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Acids and Bases
HA H + + A - HCL H + + CL - CH 3 COOH H + + CH 3 COO -
0.003M HCl 9M HNO 3 7M CH 3 COOH ethanoic acid or acetic acid 5% ethanoic acid (vinegar) Use dilute or concentrated and weak or strong to describe the acids above.
2H 2 O H 3 O + + OH - [H + ] [OH - ] [H 2 O] H 2 O H + + OH - K c = K w = [H + ] [OH - ] = 10 -14
[H + ] for pure water is 1 X 10 -7 K w = [10 -7 ] [10 -7 ] = 10 -14 pH is -log [H + ] So the pH of pure water is 7
HA H + + A - H + + OH - H 2 O during titration Strong/weak acids cannot be differentiated by titration.
Mohr burette Remember to: Remove bubbles from the valve area Record data as you titrate including uncertainties What is the second burette for? Flush your burette with distilled water when finished
Acidic pH 0-8.2 Basic pH 8.2-12 Phenolphthalein
Strength of Acids and Alkalis By SK Chan. Why do acids/alkalis show different properties? Acid/AlkalipH value Electrical conductivity 0.1 M Ethanoic acid4Low.
Buffer Capacity Lab.
Daniel L. Reger Scott R. Goode David W. Ball Chapter 15 Solutions of Acids and Bases.
PH (potential of Hydrogen). According to the Bronsted-Lowry theory, both acids and bases are related to the concentration of hydrogen ions. Acids will.
PH. There is a formula to find pH pH = -log [H + ] or pH = -log [H 3 O + ] – (brackets around a substance means that substances concentration in molarity)
Ch.15: Acid-Base and pH Part 1.
Acids, Bases, and Salts Chapter 19.
Acids and Bases. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0
Strong Acids Strong acids fully dissociate so: They are fully separated into their ions They are good conductors of electricity Are not in a state of equilibrium.
ASİT. BAZ [H + ].[OH - ]=1x pH=-log[H + ] pOH=-log[OH - ] pH + pOH=14.
Raymond Chang 10th edition Chapter 16
Calculating pH of strong acids and bases. Strong acids or bases are those which dissociate completely. HCl(aq) + H 2 O(l) → H 3 O + (aq) + Cl - (aq) So.
1 Acetic acid, has a K a of 1.7 x Determine the pH of a 0.10 M solution of acetic acid. Hint: First write out the equilibrium expression of the.
Buffers and Titrations
Acidic, basic and neutral salts. Salts Salts are formed when acids react with bases. acid + base → salt + water When strong acids react with strong bases.
Ionic equilibrium Lec.9. Introduction Ionization: a process in which unionized molecules are changed into ions. Types of electrolytes: Strong electrolytesWeak.
Slide 1 of 45 Worked Examples Follow:. Slide 2 of 45.
Conjugate acids and bases. When a substance loses ONE hydrogen ion, the species produced is called a “conjugate base” What’s the conjugate base of H 2.
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