Acids and Bases Flashcards
2 ways to make a solution
- dissolving a solid
- diluting a stock/standard
dilution
the process of reducing the concentration of a solution by adding more solvent
dilution factor
the concentration of the diluted solution divided by the concentration of the concentrated solution
qualitative analysis
the identification of the specific substances present
quantitative analysis
the measurement of the quantity of a substance present
qualitative chemical analysis
planning a double displacement reaction that forms a precipitate with a specific compound to detect the presence of an element
acids taste
sour
bases taste
bitter
acid SOLUTIONS conduct electricity T/F
T
acids (by themselves) conduct electricity T/F
F
bases conduct electricity T/F
T
bases feel
slippery
acids and litmus paper
turns blue litmus paper RED
bases and litmus paper
turns red litmus paper BLUE
acids reaction with active metals
produces hydrogen gas
bases reaction with active metals
no reaction
acids reaction with carbonate compounds
produces carbon dioxide
bases reaction with carbonate compounds
no reaction
3 types of acid-base theory
- arrhenius theory
- brosnted-lowry theory
- lewis theory
arhenius
- describes acitivies of acids and bases dissolved in water
- acids ionize/dissociate in aqueous solution to increase H+ ion concentration
- bases ionize/dissociate in aqueous solution to increase OH- concentration
limitations of arrhenius theory
- occurs in aquous solution, but water is often left out, but water is a polar molecule and must interact with the ions in some way
- ammonia produces a basic solution but does not contain OH- ions, ammonia also neutralizes acids
- limited to reactions in water
- cannot explain why salts that concain arbonate ions also have basic properties
H+ DO NOT exist is water solution but are snatched up by water molecules ro form hydronium ions
hydrogen ion H30+ aka hydrogen ion
amphiprotic/amphoteric
compounds that can act as either an acid or a base depending on the chemical reaction
conjugate pairs
two molecules or ions that differe because of the transfer of a proton
conjugate base (of the acid)
the particle that remains when a proton is removed from the acid
conjugate acid (of the base)
the particle formed when the base receives the proton of the acid
ionization
the formation of ions from uncharged molecules
dissociation
the seperation of individual ions from an ionic compounds as it dissolves inw water (started charged)
Bronsted-Lowry Theory
- includes all arrhenius acids + bases*
acids = a substance from which a proton (H+ ion) can be removed
bases = a substance that can remove a proton (H+ ion) from an acid
monoprotic acid
an acid which can supply one one proton
diprotic acid
acid which can supply up to two protons
triprotic acid
acid which can supply up to three protons
polyprotic acid
acid which can supply more than one proton
How is acid strength determined?
determined by the concentration of H+ ions in solution
strong acids
ionize > 99% upon dissolving in water
What are the strong acids?
- HCl
- HBr
- HClO4
-H2SO4 - HNO3
- HI
are all vey good electrolytes because of all the ions in solution
weak acids
dissociate less than 5% in water
very poor electrolytes because of the low concentration of ions in solution
How is base strength determined?
by the concentration of OH- ions is solution
the more OH- ions the stronger the base
strong bases
dissociate 100% upon disssolving in water.
strong base examples
oxides and hydroxides of group 1 metals and all group 2 metals below berllium
bery good electrolytes because of alll the ions in the solution
Weak Bases
dissociate much less than 100% upon dissolving in water, poor electrolytes
strong and weak refer to the % of ionization of dissociation of particles in water, concetrated and dilute refer to the amount of solute in a solvent
titration
an analytical procedure used in chemistry to determine the concentration of an unknown acid or base, uses a neutralization reaction and stoichiometry to calculate the concentration of the unknown solution
burette
a calibrated (has accurate volume markings) tube used to deliver variable known volumes of a solution during a titration
titrant
the solution in the burette during the titration (most often the solution of known concentration)
analyte
the solution in the Erlenmeyer flask during the titration most often the solution of unknown concentration
equivalence point
the point in a titration when the quantity of acid has exactly neutralized the quantity of base
endpoint
the point during a titration in which an observable change (usually colour change) caused by a significant change in pH has occured, signifying that the equivalence point has been reached
