Question
In: Chemistry
A solution contains 0.003Mof sodium phenobarbital together with a buffer consisting of 0.20 M sodium acetate...
A solution contains 0.003Mof sodium phenobarbital together with a buffer consisting of 0.20 M sodium acetate and 0.30 M acetic acid. Acetic acid is a weak electrolyte; its degree, or fraction, of dissociation, α, at this concentration is 0.008 and the undissociated species do not contribute to the ionic strength. What is the ionic strength of the solution?
pka for acetic acid = 4.8
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared....
A buffer solution that is 0.10 M sodium acetate and 0.20 M
acetic acid is prepared. Calculate the initial pH of this
solution.
The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2
decimal places.
A buffered solution resists a change in
pH.
Calculate the pH when 21.1 mL of 0.031 M HCl is added to 100.0 mL
of the above buffer.
A buffer solution is 0.20 M in acetic acid and sodium acetate. Calculate the change in...
A buffer solution is 0.20 M in acetic acid and sodium acetate.
Calculate the change in pH upon adding 1.0mL of 0.10 M HCL to 10mL
of this solution.
2. A buffer solution contains .120 M acetic acid and .150 M sodium acetate. (a) how...
2. A buffer solution contains .120 M acetic acid and .150 M
sodium acetate.
(a) how many moles of each component are in 50.0 mL of
solution?
(b) If you add 5.55 mL of .092 M NaOH to the solution in part
(a), how many moles of acetic acid, sodium acetate, and NaOH will
be present after the reaction?
(c) If you add .50 mL of .087 M HCl to the solution in part (a)
how many moles of acetic...
2. A buffer solution contains .120 M acetic acid and .150 M sodium acetate. (a) how...
2. A buffer solution contains .120 M acetic acid and .150 M
sodium acetate.
(a) how many moles of each component are in 50.0 mL of
solution?
(b) If you add 5.55 mL of .092 M NaOH to the solution in part
(a), how many moles of acetic acid, sodium acetate, and NaOH will
be present after the reaction?
(c) If you add .50 mL of .087 M HCl to the solution in part (a)
how many moles of acetic...
You are preparing a buffer consisting of acetic acid and sodium acetate with a total of...
You are preparing a buffer consisting of acetic acid and sodium
acetate with a total of acetic acid and sodium acetate
concentration of 250 mM and a PH of 5.0. What concentration of
acetic acid and sodium acetate should you use?
1. A buffer solution consists of 0.25 M acetic acid (CH3COOH) and 0.10 M sodium acetate...
1. A buffer solution consists of 0.25 M acetic acid (CH3COOH)
and 0.10 M sodium acetate (CH3COONa). The Ka of acetic acid is
1.8×10−5. a. Calculate the equilibrium pH using the equilibrium
mass action expression.
b. Calculate the equilibrium pH using the Henderson-Hasselbalch
equation approach.
2. Consider a buffer solution that consists of both benzoic acid
(C6H5COOH) and sodium benzoate (C6H5COONa) and has a pH of 4.18.
The concentration of benzoic acid is 0.40 M. The pKa of benzoic
acid...
A 250.00 mL buffer solution is 0.250 M acetic acid (CH3COOH) and 0.100 M sodium acetate...
A 250.00 mL buffer solution is 0.250 M acetic acid (CH3COOH) and
0.100 M sodium acetate (NaCH3COO). The Ka of acetic acid is 1.8 •
10-5 at 25 o C. Calculate the pH of the resulting buffer solution
when 10.00 mL of a 0.500 M aqueous HCl solution is added to this
mixture.
A 1 liter solution contains 0.487 M acetic acid and 0.365 M sodium acetate. Addition of...
A 1 liter solution contains 0.487 M
acetic acid and 0.365 M
sodium acetate.
Addition of 0.183 moles of hydrobromic
acid will:
(Assume that the volume does not change upon the addition of
hydrobromic acid.)
Raise the pH slightly
Lower the pH slightly
Raise the pH by several units
Lower the pH by several units
Not change the pH
Exceed the buffer capacity
A 1 liter solution contains 0.474 M
hydrocyanic acid and 0.356 M
potassium cyanide.
Addition of 0.391...
1. A 1.00 liter solution contains 0.38 M acetic acid and 0.49 M sodium acetate. If...
1. A 1.00 liter solution contains
0.38 M acetic acid and
0.49 M sodium acetate.
If 0.120 moles of calcium
hydroxide are added to this system, indicate whether the
following statements are true or false.
(Assume that the volume does not change upon the addition of
calcium hydroxide.)
A. The number of moles of
CH3COOH will remain the
same.
B. The number of moles of
CH3COO- will
decrease.
C. The equilibrium concentration of
H3O+ will decrease.
D. The pH will...
Consider a buffer solution that contains 0.50 M NaH2PO4 and 0.20 M Na2HPO4. pKa(H2PO4-)=7.21. a) Calculate...
Consider a buffer solution that contains 0.50 M NaH2PO4 and 0.20
M Na2HPO4. pKa(H2PO4-)=7.21. a) Calculate the pH. b)Calculate the
change in pH if 0.120 g of solid NaOH is added to 150 mL of this
solution. c) If the acceptable buffer range of the solution is
±0.10 pH units, calculate how many moles of H3O+ can be neutralized
by 250 mL of the initial buffer.
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