble • Good conductors of electricity, therefore electrolytes

  7. Bases • Chemical Properties • Corrosive • Make chemical indicators change colour • React with acids to produce a neutral solution

  8. Bases • Examples:

  9. Chemical Indicators • Are solutions that change colour in acids and in bases • Can be either • natural or • synthetic

  10. Chemical Indicators • Litmus paper: • Base turns it Blue! • Acid turns it Red! Universal Indicator is a mixture of chemicals that changes colour through a wide range of pH values

  11. The pH scale • A numerical scale used to show how acidic or basic a solution is • pH stands for “power of hydrogen”

  12. The pH scale • pH is a logarithmic scale which means that every unit on the scale represents a tenfold (10X) effect on the concentration of the solution

  13. The pH scale: Logarithmic • This means that pH 3 is 10 times more acidic than ph 4. • If the value changes by more than one number you must multiply • ex. From pH 5 to pH 8 = 10 x 10 x 10 (3 steps = 10 multiplied by itself 3 times)

  14. Naming Acids • A binary acid forms when an H+ bonds with a non-metal • HF (aq), HCl (aq), HBr (aq), HI (aq), H2S (aq), and H3P (aq) are some common binary acids • To name them, use the following structure: • “hydro + ______ ic acid”

  15. Naming Acids • An oxyacid has a non-metal and an oxygen component • H3PO4, HClO3, HIO3, H2SO4, HBrO3, H2CO3, and HNO3 are some common oxyacids • To name them: • “_____________ ic acid”

  16. Naming Bases • Name the metal • Name the polyatomic (i.e. hydroxide) • Example • Mg(OH)2 • magnesium hydroxide

  17. Neutralization Reactions • A type of double displacement reaction • Acid + Base Water + Salt • A salt is an ionic compound. The pH of the products is around 7 (neutral) Example hydrochloric acid + sodium hydroxide  water + sodium chloride

  18. Practise!! • Try the practise questions on your worksheet!

  19. Naming Acids and Their Ions • There are two main kinds of acids: binary acids and oxoacids. • A binary acid is composed of two elements: hydrogen and a non metal. The general formula for a binary acid is HX, where X is the non-metal. (HBr and HCl are two examples).

  20. To name a binary acid • Attach the prefix hydro • Use the non-metal name as the root • Attach the suffic “ic” • Add the word acid

  21. HF • Hydrofluric acid • HCl • Hydrochloric acid • HBr • Hydrobromic acid • HI • Hydroiodic acid • H2S • Hydrosulfuric acid

  22. An oxoacid (oxyacid) is an acid formed from a polyatomic ion that contains oxygen, hydrogen, and another element. • For anions that end in “ate”, change the ending to “ic” and add the word acid • ClO3- is chlorate • HClO3- is called chloric acid

  23. For anions that end in “ite”, change the ending to “ous” and add the word acid. • ClO2- is chlorite • HClO2- is chlorous acid

  24. The prefixes hypo and per remain as part of the acid name. • ClO4- is perchlorate • HClO4- is perchloric acid

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