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Acids and Bases - Coggle Diagram
Acids and Bases
Acids and Bases (review) (L1)
Properties of Acids/Bases
Acids: -Turns red litmus red and blue litmus red
-pH less than 7
-Conduct electric current
-Reacts to produce H2
-Tastes sour
Bases: -Turns blue litmus blue and red litmus blue
-pH greater than 7
-Conducts electricity
-Do not react with metals to produce H2
-Tastes bitter
-Feels slippery
Acids:
IUPAC Naming: Just naming the compound but with the word aqueous in front of it.
Classical Naming: Anion ending with id - hydro
ic acid Anion ending with ate -
ic acid Anion ending with ite - ____ous acid
Exceptions to Rules:
Bases:
IUPAC naming: Just naming the compound but adding the word aqueous in front of it.
Strong and Weak Acids and Bases:
Acids:
Strong Acids: Reacts completely with water to form hydronium. In other words, they are acids that ionize 100% in water.
Properties: Very reactive and are very conductive.
Where to find them: There are 6 of them on the acid table in data booklet.
Weak Acids: Acids that react incompletely with water (less than 50%) to form hydronium ions.
Properties: Slightly reactive and have weak conductivity.
mono/polyprotic:
Monoprotic Acid: An acid that only has one hydrogen atom which ionizes in water.
Polyprotic Acid: An acid that has more than one hydrogen atom which ionizes in water.
Bases:
Strong Bases: Anything that completely dissociates into ions when in water to produce hydroxide.
Properties:
Where to find them: Everything in group 1 and 2 excluding Li and H
Weak Bases: When a low percentage of molecules react/dissociate in water to produce hydroxide ions.
Properties:
Mono/polyprotic:
Monoprotic Bases: A base that can dissociate/react with water (forming OH ions) in 1 step. Basiclly, it only takes 1 hydrogen ion.
Polyprotic Bases: Bases that can dissociate/react with water in more than one step. Basically, it takes more than 1 hydrogen ion.
Neutralization Reaction: When an acid and base react with each other and produce an ion(salt) as well as water.
Arrhenius and Modified Arrhenius and Acid and Base in Solution (L2):
Arrhenius Theory of Acids and Bases:
Acid: Any substance that ionizes and forms hydrogen ions (H+) in aqueous solution.
Base: Any substance which dissociates to form hydroxide ions (OH-) in aqueous solution.
Modified (revised) Theory of Arrhenius:
Examples:
Bases: Anything that dissociates to produce hydroxide ions (OH-) and goes through a single replacement or two step process.
Acids: Anything that which ionizes to produce hydronium ions (H3O) in an aqueous solution.
Brownsted-Lowry Acid Base Definitions: Note that this doesn't need to be memorized, but it is very useful.
In a reaction, H+ ions will be transferred to the base to neutralize it. So bases gain protons.
In a reaction, H+ ions will be taken from acids, also to neutralize it. So bases loose protons.
Concentration of Acid and Base and Ph and pOH (L4):
Concentration: Do practice Problems. P.g. 11
Finding Concentration Of Hydronium Ions (H3O): Ionize the compound in water (make equation) then balance it to find the mole ratio. Based on your given, convert it to the H3O ion by using the formula C=n/V x mole ratio. The mole ratio is found from the balanced equation.
Finding Concentration of Hydroxide Ions (OH): Dissociate the compound then balance the equation. Then use the formula C=n/V x mole ratio to find the C of OH ions.
pH and pOH:
Significant Digits and pH: Anything past the decimal is a significant digit for your final answer. This does not apply to your given. Lets say your final answer is 2.22974 and your smallest given is 4.2, this means your round to 2 sig digs. So the answer is 2.23.
Convert pH to pOH and pOH to pH: To find pOH when given pH, just subtract the pH from 14. To find the pH when given the pOH, just subtract the pOH from 14
Just subtract the given from 14 to convert
Finding concentration of H3O from pH: Use your anti lock (10^x) and input your pH with a negative sign in front of it. E.g. [H3O]=10-pH
Finding concentration of OH from pOH: Use your anti-lock (10^x) and input your poH with a negative sign in front of it. E.g. [OH]=10-pOH
Finding pH (For H3O): Once you have converted the C of solution to the C of H3O ions, then you can plug it into the following formula
Formula: pH = -log[Concentration of H3O ions] where C = concentration.
Finding pOH (For OH): Once you have converted the C of of solution ot C of OH ions, then you can plug it into the following formula
Formula: pOH = -log(Concentration of OH ions) where C = concentration.
Common Acid-Base Indicators (L5): Just practice this.