neutralizes (partially) a base - colorless - blue to red - electrolyte - reacts with reactive metals, to create hydrogen - tastes sour

neutrallizes (partially) with acids - colorless - red turns blue - electrolyte - feels slippery tastes bitter

forms colored and colorless solutions - only ionic have color - does not affect litmus

unit c - topic two Flashcards by Ella Thorsteinson

common uses of an acid

wart removal, enhance food flavor

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common uses of an base

relieve indigestion (acidic stomach)

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(naming acids) acids in pure form

are named like an ionic compound

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(naming acids) acids in colution

given an acid name

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hydrogen ____ ide —>

hydro_____ic acid

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hydrogen _____ ate —->

______ ic acid

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hydrogen _____ ite —->

____ ous acid

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acids

neutralizes (partially) a base

colorless
blue to red
electrolyte
reacts with reactive metals, to create hydrogen
tastes sour

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base

neutrallizes (partially) with acids

colorless
red turns blue
electrolyte
feels slippery tastes bitter

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neutral solution

forms colored and colorless solutions

only ionic have color
does not affect litmus

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electrolytes help to determine

strength

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sir humphrey davy

discovered elements

-just the thought that hydrogen was responsible for acids properties

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justin von lieberg

acids bare just salts of ionic compounds with hydrogen replacing the metal ion

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neutralizes

balancing using acids + bases to cancel/balance out

-creates a salt –> cation and anion, with no net charge

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what is this an example of

HCL + NaOH –> H2O + NaCl

neutralizing (creates a salt and water)

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ionize

creating a seperation of charge

-can ionize molecular compounds

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acids are not ____ but can ____

ionic, ionize

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salt

cation + anion then form neutral charge
              example Na(+)Cl(-)

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svante arrehenius

provided first useful theoretical defintion
-acids are substances that ionize in water to form hydrogen ions, while
-bases are compounds that dissociate in water to form hydroxide ions
key- interacts with water

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paul antoine giguere

hydrogen ions assosciate with a water molecule to form a hydronium ion > H3O

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arrenhius acid

ionizes in water to form a Hydrogen ion and a balancing species

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arrenhius base

dissosciates in water to form OH ion and a balancing species

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balancing species

ion that is not hydrogen to balance out the charge

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no current is a

molecular compound (do not dissosciate)

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weak current is a

weak acids + bases

strong current is a

strong acid or base

dissosciating vs ionzing

- dissosciate is seperation of IONS, who are not literally attached - ionize literal seperation to create charge

dissosciating

breakdown of a substance into smaller particles

ionizing

process which atoms get a positive or negative charge | -formation of ions

revision of arrhenius (acids)

acids are substances that react with water to produce hydronium ions

revision of arrhenius (bases)

are substances that react with water to produce hydroxide ions

straight arrow in an equation

strong acid/base

arrow points either way

weak acid/base

buffers

allows pH to stay at a certain point | -acid buffer or basic buffer

polyprotic

things have two hydrogens | -there is going to be more of an answer

negative ions that still have a hydrogen often can be

BOTH acids + bases | example- HSO3(-)

since hydrogen isn't a metal..

we don't ignore it when finding the strength of an acid or base

hydrogen gas (charge)

has a net charge of zero

how do i know to use hydrogen gas

due to the balance in equation charge - since gas is neutral - other than gas hydrogen is +1

metals (charge)

are not going to have a charge

strong vs weak means

how capable it can ionize in water

weak acids

ionize 50 percent less - weak conductors - mostly molecules

strong acids

- ionize 100 percent - strong conductors - only ions

lower the pH

more acidic

higher the pH

more basic

pH at seven

neutral

dynamic equilibrium

not all the molecules stay seperat | -equal + opposite

percent ioniziation (strong acid)

*HA* is going to turn into *H-* *A+*

percent ionization (weak acids)

*HB* is going to turn into *HB* (mostly) (and small amounts of) *H-* *A+*

weak acid info

ionize less than 50 percent in water - weakly conductive - contains mainly molecules in solution

strong acid info

ionize 100 percent in water - strongly conductive - contains only ions in solution

weak bases info

reacts partially with water to form relatively few hydroxide ions

strong bases

dissosciate completely | -strong conductors

empirical properties of strong acids

pH very low to low - high conductivity - fast reaction rate

empirical properties of weak acids

pH low to medium - low conductivity - slow reaction rate

empirical properties of strong bases

pH very high to high - strong conductors - fast reaction rate

empirical properties of weak bases

pH medium to high - weak conductors - slow reaction rate

monoprotic acids

only have a single hydrogen, thus can only loose one hydrogen to produce a hydronium ion -react once with water

polyprotic acids

contain more than one hydrogen | -can react multiple times with water, each time giving up a hydrogen

monoprotic base

capable of only gaining one hydrogen from water to produce hydroxide ions

polyprotic base

bases that are able to react with water more than once | -but all reactions are less than 50%

how is the strength of a base determinded

by how well it can accept an H+ from the water it is reacting with (dissosciate) - strong base will react quickly, since it is able to accept the H+ very well - weak base will react slowly, since it is only partially able to accept the H+

how is the strenght of an acid determinded

by how well it is able to give away a H+ to produce a hydronium ion (dissosciate) - strong acids react very quickly, since they are able to give away an H+ easily - weak acids react very slowly since they are not able to easily give away a H+