Question
In: Chemistry
Suppose you have 500. mL of a solution of 0.200 M sodium benzoate (C6H5CO2Na), to which...
Suppose you have 500. mL of a solution of 0.200 M sodium benzoate (C6H5CO2Na), to which you add 100. mL of a 0.400 M HCl solution. After the resulting mixture has reached equilibrium, what is the pH of this solution? Ka of benzoic acid (C6H5CO2H) = 6.3 x 10−5 at 25°C.
Suppose you have 500. mL of a solution of 0.200 M sodium benzoate (C6H5CO2Na), to which you add 100. mL of a 0.400 M HCl solution. After the resulting mixture has reached equilibrium, you add an additional 50.0 mL of the 0.400 M HCl solution into the solution and allow it to re-establish equilibrium. What is the pH of the solution now? Ka of benzoic acid (C6H5CO2H) = 6.3 x 10−5 at 25°C. (1) 2.98 (2) 3.57 (3) 3.80 (4) 4.02 (5) 4.90
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
25.0 mL of 0.200 M solution of HBr are mixed with 25.0 mL of 0.200 M...
25.0 mL of 0.200 M solution of HBr are mixed with 25.0 mL of
0.200 M solution of NaOH in a constant pressure calorimeter. The
temperature increases from 23.00 °C to 24.37 °C. Assume that the
specific heat of the solution is the same as that of pure water
(4.18 J/(g•°C)) and that the density is the same as pure water
(1.00 g/mL). Calculate ΔH per mole of reaction for the below
chemical reaction.
HBr (aq) + NaOH (aq) →...
Part A A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric...
Part A
A 50.0-mL sample of 0.200 M sodium hydroxide is
titrated with 0.200 M nitric acid.
Calculate the pH of the solution, after you add a total of 51.9
mL 0.200 M HNO3.
Express your answer using two decimal places.
Part B
A 39.0
mL
sample of 0.146
M
HNO2
is titrated with 0.300
M
KOH.
(Ka
for
HNO2
is 4.57×10−4.)
Determine the pH at the
equivalence point for the titration of
HNO2
and
KOH
.
Assuming that you start with 2.00 g of sodium benzoate and 5 mL of 3 M...
Assuming that you start with 2.00 g of sodium benzoate and 5 mL
of 3 M HCl, how many molar equivalents of HCl are you using? Use
two decimal places.
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution....
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e)
15.0 mL. (25 points)
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution....
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e)
15.0 mL. (25 points)
For the titration of 40.0 mL of 0.200 M acetic acid with 0.150 M sodium hydroxide,...
For the titration of 40.0 mL of 0.200 M acetic acid with 0.150 M
sodium hydroxide, determine the pH when:
(a) 40.0 mL of base has been added.
(b) 53.3 mL of base has been added.
(c) 66.6 mL of base has been added.
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.
You are asked to prepare 500. mL of a 0.200 M acetate buffer at pH 5.10...
You are asked to prepare 500. mL of a 0.200 M acetate buffer at
pH 5.10 using only pure acetic acid (MW=60.05 g/mol, pKa=4.76),
3.00 M NaOH, and water. Answer the following questions regarding
the preparation of the buffer. What volume of 3.00 M NaOH must you
add to the acetic acid to achieve a buffer with a pH of 5.10 at a
final volume of 500 mL?
A solution is prepared by mixing 150.0 mL of 0.200 M Mg2+ and 250.0 mL of...
A solution is prepared by mixing 150.0 mL of 0.200 M Mg2+ and
250.0 mL of 0.100 M F-. A precipitate forms. Calculate the
concentrations of Mg2+ and F- at equilibrium. Ksp = 6.4 × 10-9
What mass of sodium benzoate should be added to 160.0 mL of a 0.13 M benzoic...
What mass of sodium benzoate should be added to 160.0 mL of a
0.13 M benzoic acid solution in order to obtain a buffer with a
pH of 4.25?
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