chemistry final
list the conjugate acid-base pairs. H2O + NH3 -> NH4 + OH
H2O and OH- are acids, NH3 and NH4 are bases
in the following reaction, HCl + NH3 -> NH4 + Cl, which substance acts as the bronsted-lowry acid?
HCl
what is the OH concentraion in a 0.1 M HCl solution?
1 x 10^-13
what is the concentration of hydroxide ions in a solution that has a pH of 6.0?
1 x 10^-8
what is the concentration of hydroxide ions in a solution that has a pOH of 8.0?
1 x 10^-8
what are the highest concentrations of H3O ions and OH ions that can coexist in an aqueous solution?
1.0 x 10^-7 M each
the concentration of OH of an aqueous solution is 6.4 x 10^-5 M. what is the concentration of the H3O?
1.6 x 10^-10
what is the H3O concentration in a 0.0040 M solution of NaOH?
2.5 x 10^-12
what is the pH of a 0.0001 M HCl solution
4
write the formula for the salt present: calcium hydroxide combined with phosphoric acid
Ca(PO4)2
in the following reaction, which substance is the conjugate base of HClO4? HClO4 + H2O -> H3O + ClO4
ClO4-
write the formula for the salt present: sulfurous acid combined with potassium hydroxide
K2SO4
in the following reaction, HCl + NH3 -> NH4 + Cl, which substance acts as the bronsted-lowry base?
NH3
how is a solute different than a solvent?
a solute is dissolved into the solvent. the solvent dissolves the solute
name the acid present in vinegar
acetic acid
a solution that has a concentration of H3O equal to 1 x 10^-4 M is
acidic
when making a dilute acid solution, should you add acid to water or water to acid?
add acid, because the reverse is exothermic and can be unpredictable
arrhenius acid
any substance that produces hydrogen ions or hydronium ions when dissolved in water
arrhenius base
any substance that produces hydroxide ions when dissolved in water
a solution that has a pH of 4.0 is
basic
do acid-base pairs come before or after the arrow?
before
a standard solution
contains a precisely measured amount of solute, must be compared with a solution of primary standard before use, is the known solution used in a titration
glacial acetic acid is a highly viscous liquid that is close to 100% CH3COOH. when it mixes with water, it forms...
dilute acetic acid
describe role of bronsted-lowry acid
donates hydrogen
what type of solute-solvent solution combination is carbon dioxide in air?
gas-gas
bronsted-lowry acids and bases...
give H and take H, respectively
a strip of pH paper
gives a quick approximation of pH
glacial acetic acid does not conduct electricity, but dilute acetic acid does. explain this statement
glacial acetic acid is concentrated- it is neutral. the dilute acid will break up and allows electricity. adding water shifts the equilibrium so that more ions are formed and can conduct electricity.
write the name for HF (aq)
hydrofluoric acid
a strong acid...
ionizes completely in solution, produces hydronium ions in a solution, and is considered a strong electrolyte (all of the above)
which of the following is not true regarding the self-ionization of water?
it shows that water is a strong electrolyte
if a solution is electrically neutral, can all of its ions have the same type of charge?
no, because neutral is when there are enough neutrons and electrons to balance each other out
arrhenius acids and bases...
produce H+ and OH-, respectively
all of the KBr that will dissolve in a solution has dissolved, and several undissolved crystals remain on the bottom of the beaker. the solution is
saturated
describe role of bronsted-lowry base
the base receives hydrogen ion
when conduct an acid-base titration,
the equivalence point must be reached
how would you classify nitric acid (HNO3) in the reaction represented by the equation? HNO3 + H2O -> H3O + NO3
strong acid
what is an example of a solid-liquid solution?
sugar-water solution
name the acid present in car batteries
sulfuric acid
if the amount of dissolved solute in a solution at a given temperature is greater than the amount that can permanently remain in a solution at that temperature, the solution is said to be
supersaturated
at the end point of a titration using an acid-base indicator,
the pH of the solution should change abruptly and the color of the acid-base indicator should change
which does not affect the rate at which a solid solute dissolves?
the vapor pressure of the solvent
