1 / 11

Warm-up

Warm-up. What happens to the solubility of a gas in solution when: The temperature is increased The pressure is increased. Acid Properties. sour taste when dissolved in water turns litmus paper red/ phenolphthalein stays clear react with metals to make H 2 (g)

pembroke
Télécharger la présentation

Warm-up

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. Warm-up What happens to the solubility of a gas in solution when: The temperature is increased The pressure is increased

  2. Acid Properties • sour taste when dissolved in water • turns litmus paper red/ phenolphthalein stays clear • react with metals to make H2(g) • Ba(s) + H2SO4(aq)  BaSO4(aq) + H2(g) • react with bases to make salt and water • HBr(aq) + KOH(aq)  H2O(l) + KBr(aq) • conduct electricity (electrolytes)

  3. Common Acids • Sulfuric acid: H2SO4 • used in car batteries • Nitric acid: HNO3 • used in explosives • Phosphoric acid: H3PO4 • used as flavoring in soft drinks • Hydrochloric acid: HCl • stomach produces it • Acetic acid: HCH3COO or HC2H3O2 • vinegar contains it

  4. Types of Acids • Monoprotic acids • Only have one acidic proton (H+) • HNO2, HBr, HCH3COO(HC2H3O2) • Polyprotic acids- diprotic, triprotic • Contains more than one acidic proton (H+) • H3PO4, H2SO4, H2Te

  5. Base Properties • taste bitter • turn pH paper blue/phenolphthalein turns bright pink • feel slippery when dissolved in water • react with acids to make salt and water • electrolyte

  6. Definitions of Acids and Bases • Arrhenius Acid- compound that creates H+ (H3O+) in an aqueous solution • Arrhenius Base- compound that creates OH- in an aqueous solution • HNO3 H+ + NO3- • NaOH  Na+ + OH-

  7. Definitions of Acids and Bases • Bronsted-Lowry Acid- molecule or ion that is a proton (H+) donor • Bronsted-Lowry Base- molecule or ion that is a proton (H+) acceptor • HCl + H2O  H3O+ + Cl-

  8. Identify the acids and bases of the following reactions • C6H5NH2 + H2O  C6H5NH3+ + OH- • HNO3 + H2O  H3O+ + NO3- • HCH3COO + H2O  H3O+ + CH3COO-

  9. Acid-Base Reactions • Amphoteric Substances • Can act as either acid or base depending on what they are mixed with • Example: Water, HSO4-

  10. Conjugate base What is left of the acid Missing a hydrogen Conjugate acid What become of the base Has an extra hydrogen Conjugate Acid-Base PairsConjugate acids and bases are always created by a B-L reaction (are products)

  11. Identify the parts of these reactions • C6H5NH2 + H2O  C6H5NH3+ + OH- • HNO3 + H2O  H3O+ + NO3- • HCH3COO + H2O  H3O+ + CH3COO- NH3 + H2O  NH4+ + OH-

More Related