chem 11 - stoichometry and acids/bases

excess reactant

excess reactant

reactant that doesn’t limit amt of product obtained as there is more than needed of this

limiting reactant

reactant that limits amt of product obtained as there is less of this as calculated stoichiometrically

theoretical yield

amt of product taht would be obtained assuming perfect conditions

H3O+ is called what

hydronium ion, formed when acid in water

amphiprotic

pH in terms of log

pH = - log [H3O+]

High pH

Low pH

Neutral pH

high = basic (at 25 celsius)

low = acid (at 25 celsius)

neutral = 7 at 25 celcius

titration

A laboratory technique where a solution of known concentration is used to determine the concentration of an unknown solution by monitoring a chemical reaction.

endpoint

The point in a titration where the indicator changes color, signaling that the reaction is complete.

indicator

A substance that changes color at a specific pH level or during a particular chemical reaction, used to identify the endpoint in a titration.

strong acids

• HClO4 - perchloric acid

• HCl - hydrochloric acid

• HBr - hydrobromic acid

• HI - hydroiodic acid

• HNO3 - nitric acid

• H2SO4 - sulfuric acid

stoichiometry

calculating/ measuring amt of substances involved in a chemical reaction

how to arrive to moles from s/l/g

• grams —> molecular mass

• volume or cocentration —> C= n/V

• volume —> PV=nRT or 22.4 L/mol

exactly reacts means

why is one reactnat added as excess

to make sure otehrs r used up completely

when can yield be over 100%?

if impurities like solvent attached

proton acceptor

base

bronsted-lowry base

conditioning

A burette is often conditioned by rinsing it with the titrant to ensure no dilution or contamination occurs.

acids can also be written as

aqueous hydorgen ——

gravimetric

calculating masses of reactants/products in chemcial reaction

titrant

solution in the buret/ known concentration

equivalence point

point at which exact theoretical amt of titrant has been added to the sample

titrand

unknown concentration

another name is analyte

usually in flask

bases are proton —- and acids are

acceptors, acids are proton donors

H+ ion is same as ? why?

proton, becayse H+ has no neutron in nucleus for most common isotope, only proton. if ionize in water, electron is taken away, so only proton.

conjugate base

A conjugate base is what remains after an acid donates a proton (H+) in a reaction. It can potentially accept a proton, acting as a base in the reverse reaction.

conjugate acid

A conjugate acid is formed when a base gains a proton (H+). It can potentially donate a proton, acting as an acid in the reverse reaction

whys pure water neutral

equal amount of h+ and oh-

acids characteristics

• Sour

• Turns blue litmus red

• Reaction with Metals: Reacts with metals to produce hydrogen gas

• Ion in Solution: Produces H+ ions (protons) in aqueous solution

• Feel: Corrosive

• electrolyte

• loses properties when neutralized

• examples: citric acid, vinegar

bases characteristics

• Taste: Bitter

• Litmus Paper: Turns red litmus blue

• Feel: Slippery or soapy

• Ion in Solution: Produces OH- ions (hydroxide ions) in aqueous solution

• Reaction with Acids: Reacts with acids to form salt and water (neutralization)

• loses properties when reacting w acids

• examples: soap/ bitter melon

• electrolyte

when acid reacts w metal

h2 + salt

conductivity

if strong = strong electrolyte

for every 1 on ph scale

10x

ph measures amt of __ ions

H+

buffers

if strong — water

dissociate completely, weaker dont as well

alkali

bases

pH stands for

power of hydrogen

sample

limiting

why always need to be moles

balanced equations in relationship coeeffiencets is mole, nothing measures moles

3 types of stoic

gravimetric, solution,gas

4 types of chem analysis

titration, crystallization, filtration, gas collection

buffer

solution can resist ph change upon addtion of acid/base

alkali

base that can dissolve in watee