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Acids Vs. Bases:
- Generally Acids are H+ ions attached to a nonmetal anion, or a polyatomic ion.
- Will usually have an H in front
- Generally Bases are Ionic Compounds with metal cations attached to a OH- ion.
- OH- are hydroxide ions.
- Will usually end in OH
→ Acids, Bases and Salts are known as electrolytes. Which means that when they are dissolved in water they split into their individual ions allowing for electrical conductivity.
The Theories:
→ There are 2 ones that we use to define Acids and Bases. (They build off of each other)
Arrhenius:
- Acids → When dissolved in water it will release H+ ions into the solution, increasing the concentration of H+ ions.
- H+ ions are also called protons, because that’s all it is. (a Hydrogen ion has no electrons).
- Bases → When dissolved in water it will release OH- ions (Hydroxide Ions) increasing their concentration in a solution.
- Base can also be referred to as Alkalinity.
- The Regents prefers this theory because it is easier to understand.
Bronsted-Lowry:
- Acids → Any substance that will donate a Hydrogen Ion. (H+)
- Bases → Any substance that will accept a Hydrogen Ion. (H+)
- Has a spot for the H+ ion to attach
- Conjugate Pairs →A base in the solution accepts the H+ Ion, becoming a conjugate Acid.
- Works the same way for conjugate Bases.
Naming:
Acids:
- For Acids with no oxygen you use the prefix “hydro”
- The add the second element's name but change the ending to “ic”
- They finally add “Acid” at the end.
- Should look like hydro(element)ic Acid
- Example: HCl (aq)
- Hydrochloric Acid
- Example: HI (aq)
- HydroIodic Acid
- For Acids with Oxygen you don’t use a prefix
- The first part is just the polyatomic Ion, then it will either end in “ic” or “ous”
- If the polyatomic ends in “ate” then the acid ends in “ic”
- If the polyatomic ends in “ite” then the acid ends in “ous”
- Finally we add “Acid to the very end”
- The pneumonic to remember this is:
- I ATE organIC apples, despITE being poisonOUS.
- Example: H
2
SO4
(aq) - The polyatomic is Sulfate so the acid will end in “ic”
Neutralization and Acid Base Equations:
Neutralization/ Titration:
→ The names can be used interchangeably.
- A neutralization reaction will usually look like
- Acid + Base → Salt + Water
- remember salt is an Ionic compound.
- The acronym to remember it is SWAB.
- When the reaction is done the acid and base neutralize each other, so the pH returns to 7.
- Titration is when you add an acid or a base with an unknown volume or Molarity, to another acid or base, with a known volume or Molarity, until it neutralizes so you can find the unknown variable
- When they are neutralized the moles of both the acid and base should be equal so from that we get the equation:
- (M
A
)(VA
) = (MB
)(VB
) - M= Molarity
- V= Volume
- A= Acid
- B= Base
- Equation is on the back of the reference table.
Other Equations:
- When you add an Acid with a more reactive metal, it will produce H
2
and a salt.- The more reactive metals can be found on Table J, in the reference table.
- Any metals shove H
2
will react with Acids, anything below it won;t - Cu, Ag, and Au won’t react with Acids.
- The acronym to remember these equations is: MASH
- Example:
- 2K + 2HCl → H
2
+ 2KCl
Strength (pH/pOH), and Indicators:
Strength:
→ The more Ions which can dissociate the stronger the acid or the base.
- Monoprotic- Has one H+ or OH- ion.
- Diprotic- Has two H+ or OH- ions.
- H
2
SO4
- This pattern for names continues on
- Organic Acids like Ethanoic Acid are generally weaker.
pH and pOH scale:
pH Scale:
→ Expression of how many H+ ions are in a solution. (The Acidity)
- 0-6 is very acidic (0 is the most acidic)
- 7 is neutral (really any number between 6-8)
- 8-14 is very basic. (14 is the most Basic)
- It is calculated using: -log[H+]
- [H+] means concentration of H+ ions in the solution.
- [ ] always mean concentration
- The higher the concentration of H+ ions, the lower the pH.
- The change between each number is x10.
- so going from a pH= 1 to pH= 2
- the concentration decreases by 10
- Going from pH=2 to pH= 4
- the concentration decreases by 100
pOH Scale:
→ Expression of how many OH- ions are in a solution. (The Alkalinity)
- opposite of pH
- found using a similar method: -log[OH-]
- 0-6 is basic
- 7 is neutral (really anything 6-8)
- 8-14 is Acidic
- You could also subtract your pH from 14 and it will give you the pOH.
Indicators:
- Change colors when Hydrogen is lost or gained. (Used to show the general pH)
- There are many different ones which have unique behaviors
- You can find the most common indicators and their colors for certain pH’s on the reference table (Table M)