 acids always have as the state and always have A. Naming Acids and Bases 6.1 Theories of Acids and Bases Section 6: Acids & Bases Rules 1. hydrogen becomes acid 2. hydrogen becomes acid 3. hydrogen becomes acid ____ide hydr____ic _____ate_____ic ____ite____ous (aq) hydrogen Rule 1 applies to H+ with elemental anions Rules #2 and 3 apply to H+ with polyatomic ions

Examples: hydroiodic acid phosphoric acid nitrous acid sulphurous acid Change each of the following to the appropriate acid name and give the formula: HI(aq) H 3 PO 4 (aq) HNO 2 (aq) H 2 SO 3 (aq) 1. hydrogen iodide = 2. hydrogen phosphate = 3. hydrogen nitrite = 4. hydrogen sulphite =

 most bases are ionic compounds that are named accordingly Examples: sodium hydroxide sodium hydrogen carbonate magnesium hydroxide ammonia Name each of the following bases: 1. NaOH(aq) = 2. NaHCO 3 (aq) = 3. Mg(OH) 2 (aq) = 4. NH 3 (aq) =

 IUPAC names for acids and bases are simply the word “aqueous” followed by the ionic name Examples: aqueous hydrogen iodide aqueous magnesium hydroxide aqueous hydrogen sulphite aqueous sodium hydrogen carbonate Write the IUPAC name for each of the following acids and bases: 1. hydroiodic acid = 2. magnesium hydroxide = 3. sulphurous acid = 4. sodium hydrogen carbonate =

B. Properties of Acids and Bases  are of a substance empirical propertiesobservable properties  acids, bases and neutral substances have some properties that distinguish them and some that are the same

AcidsBases Neutral Substances               sour bitter electrolytes electrolytes, non- electrolytes bases acids indicators do not H 2(g) eg)HCl(aq), H 2 SO 4 (aq) eg) NaCl(aq), Pb(NO 3 ) 2 (aq) eg)Ba(OH) 2 (aq) NH 3 (aq) less than 7 greater than 7 of 7 litmus - bromothymol blue - redblue yellow taste neutralize react with react with to produce metals phenolphthalein - colourless pink affect indicators the same way pH

 first proposed theory on acids and bases  his theory was that some compounds form  his explanation of the properties of acids and bases is called the electrically charged particles Svante Arrhenius Arrhenius theory of acids and bases C. Arrhenius Definition when in solution

 an Arrhenius is a substance that to form in water  a will in an aqueous solution baseincrease the [OH - (aq)] basedissociates hydroxide ions, OH  (aq),  an Arrhenius is a substance that (because it is molecular) to form  an will in an aqueous solution acidincrease the [H + (aq)] acidionizes hydrogen ions, H + (aq), in water

D. Modified Arrhenius Definition  the original definition of acids and bases proposed by Arrhenius is good but it has  some substances that might be predicted to be are actually limitations neutralbasic  it has been found that not all bases contain the eg)Na 2 CO 3 (aq), NH 3 (aq) hydroxide ionas part of theirchemical formula

 an Arrhenius is a substance that in aqueous solution base (modified) reacts with water NH 3 (aq) eg) OH  (aq)+NH 4 + (aq)  H 2 O(l)+ to produce OH  (aq) ions eg) Na 2 CO 3 (aq)+2H 2 O (l)  2Na + +2OH - H 2 CO 3 (aq)+

 it has been found using analytical technology like X-ray crystallography that in an aqueous solution  when acids ionize, they produceH + (aq) eg) HCl(g)  H + (aq) + Cl  (aq) H + (aq) ions do not exist in isolation  the hydrogen ion is extremely positive in charge and water molecules themselves are very polar so… it is that would exist in water without being attracted to the of other highly unlikelyhydrogen ions negative poleswater molecules

H 3 O + (aq)  this results in the formation of thehydronium ion +

 an Arrhenius is a substance that in aqueous solution acid (modified) reacts with water HCl(aq) eg) H 3 O + (aq)+Cl  (aq)  H 2 O( l ) + H 2 SO 3 (aq)H 3 O + (aq)+HSO 3  (aq)  H 2 O( l ) + to produceH 3 O + (aq) ions

Complete workbook questions Textbook: pg 253 #4 &5 Study for Solutions test Textbook pg #1-15, 23-26