1 / 14

Acids / Bases

Acids / Bases. Acids Taste sour Corrosive Conducts electricity pH < 7 Turns litmus paper red Formula contains H- Produces hydronium ions(H 3 O + ) in solution. Bases Taste Bitter Slippery to the touch Corrosive Conducts electricity pH > 7 Turns litmus paper blue

heman
Download Presentation

Acids / Bases

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Acids/Bases

  2. Acids Taste sour Corrosive Conducts electricity pH < 7 Turns litmus paper red Formula contains H- Produces hydronium ions(H3O+) in solution Bases Taste Bitter Slippery to the touch Corrosive Conducts electricity pH > 7 Turns litmus paper blue Formula contains –OH Produces hydroxide ions(OH-) in solution Turns phenolphthalein pink

  3. pH Scale BASES ACIDS 14 0 Strong NEUTRAL Strong 7 IONS – More ions = stronger A/B

  4. Strong Acids • Completely ionize when put in water H2SO4 HClO4 HNO3 HCl HBr HI Strong Bases • Completely ionize when put in water NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2 Any other acid/base not listed here is Weak Weak Acids/Bases – partly ionize in water

  5. Naming Acids/Bases BASES Name of metal + name of –OH EX: NaOH sodium hydroxide ACIDS Binary 2 elements H + nonmetal Prefix – hydroRoot – acid name Suffix – ic EX: HCl Hydrochloric acid Oxyacid H +polyatomic ion PI ends –ate=ic PI ends –ite = ous EX: H2SO4 sulfuric acid H2SO3 sulfurous acid

  6. Acid/Base Theories Arrhenius – in water only Acids – produce H+(H3O+)Bases – produce OH- Bronsted-Lowry Acids – proton (H+) donorBases – proton acceptor Lewis – broadest view Acids – electron pair acceptorBases – electron pair donor

  7. H+ + NH3 NH4+ 2. NaOH  Na+ + OH- 3. HF + H2O  F- + H3O+ • NH3 + H2O  OH- + NH4+ • HCl  H+ + Cl-

  8. Bronsted-Lowry • Acid – what it makes is its conjugate base Strong acid = weak conjugate base (and vice versa) • Base – what it makes is its conjugate acid Strong base = weak conjugate acid (and vice versa) NH3 + H2O  OH- + NH4+

  9. Practice • NH4+ + OH- NH3 + H2O • HBr + H2O  H3O+ + Br- • CO3-2 + H2O  HCO3- + OH- • HSO4- + H2O  H3O+ + SO4-2

  10. Neutralization Acid + Base  Salt+ water HCl + Sr(OH)2 SrCl2 + H2O **Double displacement reaction (Ionic Compound) (HOH)

  11. Self Ionization of Water H2O + H2O  H3O+ + OH- In pure water, H3O+ OH- In a solution, H3O+ OH- When H3O+> OH-, the solution is acidic When H3O+<OH-, the solution is basic

  12. Kw = [H3O+][OH-] = 1.0 x 10-14 pH = -log [H3O+] ; pOH = -log [OH-] pH + pOH = 14 [] = concentration = Molarity If a solution contains 1.3 x 10-2 M OH-, what is the hydronium ion concentration? What is the pH of the solution? Using the above equations: 1.0 x 10-14 = [x][1.3 x 10-2] [x] = [H3O+] = 7.69 x 10-13M pH = -log [7.69 x 10-13] pH = 12.1 pOH = -log [1.3 x 10-2] pOH = 1.89 pH + 1.89 = 14 pH = 12.1 OR

  13. Determine the [H3O+], [OH-], and the pH of a 0.01 M Sr(OH)2 solution. **Sr(OH)2 is a strong base, so it completely breaks apart into its ions when put in water – write the equation Sr(OH)2 (s)  Sr+2(aq) + 2OH-1(aq) Sr(OH)2 produces OH- when put into solution and since we know the [] of Sr(OH)2, we can use the mole to mole ratio to determine the concentration of the OH- Sr(OH)2(s)  Sr+2(aq) + 2OH-1(aq) 0.01 M 0.02 M [OH-] = 0.02 M Use Kw to find [H3O+] 1.0 x 10-14 = [H3O+][0.02] [H3O+] = 5.0 x 10-12M pH = -log (5.0 x 10-12) pH = 11.3

  14. If a solution has a pH of 4.23, what is the concentration of [H3O+]? What will the [OH-] be?

More Related