Question

Consider the titration of a 23.4 −mL sample of 0.125 M RbOH with 0.100 M HCl. Determine each of the following.

A) the initial pH

B) the volume of added acid required to reach the equivalence point

C) the pH at 5.3 mL of added acid

D) the pH at the equivalence point

E) the pH after adding 5.4 mL of acid beyond the equivalence point

Answer #1

Consider the titration of a 27.8 −mL sample of 0.125 M RbOH with
0.110 M HCl. Determine each of the following. A) the initial pH
B)the volume of added acid required to reach the equivalence point
C) the pH at 6.0 mL of added acid D) the pH at the equivalence
point E) the pH after adding 4.0 mL of acid beyond the equivalence
point

Consider the titration of a 26.9 −mL sample of 0.115 M RbOH with
0.100 M HCl. Determine each of the following. C. the pH at 5.1 mL
of added acid? D. the pH at the equivalence point? E. the pH after
adding 4.1 mL of acid beyond the equivalence point?

Consider the titration of a 26.9 −mL sample of 0.115 M RbOH with
0.100 M HCl. Determine each of the following.
A. the initial pH?
B. the volume of added acid required to reach the equivalence
point

Consider the titration of a 21.0 −mL sample of 0.100 M HC2H3O2
with 0.125 M NaOH. Determine each of the following.
A. the initial pH = 2.87
B. the volume of added base required to reach the equivalence
point = 16.8 mL
C. the pH at 6.00 mL of added
base = 4.49
D. the pH at one-half of the equivalence point =
4.74
F. the pH after adding
6.00 mL of base beyond the equivalence point.... I need help...

Consider the titration of a 26.0-mL sample of 0.170 M CH3NH2
with 0.145 M HBr. (The value of Kb for CH3NH2 is 4.4×10−4.)
Initial pH- 11.94
Volume of added acid required to reach the equivalence point:
30.5 mL
Determine the pH after adding 5.0 mL of acid beyond the
equivalence point.

Consider the titration of a 27.0 −mL sample of 0.175 MCH3NH2
with 0.150 M HBr. Express answers using two decimal places.
Determine each of the following.
A) the initial pH
B) the volume of added acid
required to reach the equivalence point
C) the pH at 6.0 mL of
added acid
D) the pH at one-half of the equivalence point
E) the pH at the equivalence point
F) the pH after adding 4.0 mL of acid beyond the equivalence
point

Consider the titration of a 26.0-mL sample of 0.180 M CH3NH2
with 0.145 M HBr. (The value of Kb for CH3NH2 is
4.4×10−4.)
Part A
Determine the initial pH.
Part B
Determine the volume of added acid required to reach the
equivalence point. answer to 3 sig figs
Part C
Determine the pH at 6.0 mL of added acid
Part D
Determine the pH at one-half of the equivalence point.
Part E
Determine the pH at the equivalence point.
Part...

Consider the titration of a 25.0 −mL sample of 0.180 M CH3NH2
with 0.155 M HBr. Determine each of the following.
a. the pH at one-half of the equivalence point
b. the pH at the equivalence point
c. the pH after adding 6.0 mL of acid beyond the equivalence
point
i already found that the initial pH is 11.95, the volume of acid
added to reach equivelance point is 29.0mL, and the pH og 6.0mL of
added acid is 11.23

Consider the titration of a 22.0-mL sample of 0.100 M HC2H3O2
with 0.125 M NaOH. (The value of Ka for HC2H3O2 is 1.8×10−5.)
Determine the pH at 4.0 mL of added base.Determine the pH at the
equivalence point.

Consider the titration of a 21.0 −mL sample of 0.100 M HC2H3O2
with 0.120 M NaOH. Determine each of the following.
the volume of added base required to reach the equivalence
point
the pH at the equivalence point

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