Lecture 2: Cement Hydration - CoMSIRU
Transcript of Lecture 2: Cement Hydration - CoMSIRU
Cement Chemistry for Engineers, Cape Town 31st January 2013
Lecture 2: Cement Hydration
Nature of hydrates
Thermodynamic prediction of hydrate assemblages
Evolution of microstructure
Reaction between water and cement: Increasing solid volume, replaces water
Cement grain
water hydrates
Transformation from fluid paste to solid
NB cement grains are polymineralic
alite
belite
aluminate ferrite
Hydrate Phases
Alite, C3S + H C-S-H + CH
Belite, C2S + H C-S-H + CH
Aluminate,C3A + 3C$+ H AFt (ettringite)
AFt + 2C3A + H AFm
Ferrite, C4AF
Limestone CaCO3
Silicates
Aluminates
Basic Reactions
C-S-H
48%
CH
14%anhyd
3%pores
16%ett (AFt)
4%AFm
11% other
4%
C2S
15%
C3A
8%ferrite
7%
C3S
70%
Phases present – 14 month paste from Taylor
calcium hydroxide
Hydrated lime
portlandite
Ca(OH)2
CH
crystalline
Hexagonal
morphology
hydrated calcium silicate
C-S-H
Nano crystalline
multiple morphologies
~ 15-25% of hydrated paste
~ 50-65% of hydrated paste
Hydration of calcium silicates : C3S and C2S
C-S-H
• “atomic” structure and composition
• “meso” structure
• “microstructure / morphology”
C/S =
0.8 to 1.5 for synthetic
preparations
1.7-2 PC pastes
0,00
0,50
1,00
1,50
2,00
2,50
0,00 10,00 20,00 30,00 40,00
CaO mmol/l
C/S
Flint and Wells at
30°C
Taylor at 17-20°C
Lecoq 20°C
Thordvaldson 25°C
(+expé sursat)
Source Nonat, Taylor conf
Definite phase with
reproducible behaviour
C-S-H: range of compositions
Layers of Ca-O Tetrahera of Si-O4 linked in chains
Molecules of water 14Å
1.4nm
C-S-H, analogy with natural mineral Tobermorite
Ca/Si=0.833
- the abscence of some bridging tetrahedra (Q1/Q2 increases)
H
Ca Ca Ca Ca Ca Ca Ca
H H H H H H
H Ca/Si = 0.72
Ca
Ca/Si = 0.8 H
H H H H
H H H
Ca Ca Ca Ca Ca Ca Ca Ca
H H H H H H
H H Ca/Si = 0.9
Ca Ca Ca Ca Ca Ca Ca Ca
Source Nonat, Taylor conf
The increase of Ca/Si ratio is attributed to three mechanisms :
- the substitution of a part of the protons by calcium ions
Ca Ca Ca Ca Ca Ca Ca
Ca H H H H
H H Ca/Si = 1
Ca
H H Ca/Si = 1.22
Ca Ca Ca Ca Ca Ca Ca
Ca Ca Ca
Ca
H H H H H H
H H Ca/Si = 0.9
Ca Ca Ca Ca Ca Ca Ca Ca
- the abscence of some bridging tetrahedra (Q1/Q2 increases)
Source Nonat, Taylor conf
The increase of Ca/Si ratio is attributed to three mechanisms :
- the presence of Ca-OH regions
- the substitution of a part of the protons by calcium ions
- the abscence of some bridging tetrahedra (Q1/Q2 increases)
The increase of Ca/Si ratio is attributed to three mechanisms :
In presence of portlandite (CH) – high Ca/Si ratio:
• Almost exclusively dimers
• Almost all terminating Ca, not H
CL = 5 : pentamer
CL = 8 : octamer
CL = 2 : dimer
Change occurs very slowly, years; faster at higher temperatures
Also limited by portlandite presence
Silicate polymerisation during hydration
H+
- -
-
- - - -
Al
0.0 0.1 0.2 0.3 0.4 0.5 0.60.0
0.1
0.2
0.3
0.4
0.5 Ettringite 28 days 1 year 3 years
Monosulfate
CHCSH
S/C
a
Al/Ca
OPC pastes: Al/Ca ~ 0.05 ; Al/Si ~ 0.1
Higher with Al rich SCMs
C-S-H: Si substitution by Al
C-S-H
• “atomic” structure and composition
• “meso” structure
• “microstructure / morphology”
Evidence
• No long range order
• “intrinsic” porosity of 26-28% (Powers)
– “gel porosity”
- from drying – therefore upper limit
• Scattering experiments (neutron, X-ray) and proton NMR
indicate “characteristic size” of about 4-5 nm
Jennings model
Nano crystalline?
~5nm
Meso structure
Two interpretations of nanocrystalline nature:
1. Granules – independent blobs
2. Sheets with disorganised structure
Open question
General agreement that C-S-H consists of nanocrystalline
regions:
The main open question is whether they are discrete or linked by
sheets
Important issues for water transport through C-S-H
C-S-H
• “atomic” structure and composition
• “meso” structure
• “microstructure / morphology”
3 hrs
10 hrs
HVEM, wet cell, C3S, 24hrs
SEM fracture surface
Two microstructurally
distinct forms:
“Outer” or “early”
“inner” or “late”
TEM from Richardson
C-S-H summary
Atomic level structure fairly well understood:
CaO sheets with chains (dimers) of SiO4 tetrahedra attached
Al substitutes for Si, in bridging sites
Meso level structure less clear
Nanocrystallites or nanocrystalline regions with characteristic scale of about 5nm
Microstructure
Outer, formed early through solution
Inner formed later
ettringite
AFt – aluminate ferrite tri
Aluminate hydrates
2 24 3SO CO
Possible exchange
Ca3Si(OH)6(CO3)(SO4)·12H2O
(thaumasite)
AFm aluminate ferrite mono
[Ca2Al(OH)6]+ layers
Many inter layers ions:
24SO
3 32C A.3C$.H
hydrogarnet
katoite
monsulfate
8AlSi(OH) stratlingite
3 6C AH
2H Si
Possible exchange
OH 4 13C AH
23CO
Cl
monocarbonate
Friedel’s salt
C3A
+
water
stiffening
flash set
Fast reaction Large plates of hydrates
Calciumaluminate hydrates : C2AH8 , C4AH13 : AFm phases
then C3AH6
Hydration of aluminate phases : C3A
C3A + CaSO4Hx
_ _
3 2 3 32C A 3CSH 26H C A.3CS.H (ettringite)
_2 2
4 4 3 326Ca 2Al(OH) 3SO 4OH 26H Ca A.3CS.H
_ _
3 3 32 3 122C A C A.3CS.H 4H 3C A.CS.H
Exhaustion of sulfate
Calcium aluminate monosulfate
AFm phase stablised by solid solution
It forms in the presence of anhydrous C3A
In presence of CaCO3 (fine limestone)
monocarbonate forms instead of monosulfate
Setting regulation by sulfates
Hydration of aluminate phases : C3A
C3A + water + calcium sulfate
Note
Reaction of C3A is not blocked by ettringite
Reaction controlled by absorption of sulfate ions at reacting sites
Cement paste after 2-7 days -
local formation of monosulfate inside layer of C-S-H where there is C3A available.
Ettringite remains on exterior of grain.
Hydration of aluminate phases : C3A
2. Hydration Kinetics
3. Microstructure formation
equilibrium curve of the cement phase
equilibrium curve of the hydrate
condition of equilibrium of the
solids (thermodynamics)
precipitation [nucleation and
growth] with dissolution Path of solution composition resulting
from the dissolution of solids
[conc X]
[conc Y]
Hydrates form “through solution” due to difference in solubility of anhydrous compounds and hydrates
0
1
2
3
4
0 3 6 9 12 15 18 21 24
He
at F
low
(m
W/g
)
Age of Specimen (Hours)
sta
ge
1
sta
ge
2
sta
ge
3
sta
ge
4
Alite reaction
0
1
2
3
4
5
0 10 20 30 40 50
Heat
Evo
luti
on
Rate
[m
W/g
]
Time [h]
Secondary
formation
of ettringite
Formation
of AFm phase
Alite reaction
Portland cement: silicate plus aluminate
1μm
~10 h ~3 h ~10 m ~24 h
Heat flow
time
1μm
Initial
dissolution
Induction
Nucleation and growth
~10 h ~3 h ~10 m ~24 h time
Heat flow
Initial
dissolution
Induction
Nucleation and growth
12hr cement paste: ion thinned section TEM
For some (as yet unknown reason) the alite dissolves beneath the outer C-S-H,
leaving a gap or low density area
This hydrates of seems to grow the outside this “shell”,
small hollow shells persist in mature concrete
The presence of aluminate seems to be important as these shells are not so
clearly separated in the case of C3S
Formation of Hadley grains (hollow shells)
28 days, SEM
SCRIVENER, 1984
Summary Microstructural Development
50 mm
Hydration of different phases
Ph D Vanessa Kocaba (NANOCEM, CP4)
1 10 100 0
20
40
60
80
100
alit
e (
%w
t)
1 10 100
0
20
40
60
80
100
be
lite
(%
wt)
Time (d)
1 10 100 0
20
40
60
80
100
alu
min
ate
(%
wt)
1 10 100 0
20
40
60
80
100
ferr
ite
(%
wt)
A
B
C
D
Time (d)
Reaction of Belite
Old concrete, only belite and ferrite apparent
Reaction of ferrite phase
XRD shows reaction but in BSE appears unreacted
Alumina and calcium “leach” out leaving Fe “relic” as
hydrous Fe hydroxide of iron rich hydrogarnet
Aluminate phases in hardened cement paste
1 mm
Intermixing of ettringite and/or
Monosulfate at submicron scale
0.0 0.1 0.2 0.3 0.4 0.5 0.60.0
0.1
0.2
0.3
0.4
0.5 Ettringite 28 days
Monosulfate
CHCSH
S/C
a
Al/Ca
0.0 0.1 0.2 0.3 0.4 0.5 0.60.0
0.1
0.2
0.3
0.4
0.5
0.6
28 days
CH C1.7
SH
Ettringite
Monosulfo
Al/C
a
(Si+Al)/Ca
28 days. Formation of C-S-H, CH
ettringite and then monosulfate
3 3 32 3 12. . . .2C A C A 3CS H 4H 3C ACS H
0.0 0.1 0.2 0.3 0.4 0.5 0.60.0
0.1
0.2
0.3
0.4
0.5 Ettringite 28 days 1 year 3 years
Monosulfate
CHCSH
S/C
a
Al/Ca
0.0 0.1 0.2 0.3 0.4 0.5 0.60.0
0.1
0.2
0.3
0.4
0.5
0.6
28 days 1 year 3 years
CH C1.7
SH
Ettringite
Monosulfo
Al/C
a
(Si+Al)/Ca
1, 3 years. Further formation of C-S-H, CH
Reaction of ettringite into monosulfate
Source thesis Severine Lamberet
Microprobe analyses
Ettringite is commonly found in old concrete through recystallisation Quantity may increase due to carbonation – sulfate released as monosulfate converts to moncarbonate
This
reaction is
not
damaging
Impact of temperature on microstructural development
PhD Xinyu Zhang http://library.epfl.ch/theses/?nr=3725
0 5 10 15 20 25 30
-5
0
5
10
15
20
25
30
He
at e
vo
lutio
n r
ate
(m
W/g
)
Time (hours)
20°C
40°C
55°C
55°C
40°C
20°C
Effect of temperature
1 2 3 4 5 6 7 8 910 20 30
0
50
100
150
200
250
300
55°C
20°C
Cu
mu
lative
he
at (J
/g)
Time (hours)
20°C
40°C
55°C
40°C
Arrhenius’ equation
k = A exp(-Ea/(RT))
ln(k) = ln(A) - Ea/(RT)
k rate of reaction
A constant
Ea apparent activation energy
R gas constant,
8.31 J/K mole
T temperature in Kelvin
Temperatures does not affect mechanical properties and “durability” in the same way
0 2 4 6 8 10 12 14 16 18 20
0
1
2
3
4
5
6
7
8
Wa
ter
so
rptivity (
ms
ec
-1/21
0-6)
Time (d1/2
)
5°C
20°C
40°C
60°C
0 2 4 6 8 10 12 14 16 18 20
0
5
10
15
20
25
30
35
40
45
50
55
Co
mp
ressiv
e s
tre
ng
th (
MP
a)
Time (d1/2
)
5°C
20°C
40°C
60°C
strength Water absorption
Why?
Lower final degree of hydration at higher temperatures?
Different hydration products?
Need strength as a function of hydration degree not time
0
10
20
30
40
50
60
20 40 60 80 100
hydration degree (%)
co
mp
res
siv
e s
tre
ng
th (
MP
a)
20°C
40°C
60°C
5°C
(w/c=0.5)
90d
0.00
0.05
0.10
0.15
0.20
0.25
0.30
0.35
0.40
0.45
mix1 mix5 mix4 mix2 mix3
20°C
40°C
60°C
inner CSH is very
thin
w/c=0.6
CEM42.
5
w/c=0.35
CEM52.5
R
20°C
60°C
CSH relative density
Due to lower microporosity in C-S-H
– more capillary porosity at higher
temperatures.
Building Materials Analysis 2009
C-S-H formed at 90°C
Brighter = more dense;
less microporosity
C-S-H formed at 20°C
Darker = less dense;
more microporosity
58
Cement Chemistry for Engineers, Cape Town 31st January 2013
End Lecture 2