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Chapter 9 Acids & Bases.

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Presentation on theme: "Chapter 9 Acids & Bases."— Presentation transcript:

1 Chapter 9 Acids & Bases


3 Acids donate protons to water to form hydronium ions taste sour
turn cabbage juice red turn litmus paper red neutralize bases

4 Bases donate hydroxide groups accept protons taste bitter feel slimy
turn cabbage juice yellow, green or blue depending upon the solution concentration turn litmus paper blue


6 Everyday Uses for Acids
digestion of food clean metals production of fertilizers making explosives carbonating beverages

7 What Makes a Compound an ACID?
When dissolved in water, all acids share certain physical & chemical properties sour taste color change (litmus paper to red, phenolphthalein turns colorless) corrode metals all contain hydrogen produce a positive hydrogen ion when dissolved in water (creates the hydronium ion H3O) known as proton donors

8 Three Common & Strong Acids
HCl – hydrochloric acid H2SO4 – sulfuric acid HNO3 – nitric acid strong acids ionize to a high decree in water many H+ ions strong acids are good electrolytes


10 What is an Electrolyte? a substance whose water solution conducts an electric current Strong acids conduct electricity very well because they produce many ions in water Weak acids do not conduct electricity as well

11 Everyday Uses for Bases
found in antacids (like Mylanta & Milk of Magnesia) to neutralize extra acids in the stomach used to make soaps (lye) used to make household cleaner (ammonium) found in deodorants

12 What Makes a Compound a BASE?
When dissolved in water, all bases share certain physical & chemical properties bitter taste color change (litmus paper to blue, phenolphthalein turns bright pink) slippery to the touch all contain hydroxide ion OH- known as proton acceptors

13 Three Common & Strong Bases
KOH – potassium hydroxide NaOH – sodium hydroxide Ca(OH)2 – calcium hydroxide strong bases readily dissolve in water to produce a high # of ions strong bases are good electrolytes (good conductors of electricity)


15 Acids & Bases in Solution
Solutions can be acidic, basic, or neutral the pH scale is used to determine the acidity of a solution the pH of a solution is a measure of the hydronium ion (H3O+) concentration

16 Higher Concentration of H+ (proton donors)

17 Equal Concentration of H+ and OH-

18 Higher Concentrationof OH- (proton acceptor)

19 pH the pH scale is a series of #s from 0 – 14 0 – 6 = acidic
7 = neutral (like distilled water) = basic strong acids have low pH numbers while strong bases have high pH numbers



22 pH of Common Items


24 Formation of Salts when acids react chemically with bases, they for a class of compounds called the salts a salt forms from the positive ion of a base & the negative ion from an acid this reaction, called neutralization, also produces water as a by-product H+Cl- + Na+OH- → H2O + NaCl What kind of reaction is neutralization?

25 Precipitates many of the salts created by the neutralization process do not dissolve in water they crystallize out of the solution to form a precipitate



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