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SNC2P

SNC2P. Acids and Bases. Acids and Bases. And neutralization reactions. Acids. Substances that release hydrogen ions (H+) when mixed in water Physical Properties: Sour tasting Wet to the touch when in solution Water soluble Good conductors of electricity, therefore electrolytes.

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SNC2P

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  1. SNC2P Acids and Bases

  2. Acids and Bases And neutralization reactions

  3. Acids • Substances that release hydrogen ions (H+) when mixed in water • Physical Properties: • Sour tasting • Wet to 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!

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