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Vocabulary

Vocabulary. Hydronium = H 3 O + Proton = H+ or H 3 O + Hydroxide = OH- Amphoteric = a compound that can act as an acid or base. Alkaline = When a base completely disassociates in water to yield OH- ions.

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Vocabulary

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  1. Vocabulary • Hydronium = H3O+ • Proton = H+ or H3O+ • Hydroxide = OH- • Amphoteric = a compound that can act as an acid or base. • Alkaline = When a base completely disassociates in water to yield OH- ions.

  2. H2OHCl H+ + Cl- Acid is a proton donor (H+), which creates hydronium ions.H2ONaOH Na+ + OH-A base is a proton acceptor

  3. Acid • Bronsted-Lowry – H+ (proton) donor (doesn’t have to happen in an aqueous solution) • Ex., HCl + NH3NH4+ + Cl- • Arrhenius – produce H+ in aqueous solution • [H+] > [OH-]

  4. Base • Bronsted-Lowry – H+ (proton) acceptor • Arrhenius – produce hydroxide (OH-) in an aqueous solution • [H+] < [OH-]

  5. http://www.chem.utk.edu/yang/chap8.ppt

  6. Strong AcidsChloric Acid HClO3 Hydrobromic Acid HBr Hydrochloric Acid HCl Hydriodic Acid HI Nitric Acid HNO3 Perchloric Acid HClO4Sulfuric Acid H2SO4 Hydronium Ion H3O+

  7. Strong BasesCarbonate Ion CO2/3 - Phosphate Ion PO3/4-Hydroxide Ion OH- Amide Ion NH2- Hydride Ion H-

  8. http://www.chem.utk.edu/yang/chap8.ppt

  9. Conjugate acid – base pair • Conjugate acid-base pair: any pair of molecules or ions that can be interconverted by transfer of a proton http://www.chem.utk.edu/yang/chap8.ppt

  10. In the reaction of a Bronsted-Lowry acid, the molecule or ion that remains is the conjugate base.

  11. Neutralization Reactions • Occurs in an aqueous solution between a strong acid and a strong base. • When neutralization occurs, a salt and water are formed. • Ex., HCl + NaOH H2O + NaCl

  12. Lewis Acid- an atom, ion or molecule that accepts an electron pair to form a covalent bond. • Applies to any ion that can accept an electron pair. • H+ +2:NH3 [H-NH3]+ or [NH4]+ • A Lewis base is an atom or molecule that donates an electron pair to form a covalent bond.

  13. Net Ionic Equations • A net ionic equation includes only those compounds and ions that undergo a chemical change. • Write an overall ionic equation • All soluble compounds are shown as dissociated ions in solution, ppt are shown as solids. • Ex., ppt of cadmium sulfate Cd2+ (aq) + 2NO3- + 2NH4+(aq) SO42- CdSO4(s) + 2NO3-(aq) +2NH4+(aq)

  14. Net Ionic Equation • Cd2+(aq) + SO42-(aq) CdSO4(s)

  15. HCl + H2O H3O+ + Cl-(acid) (base) (conjugate acid) (conjugate base)

  16. Water can be both a acid and a baseH2O + H2O H3O+ + OH- The animation here shows the formation of H3+O ions and OH- ions in an aqueous system

  17. Kw = ion-product constant • Kw = in any aqueous solution @ 25 degrees Celcius the product of [H3O+][OH-] must always equal 1.0 X 10-14 [H +] = [OH-] = 1.0 * 10-7Kw = [H+] [OH-] = (1.0 *10-7)(1 *10 -7)Kw = 1.0 * 10-14

  18. Calculating pH and pOH Next let's look at values forpH and pOH. pOH is simply the power of hydroxide ion concentration and is figured the same way as pH but using the concentration of hydroxide ion instead.) Source: http://dl.clackamas.cc.or.us/ch105-05/calculat1.htm

  19. pH [H3O+] [OH-] pOH 7 1.0 x 10-7M 1.0 x 10-7M 7 Let's start by working with the concentrations that are 1.0 x 10(raised to some power). These pH and pOH values can be figured very simply. When [H3O+] is 10-7M, the pH is 7. Also the [OH-] is 10-7M and the pOH is 7. Note that the pH and pOH add up to 14.

  20. 65 pH 1.0 x 10-6M1.0 x 10-5M [H3O+] [OH-] 1.0 x 10-8M1.0 x 10-9M pOH 89 Now look at the acidic solutions. When the [H3O+] is 10-6M, the pH is 6. Also, the [OH-] is 10-8M and the pOH is 8. Again, the pH and the pOH add up to 14. When the [H3O+] is 10-5M, pH is 5, [OH-] is 10-9M, and pOH is 9. pH + pOH = 14.

  21. 89 pH 1.0 x 10-8M1.0 x 10-9M [H3O+] [OH-] 1.0 x 10-6M1.0 x 10-5M pOH 65 Next, the basic solutions. When [OH-] is 10-6M, the pOH is 6. Since [H3O+] 10-8M, the pH is 8. When [OH-] is 10-5M, and [H3O+] is 10-9M, the pOH is 5 and pH is 9. Again in both cases the sum of pH and pOH is 14.

  22. 6.707.30 pH 2.0 x 10-7M1.0 x 10-7M [H3O+] 1.0 x 10-7M2.0 x 10-7M [OH-] 7.306.70 pOH However, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. For example, we skipped over the value of 2.0 x 10-7. This is more complicated. However, if you use a calculator that will handle logarithms, it is a very simple calculation. First you enter the hydronium ion concentration. You can use decimal format or scientific notation. Next push the log button. Then change the sign by pushing the +/- button. In this case we get 6.70 for the pH. The other values can be obtained in the same way.

  23. PH ScalePH = -log [H+]Step 1 : Enter [Molarity of H+]Step 2 : Press “log” and hit +/- keyReverse for graphing calculator

  24. More vocabulary • Diprotic Acid • H2CO3   =    H+  +    HCO3- • HCO3-=   H+  +    CO3-2 • Triprotic acid • H3PO4+H2O-->H3O+H2PO4 • It's second ionization: H2PO4+H2O-->H3O+HPO4 • It's third ionization: HPO4+H2O-->H3O+PO4 • Oxyacid – compound of H, O, and a third element usually a nonmetal. Ex HNO3 • Organic acid – has a carbon

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