# Difference between revisions of "Ionic Strength"

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Where n is the number of charged species. | Where n is the number of charged species. | ||

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+ | == Converting from Mole fraction to Molal-based units == | ||

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+ | The equation to use is the following: | ||

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[[user:DMILLER | Author: Diana Miller]] | [[user:DMILLER | Author: Diana Miller]] |

## Revision as of 05:53, 7 September 2022

# Ionic Strength (molal based or m-based)

The ionic strength is a quantity representing the strength of the electric field in a solution, and it is equal to the sum of the molalities of each type of ion present multiplied by the square of their charges, as represented by the following equation:

Where n is the number of charged species.

For example, a 1.0 molar solution of NaCl has 1.0 moles of Na^+ions and 1.0 moles of Cl^- ions in 1 kg of H2O. Therefore, the ionic strength is 1.0 molal.

Now, consider a 1.0 molal solution of CaCl2. This solution has 1.0 moles of Ca^(+2) ions and 2.0 moles of Cl^- ions in 1 kg of H2O. Therefore, the ionic strength is 3.0 molar, or it can be said that a 1.0 molal solution of CaCl2 behaves similar to a 3.0 molar solution of NaCl.

# Ionic Strength (mole fraction based or x-based)

In this case the ionic strength is calculated using the mole fraction rather than the molality:

Where n is the number of charged species.

## Converting from Mole fraction to Molal-based units

The equation to use is the following: