From the two given titration curves, the curve that denotes the strong base should be identified. Concept introduction: Strong Base: Bases that has strong attraction towards protons and accepts readily. Strong base forms weaker conjugated acid. pH : The concentration of hydrogen ion is measured using pH scale. The pH of a solution is a figure that expresses the acidity or the alkalinity of a given solution. It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration. pH = -log[H 3 O + ] Acid dissociation constant K a represents how strong the acid is in a solution. pK a is defined as negative logarithm of acid dissociation constant( K a ). p K a = − log K a The strength of acid decreases as the value of p K a increases p K a represents the chance of losing proton from a compound. Henderson-Hasselbalch equation pKa = pH + log [ HA ] [ A - ] Henderson-Hasselbalch equation explains the relationship between p H of solution and p K a of acid. For a dissociation of acid ( H A ) in aqueous solution, H A + H 2 O ⇌ H 3 O + + A − p K a = p H + log [ H A ] [ A − ] Titration is a process where a known concentrated solution is used for determining the concentration of an unknown solution. The known concentrated solution is called the titrant, while the unknown concentrated solution is called the analyte. The equivalence point is a point in a titration where the amount of standard solution added is sufficient to neutralize the unknown solution completely. At this point, the total number of moles of standard solution (titrant) is equal to the number of moles of an unknown solution (analyte).
From the two given titration curves, the curve that denotes the strong base should be identified. Concept introduction: Strong Base: Bases that has strong attraction towards protons and accepts readily. Strong base forms weaker conjugated acid. pH : The concentration of hydrogen ion is measured using pH scale. The pH of a solution is a figure that expresses the acidity or the alkalinity of a given solution. It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration. pH = -log[H 3 O + ] Acid dissociation constant K a represents how strong the acid is in a solution. pK a is defined as negative logarithm of acid dissociation constant( K a ). p K a = − log K a The strength of acid decreases as the value of p K a increases p K a represents the chance of losing proton from a compound. Henderson-Hasselbalch equation pKa = pH + log [ HA ] [ A - ] Henderson-Hasselbalch equation explains the relationship between p H of solution and p K a of acid. For a dissociation of acid ( H A ) in aqueous solution, H A + H 2 O ⇌ H 3 O + + A − p K a = p H + log [ H A ] [ A − ] Titration is a process where a known concentrated solution is used for determining the concentration of an unknown solution. The known concentrated solution is called the titrant, while the unknown concentrated solution is called the analyte. The equivalence point is a point in a titration where the amount of standard solution added is sufficient to neutralize the unknown solution completely. At this point, the total number of moles of standard solution (titrant) is equal to the number of moles of an unknown solution (analyte).
Solution Summary: The author explains the titration curve that denotes the strong base. The concentration of hydrogen ion is measured using pH scale.
From the two given titration curves, the curve that denotes the strong base should be identified.
Concept introduction:
Strong Base: Bases that has strong attraction towards protons and accepts readily. Strong base forms weaker conjugated acid.
pH: The concentration of hydrogen ion is measured using pH scale. The pH of a solution is a figure that expresses the acidity or the alkalinity of a given solution.
It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.
pH=-log[H3O+]
Acid dissociation constant Ka represents how strong the acid is in a solution. pKa is defined as negative logarithm of acid dissociation constant(Ka).
pKa=−logKa
The strength of acid decreases as the value of pKa increases
pKa represents the chance of losing proton from a compound.
Henderson-Hasselbalch equation
pKa=pH+log[HA][A-]
Henderson-Hasselbalch equation explains the relationship between pH of solution and pKa of acid. For a dissociation of acid (HA) in aqueous solution,
HA+H2O⇌H3O++A−
pKa=pH+log[HA][A−]
Titration is a process where a known concentrated solution is used for determining the concentration of an unknown solution. The known concentrated solution is called the titrant, while the unknown concentrated solution is called the analyte.
The equivalence point is a point in a titration where the amount of standard solution added is sufficient to neutralize the unknown solution completely. At this point, the total number of moles of standard solution (titrant) is equal to the number of moles of an unknown solution (analyte).
LTS
Solid:
AT=Te-Ti
Trial 1
Trial 2
Trial 3
Average
ΔΗ
Mass water, g
24.096
23.976
23.975
Moles of solid, mol
0.01763
001767
0101781
Temp. change, °C
2.9°C
11700
2.0°C
Heat of reaction, J
-292.37J -170.473
-193.26J
AH, kJ/mole
16.58K 9.647 kJ 10.85 kr
16.58K59.64701
KJ
mol
12.35k
Minimum AS,
J/mol K
41.582
mol-k
Remember: q = mCsAT (m = mass of water, Cs=4.184J/g°C) & qsin =-qrxn &
Show your calculations for:
AH in J and then in kJ/mole for Trial 1:
qa (24.0969)(4.1845/g) (-2.9°C)=-292.37J
qsin =
qrxn =
292.35 292.37J
AH in J = 292.375 0.2923kJ
0.01763m01
=1.65×107
AH in kJ/mol =
=
16.58K
0.01763mol
mol
qrx
Minimum AS in J/mol K (Hint: use the average initial temperature of the three trials, con
Kelvin.)
AS=AHIT
(1.65×10(9.64×103) + (1.0
Jimai
For the compound: C8H17NO2
Use the following information to come up with a plausible structure:
8
This compound has "carboxylic acid amide" and ether functional groups.
The peaks at 1.2ppm are two signals that are overlapping one another.
One of the two signals is a doublet that represents 6 hydrogens; the
other signal is a quartet that represents 3 hydrogens.
Vnk the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest bolling
point, choose 2 next to the substance with the next highest boiling point, and so on.
substance
C
D
chemical symbol,
chemical formula
or Lewis structure.
CH,-N-CH,
CH,
H
H 10: H
C-C-H
H H H
Cale
H 10:
H-C-C-N-CH,
Bri
CH,
boiling point
(C)
Сен
(C) B
(Choose
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell