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Solubility of Mercury Oxide in Different Aqueous Solutions at 25°C, Lecture notes of Communication

Experimental data on the solubility of mercury oxide (HgO) in various aqueous solutions, including hydrofluoric acid (HF), sodium hydroxide (NaOH), potassium hydroxide (KOH), and sodium hydroxide with different concentrations. The document also includes information on the preparation of the solutions, the experimental procedure, and the sources and purity of materials.

What you will learn

  • How does the concentration of sodium hydroxide affect the solubility of mercury oxide?
  • What is the solubility of mercury oxide in hydrofluoric acid at 25°C?
  • What is the solubility of mercury oxide in sodium hydroxide solutions at 25°C?
  • How does the addition of potassium fluoride affect the solubility of mercury oxide in hydrofluoric acid?
  • What is the solubility of mercury oxide in potassium hydroxide solutions at 25°C?

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Mercury(ll)
Oxide
319
COMPONENTS:
(1)
Mercury(II)
oxide;
HgO;
[21908-53-2]
(2)
Hydrofluoric
acid;
HF;
[7664-39-3]
(3)
Water;
H2
0;
[7732-18-5]
VARIABLES:
Concentration
of
HF
at
25°C.
EXPERIMENTAL
VALUES:
ORIGINAL
MEASUREMENTS:
Jaeger,
A.
Z.
AnoJLg.
Chern.
1901,
27,
22-40.
PREPARED
BY:
T.
P.
Dirkse
Solubility
of
HgO
in
aqueous
HF
at
25°C.
-3
g
Hg/9.6
-3
cHF/mol
dm
ccm
CHgO/mol
dm
0.12
0.0242
0.01258
0.24
0.0475
0.0247
0.57
0.1210
0.0629
1.11
0.2247
0.1168
2.17
0.4976
0.2586
The
solid
phase
is
not
identified
but
the
implication
is
that
it
is
HgO.
The
concentration
of
HgO
varies
almost
linearly
with
the
concentration
of
HF.
The
author
concludes
from
this
that
the
reaction
of
dissolution
is
HgO(s) +H2F2=
HgF
2+H2
0,
i.e.,
the
molecular
formula
of
hydrogen
fluoride
is
H2F2
In
additional
experiments,
details
of
which
are
not
included
in
the
article,
the
solubility
of
HgO
in
aqueous
HF
was found
to
decrease
when
KF
was added
to
the
aqueous
HF.
The
author
attributes
this
to
the
lack
of
formation
of
mercury
fluoride
complexes.
AUXILIARY
INFORMATION
METHOD/APPARATUS/PROCEDURE:
Mixtures
of
red
HgO
and
aqueous
HF
were
shaken
in
a
thermostat
at
25°C. The
mercury
content
of
the
saturated
solutions
was
de-
termined
by
electrolysis.
No
information
is
given
about
the
length
of
time
the
mixtures
were
shaken.
The
glass
apparatus
was
protected
from
attack
by
the
HF
by
coating
it
with
bee's
wax
or
a
commercially
available
gelatin-like
material.
SOURCE
AND
PURITY
OF
MATERIALS:
The
materials
were
of
a
chemically
pure
grade.
ESTIMATED
ERROR:
No
details
are
given.
REFERENCES:
pf3
pf4
pf5
pf8
pf9
pfa
pfd
pfe
pff

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Mercury(ll) Oxide 319

COMPONENTS:

(1) Mercury(II) oxide; HgO; [21908-53-2]

(2) Hydrofluoric acid; HF; [7664-39-3]

(3) Water; H 2

0; [7732-18-5]

VARIABLES:

Concentration of HF at 25°C.

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Jaeger, A. Z. AnoJLg. Chern. 1901, 27,

PREPARED BY:

T. P. Dirkse

Solubility of HgO in aqueous HF at 25°C.

-3 (^) g Hg/9.6 - cHF/mol dm ccm^ CHgO/mol^ dm

0.12 0.0242^ 0.

0.24 0.0475^ 0.

0.57 0.1210^ 0.

1.11 0.2247^ 0.

2.17 0.4976^ 0.

The solid phase is not identified but the implication is that it is HgO.

The concentration of HgO varies almost linearly with the concentration of HF. The author concludes from this that the reaction of dissolution is

HgO(s) + H 2 F 2 = HgF 2 + H 2 0,

i.e., the molecular formula of hydrogen fluoride is H 2 F 2 •

In additional experiments, details of which are not included in the article, the solubility of HgO in aqueous HF was found to decrease when KF was added to the aqueous HF. The author attributes this to the lack of formation of mercury fluoride complexes.

AUXILIARY INFORMATION

METHOD/APPARATUS/PROCEDURE:

Mixtures of red HgO and aqueous HF were shaken in a thermostat at 25°C. The mercury content of the saturated solutions was de- termined by electrolysis. No information is given about the length of time the mixtures were shaken. The glass apparatus was protected from attack by the HF by coating it with bee's wax or a commercially available gelatin-like material.

SOURCE AND PURITY OF MATERIALS:

The materials were of a chemically pure grade.

ESTIMATED ERROR:

No details are given.

REFERENCES:

320 Mercury(ll) Oxide

COMPONENTS:

(1) Mercury(II) oxide; RgO; [21908-53-2]

(2) Barium hydroxide; Ba(OR)2; [17194-00-2]

(3) Water; R 2 0; [7732-18-5]

VARIABLES:

Red and yellow RgO were used at 25°C.

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Schick, K. Z. physik. Chern. 1903, 42, 155-

PREPARED BY:

T. P. Dirkse

yellow RgO

red RgO

Table I Solubility of RgO in water at 25.0 0 C.

0.0518 g dm- 3 2.39 x 10- 4 mol dm- 3 a

0.0513 g dm- 3 2.37 x 10-

mol dm- 3 a

a Calculated by compiler.

Table II

Solubility of yellow RgO in barium hydroxide solutions at 25.0°C.

mol Ba(OR)2 dm-3 g RgO dm-3 mol RgO dm-3 a

a'Calculated by compiler.

AUXILIARY INFORMATION

2.71 x 10- 4

6.29 x 10- 4

METHOD/APPARATUS/PROCEDURE: SOURCE AND PURITY OF MATERIALS:

Oxide-solvent mixtures were shaken in a closed vessel in a thermostat for a week, allowed to settle for 36 hours, and filtered The mercury content was determined by two methods: (a) add 5 g NaCl to 100 ml of solution, heat to boiling and cool to 40-50° , add phenolphthalein and titrate the NaOR pro duced by this reaction with RCl; (b) evapora e an aliquot of the solution to dryness and weigh the residue. Equilibrium was approach ed from both supersaturation and under saturation.

Conductivity water and purified forms of the red and yellow RgO were used.

ESTIMATED ERROR:

The impurities in the oxides were estimated at less than 0.005%.

REFERENCES:

322 Mercury(1I)^ Oxide

COMPONENTS: (1) Mercury(II) oxide; HgO; [21908-53-2]

(2) Lithium hydroxide; LiOH; [1310-65-2]

(3) Water; H 2

0; [7732-18-5]

VARIABLES:

Lithium hydroxide concentration at 25°C.

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Garrett, A. B.; Hirschler, A. E.

J. Am. Chern. Soa. 1938, 60, 299-

PREPARED BY:

T. P. Dirkse

Solubility of yellow HgO in LiOH solutions at 25°C.

mol LiOH/kg H 2

METHOD/APPARATUS/PROCEDURE:

(mol HgO/kg H 2

  1. x 105

AUXILIARY INFORMATION

SOURCE AND PURITY OF MATERIALS:

Samples of HgO and solvent were sealed in nitrogen-filled flasks and shaken for 3 weeks at 25°C. Other mixtures were shaken at 42°C for about 3 days and then at 25°C for 3 weeks. After agitation, the samples were allowed to sediment for 4 da)s, then filtered through a sintered glass filter. Alkali concentration was determined by weight titration using methyl o~ange indi- cator. Mercury content was determined by potentiometric titration with KI (1).

Two different preparations of yellow lIg were used. Reagent grade LiOH was dis- solved in water and allowed to stand for a while so that the slight precipitate could settle out. Conductivity water was used throughout.

ESTIMATED ERROR:

Mercury analysis had a reproducibility with- in 0.5% The alkali analysis had an error of less than 5%. Separate solubility values were within 2% of the avera~e.

REFERENCES:

  1. Maricq, L. Bu~~, Boa. ahim. be~g. 1928, 37, 241.

Mercury(ll) Oxide 323

COMPONENTS:

(1) Mercury(II) oxide; HgO; [21908-53-2]

(2) Potassium hydroxide; KOH; [1310-58-3]

(3) Water; H 2 0; [7732-18-5]

VARIABLES:

Concentration of KOH at 25°C.

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Garrett, A. B.; Hirsch1er, A. E.

J. Am. Chern. Soa. 1938, 60. 299-

PREPARED BY:

T. P. Dirkse

Solubility of yellow HgO in KOH solutions at 25°C.

mol KOH/kg H 2

5 (mol HgO/kg H 2 0)x 10

AUXILIARY INFORMATION

METHOD/APPARATUS/PROCEDURE:

Samples of HgO and solvent were sealed in nitrogen-filled flasks and shaken for 3 weeks at 25°C. Other mixtures were shaken at 42°C for about 3 days and then at 25°C for 3 weeks After agitation, the samples were allowed to sediment for 4 days, then filtered through a sintered glass filter. Alkali concentration was determined by weight titration using methyl orange indicator. Mercury content was determined by potentiometric titration with KI (1).

SOURCE AND PURITY OF MATERIALS:

Two different preparations of yellow HgO were used. The hydroxide solutions were carbonate-free. Conductivity water was used throughout.

ESTIMATED ERROR:

Mercury analysis had a reproducibility with- in 0.5%. The alkali analysis had an error of less than 5%. Separate solubility values "',." ",i ~hi" ?OJ nJ' ~h" REFERENCES:

  1. Maricq, L. BuZZ. soa. ahim. beZg. 1928,

Mercury(ll) Oxide 325

COMPONENTS:

(1) Mercury(II) oxide; HgO; [21908-53-2]

(2) Sodium hydroxide; NaOH; [1310-73-2]

) (3) Water; H 2 0; [7732-18-5]

VARIABLES:

Sodium hydroxide concentration at 25°C.

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Garrett, A. B.; Hirschler, A. E.

J. Am. Chern. Boa. 1938, 60. 299-

PREPARED BY:

T. P. Dirkse

Solubility of red HgO in NaOH solutions at 25°C.

mol NaOH/kg H 2

O (mol HgO/kg H 2 O)^

x 105

0.1064 22.7 (^) (s) 0.3398 (^) 23. 0.4406 (^) 24.2 (s) 0.5818 (^) 24. 0.7223 (^) 25.1 (u) 1.001 (^) 26. 1.638 (^) 27. 1.987 27.6 (u) 2.940 29. 3.956 29. 4.936 29.

(s) equilibrium approached from supersaturation only.

(u) equilibrium approached from undersaturation only.

AUXILIARY INFORMATION

METHOD/APPARATUS/PROCEDURE: SOURCE AND PURITY OF MATERIALS:

Samples of HgO and solvent were sealed in nitrogen-filled flasks and shaken for 3 weeks at 25°C. bther mixtures were shaken at 42°C for about 3 days and then at 25°C for 3 weeks After agitation, the samples were allowed to sediment for 4 days, then filtered through a sintered glass filter. Alkali concentratio was determined by weight titration using meth 1 orange indicator. Mercury content was deter- mined by potentiometric titration with KI (1)

Five different preparations of red HgO were used. The hydroxide solutions were carbonate-free. Conductivity water was used throughout.

j

ESTIMATED ERROR:

Mercury analysis had a reproducibility with in 0.5%. The alkali analysis had an error of less than 5%. Separate solubility value were within 2% of the average. REFERENCES:

1. Maricq, L. BuZZ. soa. ahim. beZg. 1928,

326 Mercury(ll)^ Oxide

COMPONENTS:

(1) Mercury(II) oxide; HgO; [21908-53-2] (2) Nitric acid; HN0 3 ; [7697-37-2] (3) Water; H 2 0; [7732-18-5)

VARIABLES:

Concentration of HN 3

at 25°C.

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Garrett, A. B.; Howell, W. W. J. Am. Chern.

Soa • .1m, 61, 1730-4.

PREPARED BY:

T. P. Dirkse

Table I

Solubility of red HgO in aqueous nitric acid solutions.

(moles HNO/ 3 (moles HNO/ 3 (moles^ HgO/^4 kg H 2 0) x 0 kg H 2 0)^ x^0 kg H 2 0)^ x 10 as samples were from^ pHa made up

0.100 0.14^ 2. 0.200 0.07^ 3. 0.300 0.14 2.77^ (u) 0.500 0.30^ 3.48^ (s) 0.700 0.38 3. 0.900 0.48 4.02 (u) 2.00 2.5^ 6. 3.00 1.9 9. 5.00 3.8^ 14. 7.00 4.1^ 20. 9.00 5.0^ 27. 20.0 7.3^ 64.2^ (s)

a The value of H+ so determined was divided by the activity coefficient of HN 3

(s) equilibrium approached from supersaturation only.

(u) equilibrium approached from undersaturation only.

AUXILIARY INFORMATION

METHOD/APPARATUS/PROCEDURE:

Samples of HgO and solvent were sealed in nitrogen-filled flasks and shaken for 3 weeks at 25°C. Other such preparations were agi- tated for about 3 days at 42°C, then trans- ferred to a 25°C. thermostat for 3 weeks. After the agitation the samples were allowed to sediment for about 4 days before analysis. The nitric acid solutions were prepared by dilution of standard solutions. pH was measured after equilibrium by using a glass electrode. Mercury content was determined by potentiometric titration with KI (2).

SOURCE AND PURITY OF MATERIALS:

Materials were reagent grade. Conductivity water was used to make all solutions.

ESTIMATED ERROR~

Nothing is stated and only averages of pairs of values are given.

REFERENCES:

  1. Abel, E.; Redlich, D.; Lengyel, B. v.

Z. physik. Chern. 1928,132, 189.

2. Maricq, L. BuZZ. COC'. ahirn. belg. 1928,

J?, 241.

328 Mercury(ll) Oxide

COMPONENTS:

(1) Mercury(II) oxide; HgO; [21908-53-2]

(2) Hydrochloric acid; HCl; [7647-01-0]

(3) Water; H 2 0; [7732-18-5]

ORIGINAL MEASUREMENTS:

Garrett, A.B.; Lemley, J.

J. Am. Chern. Soa., 1942,64, 2380-3.

VARIABLES:

Concentration of hydrochloric acid. The temperature is not stated but from compari- sonwith other work it apparently is 25°C.

PREPARED BY:

T. P. Dirkse

EXPERIMENTAL VALUES: (^) Table I

Solubility of yellow HgO in aqueous HCl solutions

(s) equilibrium approached (u) equilibrium approached

(moles HgO/ 4 kg H 2 0) x 10

36

18.6(u)

56

31

19.8(u) 22.8(u) 34 (s) 47 (s) 232 (u) 414 (s) 534 (s) 1490 (s) 1480 (s)

(moles HCl/ kg H^2 2

0) x 10

from supersaturation only. from undersaturation only.

(moles HgO/ (^4) kg H 2 0) x 10

2.47(s)

  1. 7

    25.8(u)

    20.l(u)

(moles HCl/ 2

kg H 2 0) x 10

AUXILIARY INFORMATION

METHOD/APPARATUS/PROCEDURE: SOURCE AND PURITY OF MATERIALS:

Solid HgO was added to solutions and Reagent grade chemicals and conductivity shaken. Solubility was approached from water were used. under saturation and from supersaturation. The general procedure is the same as that used earlier (1).

ESTIMATED ERROR:

No estimate is given and the precision of the analyses cannot be inferred from the data given.

REFERENCES:

1. Garrett, A.B.; Howell, W. W. J. Am.

Chern. Soa., 1939, 61,1730.

Mercury(lll Oxide 329

COMPONENTS: ORIGINAL^ MEASUREMENTS

(1) Mercury^ (II)^ oxide;^ HgO;^ [21908-53-2]^ Garrett,^ A.B.;^ Lemley,^ J. J. Am. Chern. Soa., 1942,64, 2380-3. (2) Hydrochloric^ acid;^ HCl;^ [7647-01-0]

(3) Water; H 2

O; [7732-18-5]

EXPERIMENTAL VALUES continued •..

Table II

Solubility of yellow HgO in aqueous HCl solutions

moles HCl/kg H 2

O (moles HgO/ (^4) pH a^ Solid phase kg H 2

  1. x 10 color %Hg

0.00100 9.0 5.0 yellow 0.00300 20.8 4.9 yellow 0.00500 3.18 4.9 yellow 0.00700 40.7 4.7 yellow lie black 0.0090 28.9 4.9 yellow lie black 0.0120 30.9 5.1 yellow lie black 0.0160 29.1 5.0 yellow lie black 0.0200 22.1 4.8 yellow lie black 0.0300 15.0 5.0 yellow lie black 0.0400 10.0 5.2 yellow lie black 0.0500 21.6 5.1 brown 0.1007 82 4.0 black 0.1210 237 4.1 black 0.1412 387 4.2 black 85. 0.1614 (^545) 4.0 black 0.201B 8BO 3.8 black 85. 0.2425 1150 3.9 black 85. 0.2832 1410 black 85.

adetermined with a glass electrode

SD8 /.23-L

Mercury(1I) Oxide 331

COMPONENTS:

(1) Mercury (II) oxide; HgO; [21908-53-2] (2) Sodium perchlorate; NaCl 4

; [7601-89-0]

(3) Water; H 2 0; [7732-18-5]

VARIABLES:

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Dyrssen, D.; Tyrrell, V. Acta Chern. Scand.

1961, 15, 393-402 and 1622

PREPARED BY:

T. P. Dirkse

Table I

Solubility of red HgO in 3 mol dm^ -3 NaCl 4

solutions.

Concentrations are expressed as mol dm

-log [HgO]

-log [H^ + ]

AUXILIARY INFORMATION

METHOD/APPARATUS/PROCEDURE:

The solvents were allowed to percolate through a column containing the solid red HgO. The solid waflirradiated f2r 3 h~urs in a flux of 5.5 x 10 neutrons cm sec • Mercury content was determined by taking a weighed sample, counting the gamma radiation and comparing it with a carefully prepared and analyzed standard. pH measurements were made with a glass electr023' pH was adjusted by adding 0.01 mol dm NaOH or HCl0 4 •

SOURCE AND PURITY OF MATERIALS:

Reagent grade materials and conductivity water were used.

ESTIMATED ERROR: Analyses for individua!5sam- pIes had a standard deviation of 6 x 10 , but successive samples from a given system varied by 5% of the measured value. No in- dication is given as to how precisely the

332 Mercury(lll^ Oxide

COMPONENTS:

(1) Mercury(II) oxide; HgO; [21908-53-2]

(2) Sodium sulfide; Na 2 S; [1313-82-2]

(3) Water; H 2 0; [7732-18-5]

VARIABLES:

Concentration of sodium sulfide at 25°C

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Milyutina, N. A.; Polyvyannyi, I. R.;

Sysoyev, L. N. Pr. Inst. MetaZ. Obogashah.

AN Raz. BBR 1967, 21, 14-

PREPARED BY:

T. Michalowski

Solubility of HgO in aqueous Na 2 S at 25°C

mol S2- dm-3 mol Hg(II) dm-3 Ionic Strength, mol dm- 3

AUXILIARY INFORMATION

Activity coefficient of Hg(II)

METHOD/APPARATUS/PROCEDURE:

No details are given, but from other work reported by these authors it appears that equilibrium was reached isothermally after agitation for about a day.

SOURCE AND PURITY OF MATERIALS:

The HgO and Na 2 S were analytical grade materials.

ESTIMATED ERROR:

This cannot be estimated from the limited amount of information given in the paper.

REFERENCES:

334 Mercury(ll)^ Oxide

COMPONENTS:

(1) Mercury(II) oXide; RgO; [21908-53-2]

(2) Potassium hydroxide; KOR; [1310-58-3]

(3) Water; R 2

0; [7732-18-5]

VARIABLES:

Concentration of KOR and temperature.

EXPERIMENTAL VALUES:

ORIGINAL MEASUREMENTS:

Zhou, Weifang; Chen, Xialing Fudan Xuebao,

Z~n Kexueban 1983, 22, 229-31.

PREPARED BY:

T. P. Dirkse

Solubility (^) of RgO in aqueous KOR a.

10 CRgO/mol dm

t/oC (^) Ab^ B C (^) D E -- -- --^ -- -- -- 25 2.8 3.1 3.2 2.7 2. 35 4.1 4.4 4.4 3.7 2. 45 5.8 6.1 5.8 4.8 3. 55 8.1 8.1 7.3 5.9 5.

a These values are not included in the original article, but were supplied by the authors in a personal communication.

b The KOR concentrations (in mass %) for each column is: A = 1;

B = 5; C = 10; D = 20; E = 30.

AUXILIARY INFORMATION

METHOD/APPARATUS/PROCEDURE:

The e.m.f. of the following cell was measured:

HgIHg(II),KOH(aq) IKOH(aq) IHgO(s) IHg

The KOH concentration was the same in both cell compartments. The concentration of Hg(II) in the left cell compartment was prepared accurately and was less than 50% of the concentration in the right cell compartment. The temperature was controlled to within O.loC.

SOURCE AND PURITY OF MATERIALS:

The Hg, HgO and KOH were reagent grade materials. The water was distilled twice.

ESTIMATED ERROR:

Less than 5%.

REFERENCES: