Alex Acid and Bases notes

-Acids: A substance that releases a H+ (hydrogen) ion when dissolved in water.

- Bases: A substance that releases an OH- (hydroxide) ion when dissolved in water.

-pH scale: measure how acidic or basic a liquid is.

-Acids will sour and feels rough and can neutralize bases, forming water and salt.

-Acids always have H in the front of it so an example would be HCl.

-acidic solution [H]>[OH]

-acids have a pH level of 0-6

-Bases will typically feel slippery to the touch and can neutralize acids, forming water and a salt in the process.

-Bases will have an OH in there structure so an example is NaOH.

-basic solution [H]<[OH]

-basic solutions have a pH of 8-14

-neutral solutions [H] = [OH]

-neutral solutions have a pH of 7.

-In general bases and acids can be corrosive and compounds that release ions (+ or -) in a solution.

-strong acids/bases will fully dissociate 100% fully dissociate

-weak acids/bases will semi dissociate x < 100%

-strong acids that i need to know HCl (hydrochloric acid), HNO3 (Nitric acid), H2SO4 (sulfuric acid), HBr (Hydrobromic acid), HI (hydroiodic acid), HClO4 (perchlorate acid) and, HClO3 (chloric acid)

-(g) = gas (s) = solid (aq) = aqueous

-acids with and without oxygen:

Acids without oxygen rule: Hydro take off gen of hydrogen take the first part of the other gas and add ic to the end. so for an example HCl would be Hydrocloric.

naming acids with oxygen rule with ate ending: Hydrogen you get rid of, then take nitrate remove the ate and add ic

naming acid with oxygen rule with ite ending: take off hydrogen take chlorite remove the ite and add ous so HClO would be Chlourous.

exceptions: H3PO4 phosphate → phosphoric acid. H3PO4 → phosphorous acid. H3SO4 sulfuric acid or sulfurous acid.