Presentation on theme: "Warm Up A solution has a H+ ion concentration of 3.5 X 10 -8 M. a. What is the pH? b. What is the [OH - ]? c. What is the pOH? d. Would the litmus paper."— Presentation transcript:
Warm Up A solution has a H+ ion concentration of 3.5 X M. a. What is the pH? b. What is the [OH - ]? c. What is the pOH? d. Would the litmus paper turn color? e. What color would the cabbage juice turn?
Warm Up A solution has a H ion concentration of 3.50 X M. a. What is the pH? 7.46 b. What is the [OH - ]? 2.88 X M c. What is the pOH? 6.54 d. Would the litmus paper turn color? e. What color would the cabbage juice turn?
Red cabbage contains a pigment Molecule called flavin that turns color in the presence of H+ and OH- ions pHColor 2Red 4Purple 6Violet 8Blue 10Blue/Green 12Green/Yellow
Lab Debrief / Calculations 1. What color did the strong acids turn? 2. What color did the strong bases turn? 3. Were food products primarily acids or bases? 4. Were cleaning products primarily acids or bases? 5. What did you notice about the bleach? 6. Were there any surprises? 7. What did you learn about litmus paper? Is it a good quantitative measure of pH?
How did you do on the WS?
3 Definitions of Acids and Bases
Arrhenius Acids and Bases Acid- compounds containing hydrogen that ionize to yield H+ ions in aqueous solutions. Base- compounds that ionize to yield hydroxide ions in aqueous solutions.
Bronsted-Lowry Acids and Bases Acid- hydrogen-ion donor Base hydrogen-ion acceptor HNO 3 + H 2 O NO 3 + H 3 O
Bronsted-Lowry Acids and Bases always travel in pairs Reactant side Acid- hydrogen-ion donor Base hydrogen-ion acceptor Product side Conjugate acid- product formed when a base accepts a H+. Conjugate base- product formed when an acid has donated a H+.
HNO 3 + H 2 O NO 3 + H 3 O
Identify the following as Bronsted-Lowry acids or bases. 1. HNO 3 + LiOH LiNO 3 + HOH 2. 2HBr + Ca(OH) 2 CaBr 2 + 2HOH Which are the conjugate acids and bases?
Lewis Acids and Bases Where have your heard that name before??
Lewis Acids and Bases This is a more general concept and works to include compounds that may not have H+ or OH-. Acid- a substance that accepts a pair of electrons Base- a substance that can donate a pair of electrons
Draw the Lewis dot structures for NH 3 and BF 3 Which would be the Lewis Acid? Base??
Draw the Lewis Structure for PCl 3. Is it a Lewis Acid or Base??
Try this one!! AlCl 3 + Cl AlCl 4
Warm Up A solution has a OH - ion concentration of 5.3 X M. a. What is the pOH? b. What is the pH? c. Is the substance an acid or base?
Warm Up A solution has a OH - ion concentration of 5.30 X M. a. What is the pOH? 3.28 b. What is the pH? c. Is the substance an acid or base? Base– be sure that you are looking at the pH!!!
Strong Acids and Bases Strong Acids- ionize completely in aqueous solution. Weak Acids – only partially ionize in solution Strong Bases- ionize completely. Weak Bases- partially ionize.
Lets talk about neutralization reactions!!
Warm Up Predict the products and balance the following reaction KOH + H 2 SO 4 How many grams of sulfuric acid is needed to neutralize 2.76g of potassium hydroxide.
Vocab Terms Binary acid- contains two different elements, H and something else. Polyprotic acid- contains two or more H+ ions. Oxyacid- compound with H, O and a 3 rd element (typically a nonmetal).
Classify the acids-- Are they binary, polyprotic or an oxyacid? HCl H 2 SO 4 HNO 3 H 3 PO 4 HC 2 H 3 O 2 H 2 CO 3
Who remembers the 6 acids that you had to memorize?
Identify the following as Bronsted-Lowry acids or bases. 1. H 2 SO 4 + Ca(OH) 2 HOH + CaSO HF + Mg(OH) 2 CaF 2 + 2HOH Which are the conjugate acids and bases?