Acids Bases They are everywhere In

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Acids & Bases They are everywhere. . In your food In your house EVEN IN YOU!!!!!

What is an acid? § An acid is a solution that has an excess of H+ ions. It comes from the Latin word acidus that means "sharp" or "sour". § The more H + ions, the more acidic the solution.

Properties of an Acid § § § Tastes Sour Conduct Electricity Corrosive, which means they break down certain substances. Many acids can corrode fabric, skin, and paper Some acids react strongly with metals Turns blue litmus paper red

Uses of Acids § Acetic Acid = Vinegar § Citric Acid = lemons, limes, & oranges. It is in many sour candies such as lemonhead & sour patch. § Ascorbic acid = Vitamin C which your body needs to function. § Sulfuric acid is used in the production of fertilizers, steel, paints, and plastics. § Car batteries

What is a base? § A base is a solution that has an excess of OHions. § Another word for base is alkali. § Bases are substances that can accept hydrogen ions

Properties of a Base Feel Slippery Taste Bitter Corrosive Can conduct electricity. (Think alkaline batteries. ) § Do not react with metals. § Turns red litmus paper blue. § §

Uses of Bases § Bases give soaps, ammonia, and many other cleaning products some of their useful properties. § The OH- ions interact strongly with certain substances, such as dirt and grease. § Chalk and oven cleaner are examples of familiar products that contain bases. § Your blood is a basic solution.

Let’s examine the behavior of an acid, HA, in aqueous solution. HA What happens to the HA molecules in solution?

100% dissociation of HA HA H+ Strong Acid A- Would the solution be conductive?

Partial dissociation of HA HA H+ Weak Acid A- Would the solution be conductive?

HA H+ + A- HA H+ A- Weak Acid At any one time, only a fraction of the molecules are dissociated.

Strong and Weak Acids/Bases Strong acids/bases – 100% dissociation into ions HCl HNO 3 H 2 SO 4 Na. OH KOH Weak acids/bases – partial dissociation, both ions and molecules CH 3 COOH NH 3

p. H Scale § p. H is a measure of how acidic or basic a solution is. • The p. H scale ranges from 0 to 14. § Acidic solutions have p. H values below 7 § A solution with a p. H of 0 is very acidic. § A solution with a p. H of 7 is neutral. • Pure water has a p. H of 7. • Basic solutions have p. H values above 7.

p. H Scale • A change of 1 p. H unit represents a tenfold change in the acidity of the solution. • For example, if one solution has a p. H of 1 and a second solution has a p. H of 2, the first solution is not twice as acidic as the second—it is ten times more acidic.

Acid – Base Reactions § A reaction between an acid and a base is called neutralization. An acid-base mixture is not as acidic or basic as the individual starting solutions.

Acid – Base reactions § Each salt listed in this table can be formed by the reaction between an acid and a base.

Bronsted-Lowry Model acid: anything that donates a [H+] (proton donor) base: anything that accepts a [H+] (proton acceptor) acid + base <=> acid + base HNO 2 + H 2 O <=> NO 2 - + H 3 O+ Each acid has a conjugate base and each base has a conjugate acid. These conjugate pairs only differ by a proton. In this example: HNO 2 is the acid, H 2 O is the base, NO 2 - is the conj. base, and H 3 O+ is the conj. acid. The Trick- Pick a compound on the left side of the equation. Find the similar compound on the other side of the reaction. The species with 1 more Hydrogen is the acid, the one with less is the base. HNO 2 <=> NO 2 So HNO 2 is the acid. or H 2 O <=> H 3 O+ So H 3 O+ is the acid.

Past Regents Questions According to one acid-base theory, water acts as an acid when an H 2 O molecule (1) accepts an H+ (3) accepts an H(2) donates an H+ (4) donates an HAn acid can be defined as an (1) H+ acceptor (3) OH- acceptor (2) H+ donor (4) OH- donor

AUTOIONIZATION of WATER Water is Amphiprotic H 2 O(l) + H 2 O(l) <==> H 3 O+(aq) + OH¯(aq)

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