Question
In: Chemistry
A 150.0-mL solution contains 2.25 g of sodium benzoate and 2.83 g of benzoic acid. Calculate...
A 150.0-mL solution contains 2.25 g of sodium benzoate and 2.83 g of benzoic acid. Calculate the pH of the solution. For benzoic acid, Ka=6.5×10−5
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that...
What should the molar concentrations of benzoic acid and sodium
benzoate be in a solution that is buffered at a pH of 4.58 and has
a freezing point of -2.0 ∘C? (Assume complete dissociation of
sodium benzoate and a density of 1.01 g/mL for the solution.)
What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that...
What should the molar concentrations of benzoic acid and sodium
benzoate be in a solution that is buffered at a pH of 4.78 and has
a freezing point of -2.0 ∘C? (Assume complete dissociation of
sodium benzoate and a density of 1.01 g/mL for the solution.)
What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that...
What should the molar concentrations of benzoic acid and sodium
benzoate be in a solution that is buffered at a pH of 4.78 and has
a freezing point of -2.0 ∘C? (Assume complete dissociation of
sodium benzoate and a density of 1.01 g/mL for the solution.)
Express your answers using two significant figures separated by
a comma.
answer is not 0.11 and 0.44
answer is not 0.11 and 0.45
answer is not 0.11 and 0.46
Textbook says Tf is 1.86...
What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that...
What should the molar concentrations of benzoic acid and sodium
benzoate be in a solution that is buffered at a pH of 4.86 and has
a freezing point of -2.0 ∘ C ? (Assume complete dissociation of
sodium benzoate and a density of 1.01 g/mL for the solution.)
Calculate the pH of a 0.01 M solution of sodium benzoate. A: Dissociation constant of benzoic...
Calculate the pH of a 0.01 M solution of sodium benzoate.
A: Dissociation constant of benzoic acid.
B: Calculate the hydrolysis constant of sodium benzoate.
C: Calculate the pH of the 0.01 M solution.
A buffer solution is prepared by dissolving 1.50 g each of sodium benzoate, C6H5COONa, and benzoic...
A buffer solution is prepared by dissolving 1.50 g each of
sodium benzoate, C6H5COONa, and benzoic acid, C6H5COOH (Ka = 6.45 ×
10-5), in 150.0 mL of solution. The molar mass of benzoic acid is
122.12 g/mol and that of sodium benzoate is 144.10 g/mol.
a) What is the pH of this buffer solution?
b) Which buffer component must be added to change the pH to
4.00? What mass of that component is required?
c) What volume of 2.0 M...
What mass (in grams) of sodium benzoate must be added to 150.0 mL of a 0.14...
What mass (in grams) of sodium benzoate must be added to 150.0
mL of a 0.14 M benzoic acid solution in order to obtain a buffer
with a pH of 4.25? The molecular weight of sodium benzoate is
144.11g/mol. The Ka of benzoic acid is 6.46x10^-5. Be sure to
include proper units in your answer to two significant figures.
Benzoic acid is a weak acid that has antimicrobial properties. Its sodium salt, sodium benzoate, is...
Benzoic acid is a weak acid that has antimicrobial properties.
Its sodium salt, sodium benzoate, is a preservative found in foods,
medications, and personal hygiene products. Benzoic acid ionizes in
water:
C6H5COOH⇌C6H5COO−+H+
The pKa of this reaction is 4.2. In a 0.57 M
solution of benzoic acid, what percentage of the molecules are
ionized?
Express your answer to two significant figures and include the
appropriate units.
Calculate the pH in 0.050 M sodium benzoate; Ka for benzoic acid (C6H5CO2H) is 6.5×10−5.
Calculate the pH in 0.050 M sodium benzoate; Ka for
benzoic acid (C6H5CO2H) is 6.5×10−5.
What is the pH of a buffer containing 20.53g benzoic acid and 17.23g sodium benzoate in...
What is the pH of a buffer containing 20.53g benzoic acid and
17.23g sodium benzoate in 500mL of solution?
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