Question
In: Chemistry
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 moles of nitric
acid will:
(Assume that the volume does not change upon the addition of
nitric 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
Multiple choices can be selected for the answer, could you also explain how this is done?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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...
A 1 liter solution contains 0.382 M hydrofluoric acid and 0.509 M sodium fluoride. Addition of...
A 1 liter solution contains 0.382 M hydrofluoric acid and 0.509
M sodium fluoride. Addition of 0.191 moles of sodium hydroxide
will: (Assume that the volume does not change upon the addition of
sodium hydroxide.) 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 0.436 M hypochlorous acid and 0.581 M sodium hypochlorite. Addition of...
A 1 liter solution contains 0.436 M
hypochlorous acid and 0.581 M
sodium hypochlorite.
Addition of 0.109 moles of barium
hydroxide will:
(Assume that the volume does not change upon the addition of
barium hydroxide.)
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 0.460 M
hydrofluoric acid and 0.345 M
potassium fluoride.
Addition of 0.380...
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...
In the solution containing both 0.10 M acetic acid and 0.10 M sodium acetate, the acetic...
In the solution containing both 0.10 M acetic acid and 0.10 M
sodium acetate, the acetic acid undergoes ionization. The chemical
equation for this ionization reaction is the same as for a solution
containing acetic acid alone. The difference is that the initial
concentration of acetate ion (before any ionization reaction
occurs) for the solution containing acetic acid alone is zero,
whereas the initial concentration of acetate ion is 0.10 M in your
solution containing both acetic acid and sodium...
A solution contains 1.5M sodium acetate. The pKa of acetic acid (a weak acid) is 4.76....
A solution contains 1.5M sodium acetate. The pKa of acetic acid
(a weak acid) is 4.76. Calculate the fraction and
percentage of the molecules existing in the
unionized state.
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.
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...
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