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HOMEWORK – DUE THURSDAY 12/10/15 HOMEWORK – DUE THURSDAY 12/10/15 HW-BW 18 CH 18 #’s 9-18...
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Transcript of HOMEWORK – DUE THURSDAY 12/10/15 HOMEWORK – DUE THURSDAY 12/10/15 HW-BW 18 CH 18 #’s 9-18...
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HOMEWORK – DUE THURSDAY 12/10/15 HW-BW 18 CH 18 #’s 9-18 (all), 21, 23-30 (all), 41-52 (all)
NO EXTRA CREDIT FOR CHAPTER 18 HW
Lab Wednesday/Thursday – Locker check-out and questions about the final
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Sig., Figs., and Logs When you take the log of a number written in scientific
notation, the digits before the decimal point come from the exponent, and the digits after the decimal point come from the decimal part of the number.
Because the part of the scientific notation number that determines the significant figures is the decimal part, the sig. figs. are the digits after the decimal point in the log.
6log(2.0 10 ) 62.0l g( )10o 6= log(10 )6= log( ) + log10 (2.0)
= 66 = + 0.30 30300.303= 030 6 6 + = . 303030
6log( )2.0 = 010 6.3
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pKWhat does “p” mean?
p___ = -log___ (pH = - log H+, pOH = -logOH-)A way of expressing the strength of an acid or base
is pK.pKa = −log(Ka), Ka = 10−pKa
pKb = −log(Kb), Kb = 10−pKb
The stronger the acid, the smaller the pKa.Larger Ka = smaller pKa
The stronger the base, the smaller the pKb.Larger Kb = smaller pKb
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Finding pH of a Strong Acid or Strong Base Solution
For a monoprotic strong acid [H+] = [HA].
For 0.10 M HCl, [H+] = 0.10 M and pH = 1.00
For 0.025 M HNO3, [H+] = 0.025 M and pH = 1.60
For a strong ionic base, [OH−] = (number OH−) × [Base].
For 0.15 M Ca(OH)2, [OH−] = 0.30 M and pH = 13.48
For 0.15 M KOH, [OH−] = 0.15 M and pH = 13.18
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pH of an Acid/Base Mixture
17.20 mL of a 0.09000 M barium hydroxide solution is added to 25.00 mL of 0.1234 M hydrochloric acid.1) What are the pH and pOH of the original barium hydroxide?2) What is the pH of the original hydrochloric acid solution?3) What is the pH of the solution after the two solutions are mixed?
pOH Ba(OH)2(aq) = – log(0.18000) = 0.74473
pH Ba(OH)2(aq) = 14 – 0.74473 = 13.25527
pH HCl(aq) = – log(0.1234) = 0.9087
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pH of an Acid/Base Mixture
17.20 mL of a 0.09000 M barium hydroxide solution is added to 25.00 mL of 0.1234 M hydrochloric acid.1) What are the pH and pOH of the original barium hydroxide?2) What is the pH of the original hydrochloric acid solution?3) What is the pH of the solution after the two solutions are mixed?
+(aq)
0.1234 1mol H 0.02500 0.003085
1 1
+(aq) (aq) +
(aq) (aq)(aq) (aq)
HCl H HCl H
HCl HCl
mol molL mol
L mol
(aq)
0.09000 2mol OH 0.01720 0.003096
1 1
2(aq) (aq)
2(aq) (aq)2(aq) 2(aq)
Ba(OH) OH Ba(OH) OH
Ba(OH) Ba(OH)
mol molL mol
L mol
0.003096 0.003085 0.000011 +(aq) (aq) (aq) OH H OH excess mol mol mol
40.000011 2.607 10
0.02500 0.01720
(aq) OH excess
OH L L
molM
pOH = – log(2.607x10–4) = 3.5839
pH = 14 – 3.583920 = 10.4161
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Strong Bases
• The stronger the base, the more willing it is to accept H+.
• For ionic bases, practically all units are dissociated into OH– or accept H+.Strong electrolyteMulti-OH strong bases completely
dissociated
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Weak Bases
• In weak bases, only a small fraction of molecules accept H+.Weak electrolyteMost of the weak base molecules do
not take H from water.Much less than 1% ionization
in water
• [HO–] << [weak base]• Finding the pH of a weak base
solution is similar to finding the pH of a weak acid.
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TitrationIn an acid–base titration, a solution of known
concentration from a burette (titrant) is slowly added to a solution of unknown concentration (analyte) until the reaction is complete. When the reaction is complete we have reached the endpoint of the
titration.An indicator may be added to determine the
endpoint.When the moles of H+ = moles of OH−, the titration
has reached its equivalence point.
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Titration
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Titration Curve A plot of pH versus the amount of added titrant. Prior to the equivalence point, the known solution in the
flask is in excess, so the pH is closest to its pH.
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Titration Curve A plot of pH versus the amount of added titrant. The inflection point of the curve is the equivalence
point of the titration.
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Titration Curve A plot of pH versus the amount of added titrant. The inflection point of the curve is the equivalence
point of the titration. The pH of the equivalence point depends on the pH of
the salt solution. Equivalence point of neutral salt, pH = 7 Equivalence point of acidic salt, pH < 7 Equivalence point of basic salt, pH > 7
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Titration Curve A plot of pH versus the amount of added titrant. Beyond the equivalence point, the unknown solution in
the burette is in excess, so the pH approaches its pH.
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Titration of a Weak Acid with a Strong Base Titrating a weak acid with a strong base results in
differences in the titration curve at the equivalence point and excess acid region.
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Titration of a Weak Acid with a Strong Base Titrating a weak acid with a strong base results in
differences in the titration curve at the equivalence point and excess acid region.
The initial pH is determined using the Ka of the weak acid.
The pH in the excess acid region is determined as you would determine the pH of a buffer.
The pH at the equivalence point is determined using the Kb of the conjugate base of the weak acid.
The pH after equivalence is dominated by the excess strong base. The basicity from the conjugate base anion is negligible.
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Titration of a Polyprotic AcidIf Ka1 >> Ka2, there will be two equivalence points
in the titration.
Titration of 25.0 mL of 0.100 M H2SO3 with 0.100 M NaOH
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Titration of a Polyprotic AcidIf Ka1 >> Ka2, there will be two equivalence points
in the titration.
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Titration of a Polyprotic AcidIf Ka1 >> Ka2, there will be two equivalence points
in the titration.The closer the Ka’s are to each other, the less
distinguishable the equivalence points are.