Saline water (more commonly known as salt water) is water that contains a high concentration of dissolved salts (mainly sodium chloride). On the United States Geological Survey (USGS) salinity scale, saline water is saltier than brackish water, but less salty than brine. The salt concentration is usually expressed in parts per thousand (permille, ‰) and parts per million (ppm). The USGS salinity scale defines three levels of saline water. The salt concentration in slightly saline water is 1,000 to 3,000 ppm (0.1–0.3%); in moderately saline water is 3,000 to 10,000 ppm (0.3–1%); and in highly saline water is 10,000 to 35,000 ppm (1–3.5%). Seawater has a salinity of roughly 35,000 ppm, equivalent to 35 grams of salt per one liter (or kilogram) of water. The saturation level is only nominally dependent on the temperature of the water.[1] At 20 °C (68 °F) one liter of water can dissolve about 357 grams of salt, a concentration of 26.3 percent by weight (% w/w). At 100 °C (212 °F) (the boiling temperature of pure water), the amount of salt that can be dissolved in one liter of water increases to about 391 grams, a concentration of 28.1% w/w.

Properties

Water-NaCl phase diagram
Properties of water-NaCl mixtures[2]
NaCl, wt%Freezing point (°C)Freezing point (°F)Density[lower-alpha 1] (g/cm3)Refractive index[lower-alpha 2] at 589 nmViscosity[lower-alpha 3] (cP )
00320.999841.33301.002
0.5−0.331.461.00181.33391.011
1−0.5930.941.00531.33471.02
2−1.1929.861.01251.33651.036
3−1.7928.781.01961.33831.052
4−2.4127.661.02681.34001.068
5−3.0526.511.03401.34181.085
6−3.725.341.04131.34351.104
7−4.3824.121.04861.34531.124
8−5.0822.861.05591.34701.145
9−5.8121.541.06331.34881.168
10−6.5620.191.07071.35051.193
12−8.1817.281.08571.35411.25
14−9.9414.111.10081.35761.317
16−11.8910.601.11621.36121.388
18−14.046.731.13191.36481.463
20−16.462.371.14781.36841.557
[lower-alpha 4]23.3−21.1−5.981.179
26−19.18−2.521.1931.37951.676
  1. ↑ At some ambient temperature
  2. ↑ At some ambient temperature
  3. ↑ At some ambient temperature (20°C)
  4. ↑ Eutectic mixture

At 100 °C (212 °F; 373 K), saturated sodium chloride brine is about 28% salt by weight. At 0 °C (32 °F; 273 K), brine can only hold about 26% salt.[3] At 20 °C one liter of water can dissolve about 357 grams of salt, a concentration of 26.3%.[4]

The thermal conductivity of seawater (3.5% dissolved salt by weight) is 0.6 W/mK at 25 °C (77 °F).[5] The thermal conductivity decreases with increasing salinity and increases with increasing temperature. [6] [7] The salt content can be determined with a salinometer.

Density ρ of brine at various concentrations and temperatures from 200 to 575 °C (392 to 1,067 °F) can be approximated with a linear equation:[8]

where the values of an are:

Weight %a2a3
50.04372.60
100.03973.72
150.03574.86
200.03276.21
250.03077.85

Electrolysis

About four percent of hydrogen gas produced worldwide is created by electrolysis. The majority of this hydrogen produced through electrolysis is a side product in the production of chlorine.

  • 2 NaCl(aq) + 2 H2O(l) → 2 NaOH(aq) + H2(g) + Cl2(g)

See also

References

  1. ↑ "Sodium Chloride MSDS". Sigma Aldrich. c. 2004. Archived from the original on 2021-02-09.
  2. ↑ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. pp. 8–71, 8–116. ISBN 0-8493-0486-5.
  3. ↑ CRC Handbook of Chemistry and Physics, 63rd Edition 1982-1983.
  4. ↑ "Solubility". University of Wisconsin Fundamentals of Chemistry. Archived from the original on 31 March 2016. Retrieved 6 November 2014.
  5. ↑ Thermophysical properties of seawater: a review of existing correlations and data Paper published in April 2010 on web.mit.edu. Retrieved 2021-03-11.
  6. ↑ https://handbook.ashrae.org/Handbooks/F17/SI/F17_Ch31/figures/F31sf08.jpg Plots of thermal conductivity vs. temperature for 0, 5, ... 25 w/w NaCl/water solutions. Retrieved 2020-11-27.
  7. ↑ "Thermal conductivity of seawater and its concentrates". twt.mpei.ac.ru. Retrieved 2018-02-16.
  8. ↑ Dittman, Gerald L. (February 16, 1977). "Calculation of Brine Properties". Lawrence Livermore Laboratories. Livermore CA. doi:10.2172/7111583.

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