Consider the titration of 0.100 L of 0.200 M sulfurous acid (see
Ka/Kb table from table)...
Consider the titration of 0.100 L of 0.200 M sulfurous acid (see
Ka/Kb table from table) with 0.500 M NaOH. What is the pH at the
endpoint of the titration?
12. Consider the titration of 0.100 L of 0.200 M ascorbic acid
with 0.500 M NaOH. What is the pH at the endpoint of the titration?
Enter your answer to two decimal places; for this question we can
assume the 5% assumption is valid.
Consider the titration of 100.0 mL of 0.100 M H2NNH2
(Kb=3.0E-6) by 0.200 M HNO3. Calculate the pH of the resulting
solution after the following volumes of HNO3 have been added.
A) 0.0 mL
B) 20.0 mL
C) 25.0 mL
D) 40.0 mL
E) 50.0 mL
F) 100.0 mL
Consider the titration of 50.0 mL of 0.100 M HN3 (Ka=1.9X10^-5)
with 0.200 M CSOH. Calculate the PH after addition of
A) at initial point
B) 12.50 ml CSOH
C) 50.0 ml CSOH
D) 60.0 mL of CSOH
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka =
1.8 10-5) by 0.100 M KOH. Calculate the pH of the resulting
solution after 0.0mL of KOH has been added.
Consider the titration of a 12.0 mL solution containing 0.200
mol/L acetic acid (CH3COOH, Ka = 1.8 x 10-5 ), with a solution of
0.250 mol/L KOH. (12 points total) i) Determine the pH of the
solution when 4.80 mL of KOH has been added.
ii) Determine the pH of the solution when 14.00 mL of KOH has
been added.
Pertaining to the titration of 25.0mL of 0.100 M HCN
(Ka=6.2x10-10) with 0.200 M NaOH, calculate the pH at the following
points. a) initial pH, 0.0mL NaOH b) after the addition of 4.0mL
NaOH c) after the addition of 6.25 mL NaOH d) at the equivalence
point e) after the addition of 17.0 mL NaOH
Consider the titration of 100.0 mL of 0.400 M C5H5N by 0.200 M
HCl. (Kb for C5H5N = 1.7×10-9)
Part 1 Calculate the pH after 0.0 mL of HCl added.
pH =
Part 2 Calculate the pH after 35.0 mL of HCl added.
pH =
Part 3 Calculate the pH after 75.0 mL of HCl added.
pH =
Part 4 Calculate the pH at the equivalence point.
pH =
Part 5 Calculate the pH after 300.0 mL of HCl added....
Consider the titration of 100.0 mL of 0.400 M
C5H5N by 0.200 M HCl.
(Kb for C5H5N =
1.7×10-9)
Part 1
Calculate the pH after 0.0 mL of HCl added.
pH =
Part 2
Calculate the pH after 25.0 mL of HCl added.
pH =
Part 3
Calculate the pH after 75.0 mL of HCl added.
pH =
Part 4
Calculate the pH at the equivalence point.
pH =
Part 5
Calculate the pH after 300.0 mL of HCl added....
Consider the titration of 100.0 mL of 0.400 M
HONH2 by 0.200 M HCl.
(Kb for HONH2 = 1.1×10-8)
Part 1
Calculate the pH after 0.0 mL of HCl added.
pH =
Part 2
Calculate the pH after 40.0 mL of HCl added.
pH =
Part 3
Calculate the pH after 75.0 mL of HCl added.
pH =
Part 4
Calculate the pH at the equivalence point.
pH =
Part 5
Calculate the pH after 300.0 mL of HCl added....
Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M
KOH. Calculate the pH of the resulting solution after the following
volumes of KOH have been added. a. 0.0 mL d. 80.0 mL b. 10.0 mL e.
100.0 mL c. 40.0 mL
answers are A) 0.699 B) 0.854 C) 1.301 D) 7.00 E) 12.15 I would
just like to know how to do the work please and tbank you