Acid and Base Definitions PDF

# Chapter 16 - Acid and Bases ## Acid; Base Definition ### 1.) Arrhenius definition - Acid => a substance that produces H+ ion in solution - Acid formulas start with "H" - Base => a substance that produces OH- ion in solution - Metal hydroxides are the common base. - Ex: NaOH, KOH, Ca(OH)2 - HCl...

# Chapter 16 - Acid and Bases ## Acid; Base Definition ### 1.) Arrhenius definition - Acid => a substance that produces H+ ion in solution - Acid formulas start with "H" - Base => a substance that produces OH- ion in solution - Metal hydroxides are the common base. - Ex: NaOH, KOH, Ca(OH)2 - HCl (aq) + H2O (l) -> H+ (aq) + Cl- (aq) - L-> H+ ion => a proton - H+ + H2O -> H3O+ (hydronium ion) ### Equivalent - Bronsted-Lowry Definition of Acid; Base - In an acid-base reaction - acid => H+ ion donor - base => H+ ion accepted - HCl + NH3 -> NH4+ + Cl- - acid base conjugate acid conjugate base * H2CO3 (aq) - acid * HCl - C base definition - (conjugate base) * NH3 its derivatives are also a base - CH3NH2 ## Lewis Solution **Acid** => electron pair acceptor **Base** => electron pair donor  - Ex: Base -> C Acid - (conjugate Base) HSO4- HPO4 ^2- C6 H5 NH2 - Acid -> base - (conjugate Base) H2SO4 HPO4 ^2- C6 H5 NH2 ## Strong Acids; Weak Acids - Strong acids, like the strong electrolytes, completely dissociate in a solution. - Weak acids, only partly dissociate into ions in a solution - Perchloric acid HClO4 - Hydrochloric acid: HCl - Sulfuric Acid: H2SO4 - If the acid is not strong, it is weak - Nitric Acid: HNO3 - H2CO3, HCN, HF - HCN (aq) -> H+ + CN- - 99% -> 1% ## Strong Base; Weak Base - LiOH - NaOH - KOH - Other metal hydroxides are weak base - Al(OH)3, Mg(OH)2 - NH3, its derivatives are also the weak base ## Binary Acids - Have acidic hydrogens attached to a nonmetal ion - Ex: HCI, HF - HF, HCl, HBr, HI - F, Cl, Br, and I compare the bond strength, decreases top to bottom in a group - H2O HF; - F, Cl, Br, and I are in the same row => compare the electronegativity. - Higher the electronegativity, the stronger the acid ## Oxy - Acids - Ex: H-O-Y (always will have a third element in Oxy-acids) - HCIO vs HBrO3 - Which is stronger? HClO3 is stronger because Cl has a higher electronegativity than Br. - The "Y" is compared based on the electronegativity of "Y" - Higher the electronegativity of Y -> the stronger the acid is ## Stronger Acids and Weaker Acids - Stronger acids have a weaker C-base (conjugate - Weaker acids have a stronger C-base (conjugate) ## Monoprotic Acid, Polyprotic Acid - HCl, HNO3 => monoprotic acid - Poly protic Acid - I have more than one ionizable hydrogen - Ex: H2SO4, H2CO3, H3PO4 - Diprotic acid, Triprotic acid - In polyprotic acids, the first "H" is ionized easier than the second "H" - H2SO4 (aq) + H2O(l) -> (H3O+) + HSO4^- - HSO4 (aq) + H2O(l) -> (H3O+) + SO4^2- - H2SO4 is a stronger acid than HSO4^-