1 / 24

Identifying Acids and Bases

Identifying Acids and Bases. pH Formula Name Characteristics Reaction to other substances. Identifying Acids, Bases and Salts. 2. By their formula: Compound Ions Type HX H +   X - acid YOH Y +   OH - base YX Y +   X - salt. Identifying Acids.

nhills
Télécharger la présentation

Identifying Acids and 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. Identifying Acids and Bases • pH • Formula • Name • Characteristics • Reaction to other substances

  2. Identifying Acids, Bases and Salts 2. By their formula: Compound Ions Type HX H+  X- acid YOH Y+  OH- base YX Y+  X- salt

  3. Identifying Acids Most acids begin with an H: HCl HClO3 H3BO3 HNO3 H2SO4 HN Exceptions: water H20 and acids containing carbon: CH3COOH

  4. Identifying Acids • Acids behave like acids only when dissolved in water. • It is only in solution where they dissociate and give up their protons (H+). • Therefore, acids are often written with subscript (aq) = aqueous solution • egHCl(aq)

  5. Binary Acids Binary Acids • Hydrogen is bonded to a second non-metal: • HCl, HF, HBr, HI, H2S

  6. Naming Acids • Acids must be in solution. • The formula HF does not indicate state of matter: solid compound: hydrogen fluoride in solution: hydrofluoric acid.

  7. Naming Acids • If in aqueous form, use: Hydro……….ic acid eg. HClHydrochloric acid • If no state is given, use: Hydrogen…..….-ide eg. HClHydrogen chloride

  8. Naming Binary Acids Name the acid HI (Hydrogen Iodide): • Start with hydro- • Take anion root -iod • add -ic • Add to end acid • Hydroiodic acid

  9. Naming Binary Acids Name H2S (hydrogen sulfide) as an acid in solution: • Start with Hydro- • Add anion root Sulfur- • Add -ic • Add Acid • Hydrosulfuric Acid

  10. Naming Acids with Oxygen (polyatomic ions) • Do not add hydrogen to these names • Naming depends the anion (-ate, -ite, per-) • If ion ends in "-ate“, add “ic” Eg. NO3 is called nitrate, So HNO3 (hydrogen nitrate) will be nitric acid Eg: hydrogen perchlorate ……HClO4 (aq) will be perchloric acid

  11. Naming Acids Example SO42- Sulfate H2SO4 Hydrogen sulfate or H2SO4 (aq) Sulfuric acid

  12. Naming Acids • CH3COO- acetate ion • CH3COOH hydrogen acetate • CH3COOH (aq) acetic acid • BrO3- bromate • HBrO3 hydrogen bromate • HBrO3 (aq) bromic acid

  13. Naming Acids: Polyatomic with Oxygen • Polyatomic ion ending in “–ite”, The acid will end in "-ous." Example: ClO2- anion is chlorite, HClO2 is called chlorous acid

  14. Naming Acids • SO32- Sulfite ion • H2SO3 hydrogen sulfite • H2SO3 (aq) sulfurous acid

  15. Naming Acids: Polyatomic with Oxygen Example, the perchlorate ion is ClO4-, HClO4 (aq) is called perchloric acid.

  16. Naming Acids Summary • Binary Acids: hydro……ic acid • Containing Polyatomic ion with Oxygen: Anion Acid Ends with –ate ……………ic acid Ends with –ite ………..…ous acid Starts with per- per…………ic acid Starts with hypo- hypo……..ous acid

  17. Common Acids • Hydrochloric acid – stomach acid (HCl) • Muriatic acid – pool disinfectant (also HCl) • Acetic acid - vinegar , CH₃COOH • Citric acid – lemon juice, C₆H₈O₇ • Lactic acid - fermented milk CH₃CHCO₂H • Ascorbic acid – vitamin C, C6H8O6 • sufuric acid – battery acid, H2SO4 • Nitro-hydrochloric acid -Aqua regia

  18. Bases • Bases can be identified by their chemical formula: The chemical formula of a base usually ends with hydroxide ion (-OH). • Bases usually start with a metal or NH4 + See page 227

  19. Bases • Bases, like acids, behave like bases only when dissolved in water. • Therefore, bases are often written with subscript (aq) = aqueous = in solution

  20. Naming Bases- Strong • Most strong bases contain hydroxide (OH), a polyatomic ion. • Therefore, the naming strong bases follows same rules for naming ionic compounds: anion + cation • NaOH is sodium hydroxide, • KOH is potassium hydroxide, • Ca(OH)2 is calcium hydroxide.

  21. Naming Bases-Weak • Weak bases made of ionic compounds are also named using the ionic naming system. • NH4OH is ammonium hydroxide.

  22. Common Household Bases NaOH(aq) draino, caustic soda, lye, soap NaClO (aq) sodium hypochlorite-bleach Mg(OH)2(aq) antacid Ca (OH)2(aq) slaked lime NH4OH(aq) ammonium hydroxide, cleaning products Na2CO3 sodium carbonate (washing soda) NaHCO3 sodium bicarbonate (baking soda) See page 227

  23. Fun Facts about Bases • Sodium hydroxide is used to make soap. • Ammonium hydroxide is used to remove ink from clothes and remove grease from windows. • Bases are molecules which attract hydrogen ions from acidic molecules. • All alkalies (basic, ionic salt of an alkali metal or alkaline earth metal) are bases, but not all bases are alkalies. • Baking soda can be used to fight fires by obstructing the flow of oxygen.

  24. Properties of Acids and Bases See page 229 Take the Section 5.1 Quiz

More Related