Question

Two 23.0 mL samples, one 0.200 MKOH and the other 0.200 M CH3NH2, were titrated with 0.100 MHI. Answer each of the following questions regarding these two titrations.

a) What is the volume of added acid at the equivalence point for KOH?

b) What is the volume of added acid at the equivalence point for CH3NH2?

Answer #1

No. of moles = Molarity Volume of solution in litres

moles KOH = 0.023 L x 0.200 M = 4.6
10^{-3}

moles HI required = 4.6
10^{-3}

Volume HI added at equivalence point = (4.6 10^{-3})
/ 0.100 M = 0.046 L = 46.0 mL

the moles of CH_{3}NH_{2} are the same, so the
volume of HI added at equivalence point is the same : 46.0 mL

Two 23.0 mL samples, one 0.200 MKOH and the other 0.200 M
CH3NH2, were titrated with 0.100 MHI. Answer each of the following
questions regarding these two titrations.
a). What is the volume of added acid at the equivalence point
for CH3NH2?
b). Predict whether the pH at the equivalence point for each
titration will be acidic, basic, or neutral.
c). Predict which titration curve will have the lowest initial
pH.

Two 25.0 ml samples, on 0.100 mol/L HCl and the other 0.100mol/L
HF, were titrated with 0.200 mol/L KOH.
a) What is the volume of added base at the equivalence point for
each titration?
b) Predict whether the pH at the equivalence point for each
titration will be acidic, basic or neutral? Explain your
selection.
c) Predict which titration curve will have the lower initial pH
and explain your selection.

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.

1. A 100 mL solution of 0.200 M HF is titrated with 0.100 M
Ba(OH)2. What is the volume of Ba(OH)2 needed
to reach equivalence point?
200 mL
50 mL
100 mL
300 mL
Cannot determine based on the provided information.
2. A 100 mL solution of 0.200 M NH3 is titrated with
0.100 M HCl. What is the volume of HCl needed to reach equivalence
point?
200 mL
100 mL
50 mL
300 mL
Cannot determine based on the...

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titrated with 0.200 M KOH.
Region 1: Initial pH: Before any titrant is added to our starting
material
What is the concentration of H+ at this point in the
titration?
M
What is the pH based on this H+ ion concentration?
Region 2: Before the Equivalence Point 10.13 mL of the 0.200 M KOH
has been added to the starting material.
Complete the BCA table below at...

A 100 mL solution of 0.200 M Sr(OH)2 is titrated with
0.100 M H3PO4. What is the volume of
H3PO4 needed to reach equivalence point?
100 mL
200 mL
50 mL
300 mL
133 mL
A 100 mL solution of unknown concentration
H2SO4 is titrated with 200 mL of 0.100 M
Ba(OH)2 solution to reach equivalence point. What is the
concentration of H2SO4 solution?
0.100 M
0.050 M
0.020 M
0.200 M
Cannot determine based on the provided information.

16.5 mL of 0.168 M diprotic acid (H2A) was titrated with 0.118 M
KOH. The acid ionization constants for the acid are Ka1=5.2×10−5
and Ka2=3.4×10−10. At what added volume (mL) of base does the first
equivalence point occur?
20.8 mL of 0.146 M diprotic acid (H2A) was titrated with 0.14 M
KOH. The acid ionization constants for the acid are Ka1=5.2×10−5
and Ka2=3.4×10−10. At what added volume (mL) of base does the
second equivalence point occur?
Consider the titration of...

a) 30.0 ml of an HCl solution of unknown molarity was titrated
with .200 M NaOH. Phenolphthalien was used as the indicator. The
titrated solution turned a very pale pink after 21.8 mL of NaOH was
added. What was the initial molarity of the HCl?
b)Consider the following three titrations:
100.0 mL of 0.100 M CH3NH2 (Kb =
4.4x10-4) titrated with 0.100 M HCl
100.0 mL of 0.100 M NH3 (Kb = 1.8x10-5)
titrated with 0.100 M HCl
100.0 mL...

18.0 mL of 0.123 M diprotic acid (H2A) was titrated with 0.1020
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and Ka2=3.4×10−10.
At what added volume of base does the first equivalence point
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At what added volume of base does the second equivalence point
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Consider the titration of a 26.0-mL sample of 0.180 M CH3NH2
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4.4×10−4.)
Part A
Determine the initial pH.
Part B
Determine the volume of added acid required to reach the
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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...

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