Question
In: Chemistry
Calculate the conjugate base to acid ratio in the solution. Calculate the theoretical pH. Solution: 10.00...
Calculate the conjugate base to acid ratio in the solution. Calculate the theoretical pH. Solution: 10.00 ml of .2M acetic acid and 1.00 mL of .1 M sodium hydroxide and 9.00 mL distilled water
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
The pH of a 0.392 M solution of the conjugate base, A-, of a weak acid,...
The pH of a 0.392 M solution of the conjugate
base, A-, of a weak acid, HA, is 11.60. What is
the Kb for A-?
Please show work
Calculate the conjugate base to acid ratio in Solution D (10 mL of 0.2 M acetic...
Calculate the conjugate base to acid ratio in Solution D (10 mL
of 0.2 M acetic acid and 1 mL of 0.1 M sodium hydroxide, and 9 mL
distilled water). Then calculate the theoretical pH.
Initial pH: 3.47
Molarity of HCl:
0.0992 about 0.3 mL
added
pH after HCl addition: 3.09
Molarity of added NaOH:
0.0997M about 0.2
mL
added
pH after NaOH addition: 3.54
For an acid-conjugate base pair, when the pH is qual to the pKa, the following is...
For an acid-conjugate base pair, when the pH is qual to the pKa,
the following is true;
a. The acid concentration is the same as that of the conjugate
base.
b. The acid concentration is twice that of the conjugate
base.
c. There is only one species present in solution.
d. A and C
e. None of the above
1. The conjugate base of a stong acid has no effect on the pH. Why or...
1. The conjugate base of a stong acid has no effect on the pH.
Why or why not? Include a comment on the conjugate acid of a
base.
2. Given the discussion of question one above, then if I were to
dissolve the following salt, KNO3, in water, what would
the resulting pH be and why?
Calculation of Molar Ratios of Conjugate Base to Weak Acid from pH For a weak acid...
Calculation of Molar Ratios of Conjugate Base to Weak
Acid from pH For a weak acid with a pKa of 6.0, calculate
the ratio of conjugate base to acid at a pH of 5.0.
Choice of Weak Acid for a Buffer Which of these
com-pounds would be the best buffer at pH 5.0: formic acid (pKa 5
3.8), acetic acid (pKa 5 4.76), or ethylamine (pKa 5 9.0)? Briefly
justify your answer.
please show work thank you will rate.
Conjugate Acid-Base Pairs: a.) The formula for the conjugate base of H2C2O4 is _____________. b.) The...
Conjugate Acid-Base Pairs:
a.) The formula for the conjugate base of
H2C2O4 is _____________.
b.) The formula for the conjugate acid of
HCO3- is ______________.
c.) The formula for the conjugate acid of
C2O42_ is ______________.
d.) The formula for the conjugate acid of
HPO42_ is ______________.
e.) The formula for the conjugate base of
HCO3- is ______________.
f.) The formula for the conjugate acid of
HSO3- is _______________.
Conjugate Acid-Base Pairs: a.) The formula for the conjugate base of H2C2O4 is _____________. b.) The...
Conjugate Acid-Base Pairs:
a.) The formula for the conjugate base of
H2C2O4 is _____________.
b.) The formula for the conjugate acid of
HCO3- is ______________.
c.) The formula for the conjugate acid of
C2O42_ is ______________.
d.) The formula for the conjugate acid of
HPO42_ is ______________.
e.) The formula for the conjugate base of
HCO3- is ______________.
f.) The formula for the conjugate acid of
HSO3- is _______________.
Identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid and the conjugate base for each...
Identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the
conjugate acid and the conjugate base for each of the following
reactions.
1. H2CO3(aq) + H2O+(aq) <-----> H3O+(aq) + HCO3-(aq)
2. NH3(aq) + H2O(l) <-----> NH4+ (aq) + OH -(aq)
3. HNO3 (aq) <-----> H2O(l) H3O+(aq) + NO3- (aq)
4. C5H5N (aq) + H2O(l) <-----> C5H5NH+(aq) + OH- (aq)
12. In a solution, when the concentrations of a weak acid and its conjugate base are...
12. In a solution, when the concentrations of a weak
acid and its conjugate base are equal,….
[A] the system is not at equilibrium
[B] the -log of the [H+] and the -log of the
Ka are equal
[C] the buffering capacity is significantly decreased
[D] the buffering capacity is significantly increased
[E] All of the above are true.
13. The concentration of iodide ions in a saturated solution of
lead (II) iodide is ________ M.
The solubility product constant...
Identify the acid and conjugate base in each reaction. Calculate the pKA for each acid. List...
Identify the acid and conjugate base in each reaction. Calculate
the pKA for each acid. List them in order from
the strongest to weakest acid.
HC2H3O2 + H2O -->
H3O+ +
C2H3O2-,
KA = 1.7 x 10-5
HC7H5O2 + H2O -->
H3O+ +
C7H5O2-,
KA = 6.3 x 10-5
HC6H4NO2+H2O -->
H3O+ +
C6H4NO2-,
KA = 1.4 x 10-5
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