Question

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 KNO_{2}.

b. adding Mg(NO_{3})_{2}

c. adding HCl.

d. adding NH_{4}NO_{3}.

e. adding HNO_{2}.

Answer #1

This is a buffer so:

pH = pKA + log(conjugate/acid)

conjugate = NO-2

acid = HNO2

a. adding KNO2. --> adding KNO2; will increase conjugate, therefore, changes log(ratio) which finally changes pH; this is not an answer

**b. adding Mg(NO3)2--> since NO3- is not the same as
NO2-**

c. adding HCl. --> produces more acid from the conjugate; will change pH

d. adding NH4NO3. since NO3- is not the same as NO2-; ithis could be an answer but NH4+ in solution will interact as a base/acid therefore, will mofdify pH

e. adding HNO2. --> increases direclty acid concentration

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

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.

Calculate the pH of a 1-L solution containing 0.150 mole of
CH3COOH and 0.100 mole of HCl.

Calculate the change in pH that results from adding 0.200 mol
NaNO2 to 1.00 L of 0.200 M HNO2(aq). (Ka(HNO2)=7.2⋅10−4)

Calculate the pH after 0.15 mole of NaOH is added to 1.05 L of a
solution that is 0.48 M HNO2 and 1.06
M LiNO2, and calculate the pH after 0.30 mole
of HCl is added to 1.05 L of the same solution of HNO2
and LiNO2. ka of hno2 is 4.5 x 10^-4

Calculate the pH of the buffer solution (1.00 M HNO2
and 1.00 M NaNO2) after 0.20 mol of NaOH is added to 1.00 L of
buffer solution (Ka = 4.0 x 10^-4)

Determine the pH of the following solution:
A 1.0 L of an aqueous solution containing 3.0 grams of HBr and
7.0 mL of 1.0 M NaOH.

Calculate the pH of 300 mL of a 0.30 M aqueous solution of
sodium nitrite (NaNO2) at 25 °C given that the Ka of nitrous acid
(HNO2) is 4.5×10-4.
A) 5.59
B) 8.41 (Correct Answer)
C) 4.46
D) 7.00
E) 12.87

To a 1.00 L buffer solution made of 1.65 M nitrous acid (HNO2)
and 1.01M potassium nitrite (KNO2) was added 0.625 moles of NaOH
(assume no volume change to the solution). What is the final pH of
this buffer assuming Ka nitrous acid = 4.00e-4

Calculate the pH of a 1 L solution that contains 1.0 M HCl and
1.5 M CH3COOK. The Ka for CH3COOH
is 1.8 x 10-5.
9.56
b)
4.74
c)
4.44
d)
0.30
e) 7.45

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