Question
In: Chemistry
A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the...
A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 200.0 mL of KOH. The Ka of HF is 3.5 × 10-4.
Answer: 8.14 but how do I get this?? I'm so lost!
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A 100.0 mL sample of 0.20 M HF is titrated with 0.20 M KOH. Determine the...
A 100.0 mL sample of 0.20 M HF is titrated with 0.20 M KOH.
Determine the pH of the solution after the addition of 50.0 mL of
KOH. The Ka of HF is 3.5 × 10-4.
A. 2.08
B. 3.15
C. 4.33
D. 3.46
E. 4.15
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the...
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.
Determine the pH of the solution after the addition of 50.0 mL of
HNO3. The Kb of NH3 is 1.8 × 10-5.
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the...
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.
Determine the pH of the solution after the addition of 50.0 mL of
HNO3. The Kb of NH3 is 1.8 × 10-5.
1. A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Kb,...
1. A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.
Kb, NH3 = 1.8 × 10−5. Determine the pH of the solution at each of
the following points in the titration:
(a) before addition of any HNO3
(b) after the addition of 50.0 mL HNO3
(c) after the addition of 75.0 mL HNO3
(d) at the equivalence point
(e) after the addition of 150.0 mL HNO3
2. (12 points) Consider the titration of 37.0 mL...
A 25.0 mL sample of 0.30 M HCOOH is titrated with 0.20 M KOH. What is...
A 25.0 mL sample of 0.30 M HCOOH is titrated with 0.20 M KOH.
What is the pH of the solution after 25.0 mL of KOH has been added
to the acid? Ka = 1.8x10^-4
20.0 ml of 0.10M HCN is titrated with 0.10 M KOH. determine the ph at the...
20.0 ml of 0.10M HCN is titrated with 0.10 M KOH. determine the
ph at the equivalence point.
A 25.0mL sample of 0.35M HCOOH is titrated with 0.20 M KOH. a) Determine the volume...
A 25.0mL sample of 0.35M HCOOH is titrated with 0.20 M
KOH.
a) Determine the volume required to reach the equivalence
point
b) the pH of the solution at the equivalence point.
Ka=1.77x10-4
When you titrate 100 mL of 0.10 M HF with 0.10 M KOH a) When will...
When you titrate 100 mL of 0.10 M HF with 0.10 M KOH
a) When will this titration reach the equivalence point?
b) Calculate pH when you add 5 mL of KOH.
c) Calculate pH when you add 50 mL of KOH.
d) Calculate pH at the equivalence point.
e) Calculate pH when you add 101 mL of KOH.
(show each step)
Consider the following four titrations. i. 100.0 mL of 0.10 M HCl titrated by 0.10 M...
Consider the following four titrations.
i. 100.0 mL of 0.10 M HCl titrated by 0.10 M
NaOH
ii. 100.0 mL of 0.10 M NaOH titrated by 0.10 M
HCl iii. 100.0 mL of 0.10 M CH3NH2 titrated by 0.10
M HCl
iv. 100.0 mL of 0.10 M HF titrated by 0.10 M
NaOH Rank the titrations in order of:
increasing volume of titrant added to reach the equiva-
lence point.
increasing pH initially before any titrant has been added.
increasing...
5) A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine...
5) A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M
LiOH. Determine the pH of the solution
a) before the addition of any LiOH.
b) after the addition of 30.0 mL of LiOH.
c) after the addition of 50.0 mL of LiOH.
d) after the addition of 66.67 mL of LiOH (this is the
equivalence point).
e) after the addition of 75.0 mL of LiOH.
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