Question

Consider the titration of 120.0 mL of 0.100 *M* HI by
0.250 *M* NaOH.

**Part 1**

Calculate the pH after 35.0 mL of NaOH has been added.

pH =

**Part 2**

What volume of NaOH must be added so the pH = 7.00?

_______mL NaOH

Answer #1

**Number of moles of HI = 120*0.1 = 12 mmol**

**number of moles of NaOH = 35 * 0.25 = 8.75
mmol**

**NaOH + HI ------> NaI + H2O**

**remaining number of moles HI remainig = 12 - 8.75 = 3.25
mmol**

**concentration of HI = 3.25/(120+35) = 0.021
mol/L**

**pH = -log[H+]**

**pH = -log(0.021)**

**pH = 1.678**

**when, number of moles of H+ = number of moles OH- then
pH of the solution = 7**

**we have the formula M1V1 = M2V2**

**0.1*120 = 0.25*V2**

**V2 = 48 mL**

**so if we add 48 mL of NaoH then the pH will become pH =
7**

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

Consider the titration of 100.0 mL of 0.200 M CH3NH2 by 0.100 M
HCl. For each volume of HCl added, decide which of the components
is a major species after the HCl has reacted completely. Kb for
CH3NH2 = 4.4 x 10-4. 1) Calculate the pH at the equivalence point
for this titration 2) At what volume of HCl added in this titration
does the pH = 10.64? Express your answer in mL and include the
units in your answer.

Consider the titration of a 45.0 mL sample of 0.100 M HN3 with
0.250 M KOH. (Ka of HN3 = 2.5 x 10-5) Calculate each of the
following: (a) How many mL are required to reach the equivalence
point?
(b) What is the initial pH of the acid solution?
(c) What is the pH after the addition of 5.00 mL of KOH?
(d) What is the pH after the addition of 9.00 mL of KOH? (e)
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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 0.125 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
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Determine the pH after adding 4.00 mL of base. I have found that
the volume of the base needed to reach the equivalence point is
20.0 mL.
Show your work and be as clear as possible. Thank you in
advance!

500.0 mL of 0.100 M NaOH is added to 575 mL of 0.250 M weak acid
(Ka = 3.61 × 10-5). What is the pH of the resulting buffer?

Consider the titration of 40.0 mL of 0.250 M HF with 0.200 M
NaOH. How many milliliters of base are required to reach the
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a)After the addition of 10.0 mL of base
b)Halfway to the equivalence point
c)At the equivalence point
d)After the addition of 80.0 mL of base

A - B
100. mL of 0.200 M HCl is titrated with 0.250
M NaOH.
Part A
What is the pH of the solution after 50.0 mL of base has been
added?
Express the pH numerically.
pH =
SubmitHintsMy AnswersGive UpReview Part
Part B
What is the pH of the solution at the equivalence point?
Express the pH numerically.
pH =
SubmitHintsMy AnswersGive UpReview Part

For the titration of 30.0 mL of 0.250 M NH3 with 0.500 M HCl at
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have been added pH>7 pH<7 pH=7

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