1 / 17

Acid and Base

Acid and Base. Ch 15 and 16 7-2. acids. 1. tastes sour. 2. conducts an electric current. 3. Causes certain dyes ( indicators) to change color. 4. Liberates hydrogen when it reacts with certain metals. 5. neutralizes basic solutions to form salts. Bases. 1. tastes bitter.

xalvadora-kieva
Télécharger la présentation

Acid and Base

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. Acid and Base Ch 15 and 16 7-2

  2. acids • 1. tastes sour. • 2. conducts an electric current. • 3. Causes certain dyes ( indicators) to change color. • 4. Liberates hydrogen when it reacts with certain metals. • 5. neutralizes basic solutions to form salts.

  3. Bases • 1. tastes bitter. • 2. conducts an electric current. • 3. causes certain dyes ( indicators) to change color. • 4. feels slippery. • 5. neutralizes acid solution to form salts.

  4. Definition of Acids and Bases • An acid is a source of hydrogen ions (H+) or hydronium ions (H3O+ ) in solution. HCl(aq) + H2O(l) H3O+ (aq) + Cl- (aq)

  5. A base is a source of hydroxide ions (OH-) e.g. NaOH(s) Na+ (aq) + OH- (aq) e.g. NH3 (aq) +H2O(l) NH4+ (aq) + OH-(aq)

  6. H H – + O O Cl Cl H H H H B. Definitions • Arrhenius - In aqueous solution… • Acidsform hydronium ions (H3O+) HCl + H2O H3O+ + Cl– acid

  7. H H – + N O O N H H H H H H H H B. Definitions • Arrhenius - In aqueous solution… • Bases form hydroxide ions (OH-) NH3 + H2O NH4+ + OH- base

  8. conjugate acid conjugate base B. Definitions • Brønsted-Lowry • Acidsare proton (H+) donors. • Bases are proton (H+) acceptors. HCl + H2O  H3O+ + Cl- acid base

  9. Conjugate acid base pairs • conjugate base: the species that remains after an acid has given up a proton • conjugate acid: the species that is formed when a base gains a proton

  10. conjugate acid conjugate base base acid NH3 + H2O NH4+ + OH-

  11. In the two examples water first acts as a base, then as an acid. • Any species which can both accept and donate protons is called amphiprotic. (also known as amphoteric)

  12. Give the conjugate acid for each of the following: Br – HSO4- CO32- HBr H2SO4 HCO3-

  13. List the conjugate acids for the following Bronsted bases • OH - • CO32- • NO3- • HCO3- • CN - H2O HCO3- HNO3 HCO3 HCN

  14. Give the conjugate base for each of the following: HF H3PO4 H3O+ F - H2PO4- H2O • Polyprotic - an acid with more than one H+

  15. List the conjugate bases for the following Bronsted acids • H2SO4 • HPO42- • HCO3- • H3O+ • H2PO4- HSO4- PO43- CO32- H2O HPO42-

  16. Review 2: Name the acid, base, conjugate acid and base for each reaction. CH3NH2 + H2O CH3NH3+ + OH - conjugate acid conjugate base base acid H3PO4 + H2O H3O + + H2PO4- conjugate acid conjugate base acid base HC2H3O2 + H2O H3O + + C2H3O2- acid base conjugate acid conjugate base CH3NH3+ + H2PO4-H3PO4 + CH3NH2 acid base conjugate acid conjugate base

  17. Review 2: Name the acid, base, conjugate acid and base for each reaction. H2PO4- + OH-HPO42- + H2O conjugate base conjugate acid acid base HCN + H2O CN- + H3O + conjugate base conjugate acid acid base NH3 + H2O NH4+ + OH - base acid conjugate acid conjugate base NO2- + HCO3-CO32- + HNO2 base acid conjugate base conjugate acid

More Related