A 1.0-L buffer solution contains 0.100 molHC2H3O2 and 0.100
molNaC2H3O2. The value of Ka for HC2H3O2...
A 1.0-L buffer solution contains 0.100 molHC2H3O2 and 0.100
molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5 Calculate the
pH of the solution upon addition of 39.8 mL of 1.00 MHCl to the
original buffer.
0.2 mol of gaseous HCl is added to 1.0 L of a buffer solution
that contains 3.0 M CH3COOH and 3.0 M
CH3COONa. What is the pH of the solution? Assume that
Ka for CH3COOH is 10-5. Assume
also that the volume of the solution does not change when the HCl
is added.
Type your answer in decimal number carrying only one digit after
decimal. So you must round up or down at the second digit after
decimal.
For example,...
For the next three problems, consider 1.0 L of a solution which
is 0.6 M HC2H3O2 and 0.2 M
NaC2H3O2 (Ka for
HC2H3O2 = 1.8 x 10-5).
Assume 2 significant figures in all of the given concentrations so
that you should calculate all of the following pH values to two
decimal places.
1. Calculate the pH of this solution.
2. Calculate the pH after 0.10 mol of HCl has been added to the
original solution. Assume no volume change on...
Part A
Calculate the pH of 0.100 L of a buffer solution that is 0.27 M
in HF and 0.47 M in NaF.
Express your answer using three significant figures.
pH =
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Part B
Calculate pH of the solution on addition of the following.
0.004 mol of HNO3
Express your answer using three significant figures.
pH =
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Part C
Calculate pH of the solution on addition of the following.
0.005 mol of KOH
Express...
A) Calculate the pH of a buffer that is 0.225M
HC2H3O2 and 0.162M
KC2H3O. The Ka for
HC2H3O2 is 1.8x10-5
B) A 1.00L buffer solution is 0.250M in HF and
0.250M in NaF. Calculate the pH of the solution after the addition
of 0.100 moles of solid NaOh. Assume no volume chane uon the
addition of base. Ka for HF= 3.5x10-4
C) A 100.0ml sample of 0.20M HF is
titrated with 0.10M KOH. Determine the pH of the solution after...
A 1.0 L of a buffer solution is created which is 0.363 M in
hydrocyanic acid, HCN, and 0.303 M sodium cyanate, NaCN.
Ka for HCN = 4.0 x 10-10.
What is the pH after 0.089 mol of HCl is added to the buffer
solution?
A 1.0-L buffer solution is 0.135 M in HNO2 and 0.195
M in NaNO2.
Part A
Determine the concentrations of HNO2 and NaNO2 after addition of
1.3 g HCl.
Express your answers using three significant figures separated
by a comma.
[HNO2], [NaNO2] =
M
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Part B
Determine the concentrations of HNO2 and NaNO2 after addition of
1.3 g NaOH.
Express your answers using three significant figures separated
by a comma.
[HNO2], [NaNO2] =
M
Part C
Determine...
if 0.050 mol of hcl is added to 1.0 l of buffer solution
containing 0.125 M potassium acetate and 0.10 M acetic acid what is
the change in PH of the solution
What is the pH of a 1.0 L buffer solution containing 0.370 M
acetic acid and 0.361 M sodium acetate after you’ve added 0.095
moles of potassium hydroxide?