Question

A 1.0-L buffer solution is 0.125 M in HNO2 and 0.190 M in NaNO2.

a) Determine the concentrations of HNO2 and NaNO2 after addition of 1.9 g HCl.

b) Determine the concentrations of HNO2 and NaNO2 after addition of 1.9 g NaOH.

c) Determine the concentrations of HNO2 and NaNO2 after addition of 1.9 g HI

Answer #1

A 1.0 L buffer of 0.125 M HNO2 (weak acid) and 0.190 M NaNO2 (conjugate base of wek acid)

a) after HCl = 1.9 g/36.5 g/mol = 0.052 mol was added

new concentration [HNO2] = (0.125 M x 1 L + 0.052 mol)/1 L = 0.177 M

new concentration [NaNO2] = (0.190 M x 1 L - 0.052 mol)/1 L = 0.138 M

b) after NaOH = 1.9 g/40 g/mol = 0.0475 mol was added

new concentration [HNO2] = (0.125 M x 1 L - 0.0475 mol)/1 L = 0.0775 M

new concentration [NaNO2] = (0.190 M x 1 L + 0.0475 mol)/1 L = 0.2375 M

c) after Hl = 1.9 g/127.911 g/mol = 0.015 mol was added

new concentration [HNO2] = (0.125 M x 1 L + 0.015 mol)/1 L = 0.140 M

new concentration [NaNO2] = (0.190 M x 1 L - 0.015 mol)/1 L = 0.175 M

A 1.0-L buffer solution is 0.110 M in HNO2 and 0.165 M in
NaNO2.
Part A
Determine the concentrations of HNO2 and NaNO2 after addition of
1.1 g HCl.
Part B
Determine the concentrations of HNO2 and NaNO2 after addition of
1.1 g NaOH.
Part C
Determine the concentrations of HNO2 and NaNO2 after addition of
1.1 g HI.

1) A buffer contains significant amounts of ammonia and ammonium
chloride.
Part A
Write an equation showing how this buffer neutralizes added acid
(HI).
Express your answer as a chemical equation.
Part B
Write an equation showing how this buffer neutralizes added base
(CsOH).
Express your answer as a chemical equation.
2)
Calculate the ratio of CH3NH2 to CH3NH3Cl required to create a
buffer with pH = 10.20.
Express your answer using two significant figures.
3) A 1.0-L buffer solution...

The pH of a solution containing 2.0 mole HNO2 and 2.0 mole NaNO2
in 1.0 L of solution will not change by:
a. adding KNO2.
b. adding Mg(NO3)2
c. adding HCl.
d. adding NH4NO3.
e. adding HNO2.

1.00 mL of 12.0 M HCl is added to 1.00 L of a buffer that is
0.130 M HNO2 and 0.200 M NaNO2. How many moles of
HNO2 and NaNO2 remain in solution after addition of the HCl?
moles HNO2 =
moles NaNO2 =

Calculate the pH of 1.00 L of a buffer that is 0.120 M HNO2 and
0.150 M NaNO2.
then, Calculate the pH of the buffer described above after the
addition of 1.00 mL of 12.0 M HCl.

1.00 mL of 12.0 M HCl is added to 1.00 L of a buffer that is
0.120 M HNO2 and 0.180 M NaNO2. How many moles of HNO2 and NaNO2
remain in solution after addition of the HCl?

1.00 mL of 12.0 M HCl is added to 1.00 L of a buffer that is
0.100 M HNO2 and .190 M NaNO2. How many moles of HNO2 and NaNO2
remain in solution after of the HCl

Part A
Consider a buffer solution that is 0.50 M in NH3 and
0.20 M in NH4Cl. For ammonia, pKb=4.75.
Calculate the pH of 1.0 L of the original buffer, upon addition
of 0.190 mol of solid NaOH.
Part B
A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100
mol NaC2H3O2. The value of Ka for HC2H3O2 is
1.8×10−5.
Calculate the pH of the solution, upon addition of 0.030 mol of
NaOH to the original buffer.
(I will leave...

For the next three problems, consider 1.0 L of a solution which
is 0.3 M NH4Cl and 0.2 M NH3 (Ka for NH4Cl = 5.6 x 10-10). 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...

Does the pH increase, decrease, remain the same of the following
buffer solution, 1.0 L of 1.0 M HA and 1.0 M A−, on addition of
each of the following?
-A.B.C.
Addition of 0.05 mol HCl
Read Answer Items for Question 1
-A.B.C.
Addition of 0.05 mol NaOH
Read Answer Items for Question 1
-A.B.C.
Addition of 0.05 mol NaCl
Read Answer Items for Question 1
-A.B.C.
Addition of 0.0005 mol NaOH
A.
Remain the same
B.
Decrease
C.
Increase

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