chemistry acids and bases

Arrhenius’ theory

acids release H+ ions in solution

• H⁺ reacts with OH^- to make water

bases release OH- in solution

• OH^- reacts with H⁺ to make water

hydrogen -ide

hydro_____ic acid

hydrogen -ous

______ic acid

hydrogen -ite

________ ous acid

modified arrhenious theory

acids are substances that react with water to produce hydronium ions

bases are substances that react to produce hydroxide ions

able to differentiate between strong and weak acids/bases

ionic hydroxide

1. dissociation equation with hydroxide as product

molecular compound (with H)

1. react substance with water to form hydronium

2. react again to balance charges

ionic compound ( no O or H )

1. write dissociation equation

2. react anion with water

3. produce either hydronium or hydroxide as question asks

metallic oxide (ionic + O)

1. react compound with water to make ionic hydroxide (smush)

2. dissociate for hydroxide as product

nonmetallic oxide (molecular + O)

1. react with water to make single product (smush)

2. react with water until hydroxide/hydronium produced

strong acid

• pH << 7

• high conductivity

• fast reaction rate

• completely reacts with water

• major entities are water and product

weak acid

• major entities present are reactants and water

• equilibrium arrow used

• pH < 7

• low conductivity

• slow reaction rate

strong base

• all ionic hydroxides from groups 1 & 2 (except beryllium)

• major entities are water and products

• 7<< pH

• fast reaction rate

weak bases

• dissociate partially (< 50% )

• equilibrium arrow used

• 7 < pH

• low conductivity

• slow reaction rate

monoprotic acid

only one acidic hydrogen in formula

polyprotic acid

more that one acidic hydrogen in formula

monoprotic base

only react once to produce hydroxide

after writing arrhenious equation, only one hydrogen able to bond with anion

polyprotic base

anion is able to bond with more than one hydrogen

there is more than 1 hydroxide present in chemical formula

titration

process of measuring and controlling addition of solution into measured volume of other solution

used to determine the concentration or standardize a solution.

MUST be repeated at least 3 times with end volumes in a 0.2 mL range of each other

equivalence point

exact theoretical amount of titrant needed to react completely with sample

measured by sudden change in empirical properties called endpoint

titration process

1. place specified volume of sample solution into Erlenmeyer flask and add few drops of indicator

2. drip the titrant slowly from burette to flask

3. record total volume of titrant added

4. calculate concentration of sample solution