Question
In: Chemistry
A buffer solution was prepared by mixing 516.9 mL of 0.25 M acetic acid and 103.8...
A buffer solution was prepared by mixing 516.9 mL of 0.25 M acetic acid and 103.8 mL of 0.89 M sodium acetate. Calculate the pH of the solution given that Ka is 1.8 x 10—5 . Answer in 2 decimal places.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A buffer solution is prepared by mixing 20.0 mL 0.45 M HAc (acetic acid) with 35.0...
A buffer solution is prepared by mixing 20.0 mL 0.45 M HAc
(acetic acid) with 35.0 mL 0.45 MNaAc (sodium acetate) (a) What is
the amount of 4.0 M HAc which must be added to this buffer solution
to double [H3O+]? (b) What is the amount of 2.0 M HCl that must be
added to decrease the pH by 0.50? (c) How much NaOH(s) in g has to
be added to the solution to raise the pH by 2.00?
A buffer solution is prepared by mixing 20.0 mL 0.45M HAc (acetic acid) with 35.0 mL...
A buffer solution is prepared by mixing 20.0 mL 0.45M HAc
(acetic acid) with 35.0 mL 0.45M NaAc (sodium acetate)
(a) What is the amount of 4.0M HAc which must be added to this
buffer solution to double [H3O+]?
(b) What is the amount of 2.0M HCl that must be added to
decrease the pH by 0.50?
(c) How much NaOH(s) in g has to be added to the solution to
raise the pH by 2.00?
Calculate the pH of a buffer solution prepared by mixing 20 mL of 5.0% acetic acid...
Calculate the pH of a buffer solution prepared by mixing 20 mL
of 5.0% acetic acid with 20 mL of 0.50 M NaOH and 100 mL of
water
A buffer solution is prepared by mixing 35mL of 0.18M CHCOOH (acetic acid) and 25mL of...
A buffer solution is prepared by mixing 35mL of 0.18M CHCOOH
(acetic acid) and 25mL of 0.23M NaCH3COO (sodium
acetate). Fine the change in pH when 5.0 mL of 0.12M HCl is
added.
Been stuck on this one for a while. If you can show step by step
that would help so much!
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M solution of hydroxylamine...
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M
solution of hydroxylamine (OHNH2, Kb = 1.1 × 10-8) and 250.0 mL of
a 0.300 M solution of its hydrochloride salt (OHNH3+ Cl- ).
Calculate the pH of the solution after the addition of 1.08 g of
solid NaOH (molar mass = 40.00 g/mol). Assume that there is no
volume change upon the addition of solid.
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M solution of hydroxylamine...
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M
solution of hydroxylamine (OHNH2, Kb = 1.1 ×
10-8) and 250.0 mL of a 0.300 M solution of its
hydrochloride salt (OHNH3+ Cl- ).
Calculate the pH of the solution after the addition of 1.08 g of
solid NaOH (molar mass = 40.00 g/mol). Assume that there is no
volume change upon the addition of solid.
A.
8.22
B.
5.55
C.
6.30
D.
5.78
A student creates a buffer mixing 50. mL of 1.0 M Acetic Acid with 25 mL...
A student creates a buffer mixing 50. mL of 1.0 M Acetic Acid with
25 mL of 1.0 M Sodium Hydroxide. The buffer is then mixed with 10.
mL of 2.0 M hydrobromic acid. What is the pH of the final
solution?
The Ka of acetic acid is 1.8 x
10-5
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.
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 280.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium...
A 280.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M
in sodium acetate. For acetic acid, Ka=1.8×10−5.
Part A) What is the initial pH of this solution?
Part B) What is the pH after addition of 0.0150 mol
of HCl?
Part C) What is the pH after addition of 0.0150 mol
of NaOH?
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