The Chemistry of Acids & Bases

Properties of Acids Dilute solution have a _____taste Aqueous solutions conduct an electric current  What do we call substances that can conduct electric currents? **The greater the # of ions in solution, the greater the electrical conductivity. Acids react with bases to form a water & salt  _____________________ Acids react with certain metals to produce H 2 gas  Table J: _____________________________ Acids cause acid-base indicators to change color Lemons have citric acid! Vinegar has acetic acid! _________________ Strong acid = Weak acid =

Properties of Bases Bases have a bitter taste. Bases have a slippery or soapy feeling. Bases conduct an electric current. Bases react with acids to form water & salt. Bases cause acid-based indicators to change color. Strong base= Weak base =

Arrhenius Theory Arrhenius Acid = ______________________________________ ______________________________________ - Ex: **Some notes on the hydrogen ion!:  H + is really just a _________!  In a water solution, the positively charged proton is attracted to an unshared pair of electrons in the water molecules. Proton ends up covalently bonding with water to form _______________________ er/chap26/animate3/an26_037. mov

So, acids dissolve in water & react to produce ______________ & ________________. H 2 SO 4  2H 3 O + (aq) + SO 4 2- (aq) H 3 PO 4  3H 3 O + (aq) + PO 4 3- (aq)

Arrhenius Theory Arrhenius Base: = _____________________________________________ _____________________________________________ - Remember: hydroxide ion = OH - NaOH  Na + (aq) + OH - (aq) KOH  K + (aq) + OH - (aq) /chap26/animate3/an26_038.mov

Other Acid/Base Definitions Brønsted – Lowry Acids = _____________ Brønsted – Lowry Bases = _____________ Note: A “proton” is really just a hydrogen atom that has lost it’s electron! Lewis acid = _____________________________ Lewis base = _____________________________

Neutralization Reactions = an Arrhenius acid reacts with an Arrhenius base to produce water & a salt -General reaction: **All neutralization reactions have the same net equation: = enbowe/sections/projectfolder/animation s/HClandNaOHtgV8.html

Acid-Base Titration = the process of adding measured volumes of an acid or base of known concentration to an acid or base of unknown concentration until neutralization takes place -Through a titration, it is possible to calculate the concentration of the unknown solution: M A V A = M B V B astate.edu/group/ Greenbowe/sectio ns/projectfolder/fla shfiles/stoichiomet ry/acid_base.html

Monoprotic Acid: H+ molarity = molarity of acid solution - Ex: 2.5M HCl = 2.5M H + Diprotic Acid: H+ molarity = 2 x molarity of acid solution - Ex: 2.5M H 2 SO 4 = ___ H + Triprotic Acid: H+ molarity = 3 x molarity of acid solution - Ex: 2.5M H 3 PO 4 = ___ H + Monohydroxy Bases: OH- molarity = molarity of base solution - Ex: 3.0M NaOH = ___ OH - Dihydroxy Bases: OH- molarity = 2 x molarity of base solution - Ex: 3.0M Ba(OH) 2 = ___ OH -

Acidity vs. Alkalinity ** These terms refer to the relative strength of the acid or base in terms of H + and OH - concentrations.** -Acidity  ___________________________ -Alkalinity  _________________________ [H + ] > [OH - ] :_________ [H + ] < [OH - ] :_________

pH Scale  The pH scale expresses [H+] as a number from 0 to 14  Each pH unit represents a tenfold increase or decrease in [H + ] and [OH - ].  As [H + ] increases, [OH - ] decreases (and vice-versa).

Acid-Base Indicators Indicator = ____________________________________ ____________________________________ **REMEMBER: Everything you need to know about acid- base indicators is on Table M in the reference tables!!** matter/chap27/demos/dm 27_010.mov