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 upon addition of 0.050 mol of solid NaOH
to the original buffer solution.
Calculate the ph of a solution that is 0.30 M in ammonia (NH3) and
0.20 M in ammonium chloride. Kb=1.76 x 10^-5
Then calculate the ph if you add 10 mL of 1.0 M HCl to 50 mL
of your solution in the problem above.
The pH of a 0.50 M solution of ethylamine CH3CH2NH2 is 12.22.
Calculate the Kb of ethylamine. Use “E” for scientific
notation.
A 0.050 M solution of pyruvic acid, an intermediate in
metabolism, has a pH of 1.93. Calculate Ka for pyruvic acid, a weak
monoprotic acid. Use “E” for scientific notation.
Calculate the pH of a 0.17 M solution of HClO, with Ka1=
3.5x10.
At 25°C, 2.29E0 grams of sodium hydroxide is dissolved in
enough water to make 500....
titration of 50.0mL 0.50M NH3 with 0.50 M HCL.
Kb(NH3)=1.8x10^-5
Plot the pH of the solution after the addition of the following
volumes of HCL using ICE tables.
0.00mL, 10.00mL, 20.0mL, 25.0mL, 30.0mL, 40.0mL, 50.0mL,,
60.0mL
Calculate the pH of the 0.250 M NH3/0.5 M NH4Cl buffer system. What
is the pH after the addition of 2.0 mL of 0.250 M NaOH to 18.0 mL
of the buffer solution? After adding 10 more mL of 0.25 M NaOH what
is the pH?
If some NH4Cl is added to an aqueous solution of NH3:
A.
the pH of the solution will decrease
B.
the solution will not have pH
C.
NH4Cl cannot be added to NH3
D.
the pH of the solution will increase
E.
the pH of the solution will not change
What is the pH of a solution that is composed of 0.20 moles of
HCN and 0.035 moles of NaCN dissolved in enough water to make
1.00L? Ka(HCN)= 4.9 x 10^-10.
a. Calculate the pH of a buffer solution that contains 0.50 M
CH3COOH and 0.70 M NaCH3COO
b. What is the mximum number of moles of H+ that can be absorbed
by 100 mL of buffer given in the previous question
c. Write the net ionic equation for the reaction of H+ wiht the
buffer component