Chemistry Chapter 15
1.0x10 -7 each
what are the highest concentrations of hydronium and hydroxide ions that can coexist in an aqueous solution
transition interval
pH range over which an indicator changes color
weak
these are typically ___________ acids/bases
indicators
these changes as the pH changes
neutralization/double replacement
titrations are what kind of reactions
3.1-4.4
transition interval for methyl orange
neutral
because the hydronium and hydroxide ion concentrations are the same in pure water, it is________-
hydroxide
if the concentration of a solution is more basic, it is greater in
8-10
transition interval for phenolthalein
4
what is the pH of a 0.0001 M HCl solution
volume
what quantity do we measure directly in titration
3.0-4.6
whats the pH range of bromthymol blue
water molecules, hydronium, hydroxide
when water undergoes self ionization it has this
the equivalence point must be reached
when you conduct an acid-base titration
is acidic
a solution that has a [H3O+] equal to 1x10-4
is acidic
a solution that has a pH of 4.0
gives a quick approximation of pH
a strip of pH paper
phenolphthalein
according to the table above, which pH indicator would be the best choice when titrating acetic acid, CH3COOH, with sodium hydroxied
both b and c
at the end point of a titration using an acid base indicator,
acid'base indicators
compounds whose colors are sensitive to pH
what unknown quantity can be calculated after performing a titration?
concentration
by pH at which they change colors
how are indicators classified
1.58x10-2 mol
how many moles of NaOH must be dissolved in 1.00 L of water to make NaOH with a pH of 12.2
hydronium
if concentration of a solution is more acidic, it is greater in
is less than 7.0
in the figure on the previous page, the pH at the equivalence point
gastric juice, lemons, vinegar, soft drinks, tomatoes, oranges, milk
name some materials with a more acidic pH range
hydronium and hydroxide levels are almost equal
rapid changes in a pH solution indicate what
1.6x10-10
the [OH-] of an aqueous solution is 6.4x10-5. what is the [H3O+]
pH
the _____ of a solution can be measured using either a pH meter or acid-base indicators
all of the above
a standard solution
indicators
a compound whose colors are sensitive to pH
voltage difference between two electrodes in the meter's probe
a pH meter measures the pH of a solution by measuring the
pH meter
determines the pH of a solution by measuring the voltage between two electrodes that are placed in the solution
-log[OH-]
equation for pOH
-log[H3O+]
equation to calculate pH
50 mL
in th figure on the previous page, the volume of titration standard necessary to reach the equivalence point is
is 2:1
in the titration of a solution of Sr(OH)2 with HCl, the mole ratio of hydroxide ions to hydronium ions
titration
the controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration
a strong acid with a weak base
the figure above shows an example of the titration of
pH
the negative of the common logarithm of the hydronium ion concentration
pOH
the negative of the common logarithm of the hydroxide ion concentration
transition interval
the pH range over which an indicator changes color
equivalence point
the point at which the two solutions used in a titration are present in chemically equivalent amounts
end point
the point in a titration at which an indicator changes color
self ionization of water
two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton
strong base
what is KOH
2.5x10-12
what is the [H3O+] in a 0.0040 m solution of NaOH
1x10-13
what is the [OH-] of an aqueous solution in a 0.1 MHCl solution
1x10-8
what is the concentration of hydroxide ions in a solution that has a pH of 6.0
1x10-8
what is the concentration of hydroxide ions in a solution that has a pOH of 8.0
it shows that water is a strong electrolyte
which of the following is not true regarding the self ionization of water
