chapter 6 (cic) and chapter 16 (ctcs)
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Chapter 6 (CIC) and Chapter 16 (CTCS). Read in CTCS Chapter 16.4-7 Problems in CTCS: 16.23, 25, 27, 31, 33, 35, 37, 41, 45, 57, 49, 51, 59, 61, 63, 65. pH – Power of Hydrogen. As [H + ] increases, the pH decreases Based on logarithmic scale - PowerPoint PPT PresentationTRANSCRIPT
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Chapter 6 (CIC) and Chapter 16 (CTCS)Read in CTCS Chapter 16.4-7Problems in CTCS: 16.23, 25, 27, 31, 33, 35, 37, 41, 45, 57, 49, 51, 59, 61, 63, 65
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pH Power of HydrogenAs [H+] increases, the pH decreasesBased on logarithmic scaleCompared to a pH = 1 solution, a pH = 2 solution is 10x less acidicAn acid has a pH < 7A base has a pH > 7
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pH of Some Common SolutionsBrown, T.L.; LeMay, H.E.Jr.; and Bursten, B.E. Chemistry the Central Science, 8th Edition, Prentice Hall, Upper Saddle River, NJ, 2000, p 602.
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Why Do We Bother With pH?[H+] = 3.4 x 10-6 is too smallp stands for log and H stands for [H+] pH = -log [H+]Neutral solution has [H+] = 1 x 10-7 or pH = 7.0Q: If [H+] = 3.4 x 10-6, what is the pH? How many sig figs should there be?
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Q: What is the [OH-] of this solution? What is the pOH?
Notice that pH + pOH = 14.00 (pKw)Derived from [H+] [OH-] = 1 x 10-14 (Kw)
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Strong Acids/BasesTable 4.2 lists these as:
Note that the strong bases are all of the soluble hydroxides
Strong AcidsHClHBrHIHClO4HNO3H2SO4Strong BasesLiOHNaOHKOHRbOHCsOHSr(OH)2Ba(OH)2
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Whats the definition of a strong acid or base?
Q: What is the pH of 0.008 M HCl?
Q: The pH of the HCl soln in lab was about 1.85. What was its concentration?
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Q: What is the [OH-] in 0.010 M Sr(OH)2?
Q: What is the pH of this solution?
Q: What is the pH of a saturated Ca(OH)2 solution if the solubility is 0.97 g/100. mL?
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Weak AcidsNot to be confused with dilute acids!0.0001 M HCl is NOT a weak acid!HClO + H2O H3O+ + ClO-Remember that K = [products]/[reactants]
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If [HClO] = 1.0 M, then
[H3O+][ClO-] = 3.0 x 10-8
So, since there should be equal amounts of [H3O+] and [ClO-], then
[H3O+]2 = 3.0 x 10-8
Or [H3O+] = 1.7 x 10-4
And pH = 3.76
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Things to RememberA Ka must have H+ in the productsKas of strong acids have large values (greater than 1)A Kb must have OH- in the productsKbs of strong bases have large values (greater than 1)You may not be able to simplify the problem so much and you will have to make approximations
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Q:Calculate the pH of a 0.025 M lactic acid solution if its Ka = 1.4 x 10-4.
A: 2.75
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Q:Calculate the Ka of a 0.085 M phenylacetic acid solution if its pH is 2.68.
A: 5.3 x 10-5
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Q:Calculate the pH of a 1.0 M methylamine solution if its Kb = 4.38 x 10-4.
A: 12.32