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Acid and Bases

Acid and Bases. Acid and Bases. Some Properties of Acids. Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) Taste sour Corrode metals Electrolytes: release ions in solution

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Acid and Bases

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  1. Acid and Bases

  2. Acid and Bases

  3. Some Properties of Acids • Produce H+ (as H3O+) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) • Taste sour • Corrode metals • Electrolytes: release ions in solution • Neutralize with bases to form a salt and water • pH is less than 7 • Turns blue litmus paper to red

  4. Some Properties of Bases • Produce OH-(Hydroxide Ions) ions in water • Taste bitter, chalky • Are electrolytes • Feel slippery(forms soap w/ skin oils) • Neutralize with acids to form salts and water • pH is greater than 7 • Turns red litmus paper to blue

  5. Some Common Acids & Bases HCl Hydrochloric Acid Stomach acid HNO3 Nitric Acid Jewelry making H2SO4 Sulfuric Acid Paper making H3PO4 Phosphoric Acid Preservative in Coca-Cola CH3COOH Acetic Acid Vinegar NaOH Sodium hydroxide lye KOH Potassium hydroxide liquid soap Ba(OH)2 Barium hydroxide stabilizer for plastics Mg(OH)2 Magnesium hydroxide “MOM” Milk of magnesia Al(OH)3 Aluminum hydroxide Maalox (antacid)

  6. Acid/Base definitions • Definition #1: Arrhenius (traditional) Acids – produce H+ ions (or Hydronium ions H3O+) Bases – produce OH- (Hydroxide) ions (problem: some bases don’t have hydroxide ions!)

  7. Arrhenius acid is a substance that produces H+ (H3O+) in water Arrhenius base is a substance that produces OH- in water

  8. Acid/Base Definitions • Definition #2: Brønsted – Lowry Acids – proton donor Bases – proton acceptor A “proton” is really just a hydrogen atom that has lost it’s electron!

  9. A Brønsted-Lowryacidis a proton donor A Brønsted-Lowrybaseis a proton acceptor conjugatebase conjugateacid base acid

  10. ACID-BASE THEORIES The Brønsted definition means NH3 is aBASEin water — and water is itself anACID

  11. Conjugate Pairs

  12. Acids & Base Definitions Definition #3 – Lewis Lewis acid - a substance that accepts an electron pair Lewis base - a substance that donates an electron pair

  13. Lewis Acids & Bases Formation ofhydronium ion is also an excellent example. • Electron pair of the new O-H bond originates on the Lewis base.

  14. The pH scale is a way of expressing the strength of acids and bases. Instead of using very small numbers, we just use pH

  15. Calculating the pH pH = - log [H+] Example: If [H+] =1E-10pH = - log( 1E-10) pH = - (- 10) pH = 10 Example: If [H+] = 1.8E-5pH = - log 1.8E-5 pH = - (- 4.74) pH = 4.74

  16. Try These! Find the pH of these: • A 0.15 M solution of Hydrochloric acid (answer: .8239) 2) A 3.00 X 10-7 M solution of Nitric acid (answer: 6.5229)

  17. pH calculations – Solving for H+ If the pH of Coke is 3.12, [H+] = ??? Because pH = - log [H+] then - pH = log [H+] Take antilog (10x) of both sides and get 10-pH =[H+] [H+] = 10-3.12 = 7.6 x 10-4 M *** to find antilog on your calculator, look for “Shift” or “2nd function” and then the log button

  18. pH calculations – Solving for H+ • A solution has a pH of 8.5. What is the Molarity of hydrogen ions in the solution? pH = - log [H+] 8.5 = - log [H+] -8.5 = log [H+] Antilog -8.5 = antilog (log [H+]) 10-8.5 = [H+] 3.16E-9 = [H+]

  19. pOH • Since acids and bases are opposites, pH and pOH are opposites! • pOH does not really exist, but it is useful for changing bases to pH. • pOH looks at the perspective of a base pOH = - log [OH-] Since pH and pOH are on opposite ends, pH + pOH = 14

  20. More About Water H2O can function as both an ACID and a BASE. In pure water there can beAUTOIONIZATION H2O  H30+ + OH- Equilibrium constant for water = Kw Kw = [H3O+] [OH-] =1.00 x 10-14at 25 oC

  21. More About Water Autoionization Kw = [H3O+] [OH-] = 1.00 x 10-14 at 25 oC In a neutral solution [H3O+] = [OH-] so Kw = [H3O+]2 = [OH-]2 and so [H3O+] = [OH-] = 1.00 x 10-7 M

  22. Kw: the Constant of Water or How to find the missing # Kw = [H+1][OH-1] = 1E-14 Used to find unknown [H+1] or [OH-1] if the other is known or given If [H+1] = .0003M, find the [OH-1] 1E-14 = [.0003M] [OH-1] [OH-1]=3.33E-11M

  23. The OH- ion concentration of a blood sample is 2.5 x 10-7 M. What is the pH of the blood? (answer: 7.3979) The pH of rainwater collected in a certain region of the northeastern United States on a particular day was 4.82. What is the H+ ion concentration of the rainwater? (answer: 1.51E-5M)

  24. [OH-] 1.0 x 10-14 [OH-] 10-pOH 1.0 x 10-14 [H+] -Log[OH-] [H+] pOH 10-pH 14 - pOH -Log[H+] 14 - pH pH

  25. Calculating [H3O+], pH, [OH-], and pOH Problem 1: A chemist dilutes concentrated hydrochloric acid to make two solutions: (a) 3.0 M and (b) 0.0024 M. Calculate the [H3O+], pH, [OH-], and pOH of the two solutions at 25°C. Problem 2: What is the [H3O+], [OH-], and pOH of a solution with pH = 3.67? Is this an acid, base, or neutral? Problem 3: Problem #2 with pH = 8.05?

  26. Strong and Weak Acids/Bases The strength of an acid (or base) is determined by the amount of IONIZATION. STRONG=100% IONIZED HNO3, HCl, H2SO4 and HClO4 are among the only strong acids.

  27. Weak Acids/Bases • Weak acids are much less than 100% ionized in water. One of the best known is acetic acid = CH3COOH

  28. CaO Strong Bases • Strong Base:100% dissociated in water. NaOH (aq) ---> Na+ (aq) + OH- (aq) Other common strong bases include KOH andCa(OH)2. CaO (lime) + H2O --> Ca(OH)2 (slaked lime)

  29. Weak Bases • Weak base:less than 100% ionized in water One of the best known weak bases is ammonia NH3 (aq) + H2O (l) NH4+ (aq) + OH- (aq)

  30. HONORS ONLY! Ionization Constants for Acids/Bases Conjugate Bases Acids Increase strength Increase strength

  31. HONORS ONLY! Equilibrium Constants for Weak Acids Weak acid has Ka < 1 Leads to small [H3O+] and a pH of 2 - 7

  32. EquilibriaInvolving Weak Acids and Bases HONORS ONLY! Consider Acetic Acid(weak), HC2H3O2 (HOAc) Diss. Eq: HC2H3O2+ H2O H3O+ + C2H3O2- Equilibrium Expression: (K is designated Ka for ACID) K gives the ratio of ions (split up) to molecules (don’t split up)

  33. HONORS ONLY! Equilibria Involving A Weak Acid You have 1.00 M HOAc. Calc. the equilibrium concs. of HOAc, H3O+, OAc-, and the pH. Step 1: Diss. Eq: HC2H3O2+ H2O H3O++ C2H3O2- Step 2.Write Ka expression This is a quadratic. Solve using quadratic formula. or you can make an approximation if x is very small! (Rule of thumb: 10-5 or smaller is ok)

  34. HONORS ONLY! Equilibria Involving A Weak Acid You have 1.00 M HOAc. Calc. the equilibrium concs. of HOAc, H3O+, OAc-, and the pH. Step 3.Solve Ka expression First assume: X<<<1.00 because Ka is so small. Now we can more easily solve this approximate expression without Quadratic Equation.

  35. HONORS ONLY! Equilibria Involving A Weak Acid You have 1.00 M HOAc. Calc. the equilibrium concs. of HOAc, H3O+, OAc-, and the pH. Step 4.Solve Kaapproximateexpression x =[H3O+] = [OAc-] = 4.2 x 10-3 M pH = - log [H3O+] = -log (4.2 x 10-3) =2.37 [HOAc] = 1.00 – X = 1.00 - 4.2E-3M = .9958M

  36. HONORS ONLY! Equilibria Involving A Weak Acid Calculate the pH of a 0.0010 M solution of formic acid, HCO2H. HCO2H + H2O  H3O+ +HCO2- Ka = 1.8 x 10-4 Approximate solution [H3O+] = 4.2 x 10-4 M,pH = 3.37 Exact Solution [H3O+] = [HCO2-] = 3.4 x 10-4 M [HCO2H] = 0.0010 - 3.4 x 10-4 = 0.0007 M pH = 3.47

  37. pH meter • Tests the voltage of the electrolyte • Converts the voltage to pH • Very cheap, accurate • Must be calibrated with a buffer solution

  38. pH indicators • Indicators are dyes that will change color in the presence of an acid or base. • Indicators only work in a specific range of pH • Some dyes are natural, like radish skin or red cabbage • Phenolphthalein turns at pH 7.00

  39. Setup for Titrating an acid with a base

  40. Titration • Add solution of [known] from the buret with [unknown] in the flask. • Reagent (base) reacts with compound (acid) in solution in the flask. • Indicator shows when exact stoichiometric reaction has occurred. (moles Acid = moles Base) • This is called END POINT where NEUTRALIZATION has occurred (Acid=Base). The color turns pink if Phenolphthalein is the indicator used. Titration Math(short version) M1• V1 = M2 • V2

  41. Typical Titration is done in 3 Steps • Remember to add 4 drops Phenolphthalein to each sample • Step 1: Approximate Run. Use a stock base and a 25 ml sample of the acid to get an idea of the [ACID]. Calculate approximate concentration of the acid. If needed, make a newbasewith a concentrationthesameastheacid. • Step 2: Using the new base, titrate a second 25ml sample of the acid trying to get within 1ml of accuracy. 25ml of acid should require about 25ml of base if they are close in concentration. • Step 3: Pin Point Run. Titrate a third 25ml sample of acid with the base that you made and try to get within 1 drop accuracy. • Report results to the Instructor.

  42. New Base Needed? How to make Base.

  43. Titration using a pH Meter • Set up the buret and the chemicals the same except no Phenolphthalein is added • Set up the Nova with a pH sensor attached and insert the probe into the Unknown solution. Proceed with the addition of the base solution until the graph looks like the one attached • The volume where the large jump takes place is the End Point, moles Base=moles Acid • Begin calculations

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