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The amount of acid or base that a buffer can neutralizze is called
[H3O+] > [OH-]
a standard base
blood.
the buffer capacity.
perform an acid-base titration.
acid-base indicator.
change the pH.
excess acid.
A common example of a good buffer solution is
[H3O+] > [OH-]
a standard base
blood.
the buffer capacity.
perform an acid-base titration.
acid-base indicator.
change the pH.
excess acid.
To determine the concentration of an unknown acid or base in a titration, you need a(n)
[H3O+] > [OH-]
a standard base
blood.
the buffer capacity.
perform an acid-base titration.
acid-base indicator.
change the pH.
excess acid.
The carbonic acid-bicarbonate buffer sstem in blood has a 1:20 ratio of acid to conjugate base. Thie means it has a great capacity for neutralizing
[H3O+] > [OH-]
a standard base
blood.
the buffer capacity.
perform an acid-base titration.
acid-base indicator.
change the pH.
excess acid.
If hydronium ions or hydroxide ions are added beyond the buffer capacity, the added excess ions will
[H3O+] > [OH-]
a standard base
blood.
the buffer capacity.
perform an acid-base titration.
acid-base indicator.
change the pH.
excess acid.
For a water solution to be acidic, what must be true?
[H3O+] > [OH-]
a standard base
blood.
the buffer capacity.
perform an acid-base titration.
acid-base indicator.
change the pH.
excess acid.
How can you determine the concentration of a water solution of a weak acid?
[H3O+] > [OH-]
a standard base
blood.
the buffer capacity.
perform an acid-base titration.
acid-base indicator.
change the pH.
excess acid.
To determine the concentration of an unknown acid, one of the requirements is
[H3O+] > [OH-]
a standard base
blood.
the buffer capacity.
perform an acid-base titration.
acid-base indicator.
change the pH.
excess acid.
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