Question
In: Chemistry
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.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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. What is the pH of the buffer prepared by mixing 250. mL of 0.200 M...
a. What is the pH of the buffer prepared by mixing 250. mL of
0.200 M benzoic acid and 100. mL of 0.250M NaOH? pKa=4.19
b. A buffer containing 1.00 M concentrations of HOAc and NaOAc
has a pH of 4.742. (a) What is the pH of the soln’ after 0.0100 mol
of HCl has been added to 1.00 L of the buffer? (b) What is the pH
of the soln’ after the addition of 0.0100 mol of NaOH? (c)...
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
A buffer is prepared by adding 300.0 mL of 0.050 M Ch3COONa to a 500.0 mL...
A buffer is prepared by adding 300.0 mL of 0.050 M Ch3COONa to a
500.0 mL of 0.100 M CH3COOH. What is the pH of this buffer?
Ka=1.8x10^-5
What is the pH of the buffer upon the addition of 10.0 mL of a
1.2x10^-3 M HCl solution?
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.
a) What is the pH of a buffer solution prepared by mixing 120 mL of a...
a) What is the pH of a buffer solution prepared by mixing 120 mL
of a 0.435 M CH3CO2H with 50 mL of a .286 M
CH3CO2Na solution?
CH3CO2H Ka = 1.75 x
10-5
b) What is the resulting pH if we add 10.2 mL of a .513 M HCl
solution to this buffer? Does the pH make sense? Why/why not?
c) What is the resulting pH if we add 3.56 mL of a 0.420 M NaOH
solution to the...
A 300.0 mL buffer solution is 0.230 M in acetic acid and 0.230 M in sodium...
A 300.0 mL buffer solution is 0.230 M in acetic acid and 0.230 M
in sodium acetate.
Part A: What is the initial pH of this solution?
Part B: What is the pH after addition of 0.0050 mol of HCl?
Part C: What is the pH after addition of 0.0050 mol of NaOH?
A 300.0 mL buffer solution is 0.220 M in acetic acid and 0.220 M in sodium...
A 300.0 mL buffer solution is 0.220 M in acetic acid
and 0.220 M in sodium acetate.
What is the initial pH of this solution?
What is the pH after addition of 0.0100 mol of HCl?
What is the pH after addition of 0.0100 mol of NaOH?
Please explain I don't understand how to do this.
thank you!
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?
1. Determine the pH of the buffer solution that is prepared by mixing 259 mL of...
1. Determine the pH of the buffer solution that is prepared by
mixing 259 mL of 0.0983 M BIS−TRIS propane−H (C11H27N2O6+ ) to 855
mL of 0.0729 M BIS-TRIS_propane (C11H26N2O6) ). Assume the 5%
approximation is valid. Report your answer to 2 decimal places. The
pKa of BIS−TRIS propane−H is 9.10. Submit Answer Tries 0/3 2.
Determine the pH of the BIS−TRIS propane−H/BIS−TRIS propane buffer
solution after the addition of 25.2 mL of 0.643 M solution of
rubidium hydroxide to...
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