Question

eight

Consider the titration of a 35.0ml sample of 0.175 M HBr with .205M KOH. Determine the following.

**partA** the initial pH **express answer
using three decimal places**

**PartB** the volume of added base required to
reach the equivalence point **express answer in
millimeters**

**PartC** the pH at 11.9mL of added base
**express answer using three decimal places**

**PartD** the pH at the equilalence point
**express answer as a whole number**

**PartE** the pH after adding 5.0 mL of base beyond
the equilance point **express your answer using two decimal
places**

Answer #1

a)

initially:

[H+] = 0.175 M

pH = -log(0.175)

pH = 0.75

b)

Vequivalence:

Macid*Vacid = Mbase*Vbase

Vbase = Macid*Vacid/Mbase = 0.175*35/0.205 = 29.878 mL

c)

mmol of acid = MV = 0.175*35 = 6.125

mmol of base = MV = 11.9*0.205 = 2.4395

after reaction

mmol of H+ = 6.125-2.4395 = 3.6855

[H+] = mmol/mL = 3.6855/(35+11.9) = 0.07858

d)

in equivalence pH = 7 since strong acid/base

e)

mmol of OH- = (5)(0.205)/(29.878 +5+35) = 0.01466

ph = !4 + log(OH) = 14 + log(0.01466) = 12.17

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 0.175 M CH3NH2
with 0.150 M HBr. Determine each of the following.
1. the pH at 4.0 mL of added
acid
2.the pH at the equivalence point
3.the pH after adding 6.0 mL of acid beyond the equivalence
point

Consider the titration of a 34.0 mL sample of 0.170 M HBr with
0.205 M KOH . What is the pH after adding 5.0 mL of base beyond the
equivalence point? If you could show all work that would be
great.

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 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 a
strong acid - strong base titration OF 35.00 mL sample of 0.175 m
HBr with 0.200 m KOH
what is the ph of a solution
after 10.00 ml of the KOH has been added? Stichiometry only, no
equilibrium

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 28.0?mL sample of 0.180M CH3NH2 with
0.150M HBr. 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 6.0mL 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 6.0mL of acid beyond the equivalence
point
Some help & direction would be great very confused! Thank...

Consider the titration of a 25.0 mL sample of 0.110 molL−1
CH3COOH (Ka=1.8×10−5) with 0.130 molL−1 NaOH. Determine
each quantity:
Part A
Part complete
the initial pH
Express your answer using two decimal places.
pH =
2.85
SubmitPrevious Answers
Correct
Part B
Part complete
the volume of added base required to reach the equivalence
point
V =
21.2
mL
SubmitPrevious Answers
Correct
Part C
Part complete
the pH at 4.0 mL of added base
Express your answer using two decimal...

Consider the titration of a 27.0 −mL sample of 0.180 M CH3NH2
with 0.145 M HBr. Determine the pH after adding 6.0 mL of acid
beyond the equivalence point.

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