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Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same Solution

STEP 0: Pre-Calculation Summary
Formula Used
ionic_strength = 15*Molality
I = 15*m
This formula uses 1 Variables
Variables Used
Molality - Molality is defined as the total number of moles of solute per kilograms of solvent present in the solution. (Measured in Mole per Kilogram)
STEP 1: Convert Input(s) to Base Unit
Molality: 0.034 Mole per Kilogram --> 0.034 Mole per Kilogram No Conversion Required
STEP 2: Evaluate Formula
Substituting Input Values in Formula
I = 15*m --> 15*0.034
Evaluating ... ...
I = 0.51
STEP 3: Convert Result to Output's Unit
0.51 Mole per Kilogram --> No Conversion Required
FINAL ANSWER
0.51 Mole per Kilogram <-- Ionic strength
(Calculation completed in 00.000 seconds)

11 Other formulas that you can solve using the same Inputs

Molarity when molality of solution is given
molarity_when_molality_of_solution_is_given = (Molality*Density of solution*1000)/(1000+( Molality*Molar mass of solute)) Go
Mole Fraction Using Molality
mole_fraction_solute = (Molality*Molar Mass Of The Solvent)/(1000+Molality*Molar Mass Of The Solvent) Go
Density of solution when molarity and molality is given
density_of_solution = (Molarity/(Molality*1000))*(1000+(Molar mass of solvent*Molality)) Go
Molarity Using Molality
molarity = (molarity*Density*1000)/(1000+Molality*Molar Mass of the Solute) Go
Molal Boiling Point Elevation Constant when Boiling Point Elevation is Given
molal_boiling_point_elevation_constant = Boiling Point Elevation/Molality Go
Boiling Point Elevation
boiling_point_elevation = Molal Boiling Point Elevation Constant*Molality Go
Mole fraction of solvent when molality is given
mole_fraction_of_solvent = 1000/(1000+(Molality*Molar mass of solvent)) Go
Molal freezing point constant when freezing point depression is given
molal_freezing_point_constant = Freezing point depression/Molality Go
Freezing Point Depression
freezing_point_depression = Molal freezing point constant*Molality Go
Number of moles of solute using molality
number_of_moles_of_solute = Molality*Mass Of Solvent Go
Mass of solvent using molality
mass_of_solvent = Number of Moles of Solute/Molality Go

6 Other formulas that calculate the same Output

Ionic strength of uni-bivalent electrolyte
ionic_strength = (1/2)*(Molality of cation*((Valencies of cation)^2)+(2*Molality of anion*((Valencies of anion)^2))) Go
Ionic strength of bi-trivalent electrolyte
ionic_strength = (1/2)*(2*Molality of cation*((Valencies of cation)^2)+3*Molality of anion*((Valencies of anion)^2)) Go
Ionic strength for uni-univalent electrolyte
ionic_strength = (1/2)*(Molality of cation*((Valencies of cation)^2)+Molality of anion*((Valencies of anion)^2)) Go
Ionic strength for bi-bivalent electrolyte
ionic_strength = (1/2)*(Molality of cation*((Valencies of cation)^2)+Molality of anion*((Valencies of anion)^2)) Go
Ionic strength for bi-bivalent electrolyte if molality of cation and anion is same
ionic_strength = (4*Molality) Go
Ionic strength of uni-bivalent electrolyte if molality of cation and anion are same
ionic_strength = 3*Molality Go

Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same Formula

ionic_strength = 15*Molality
I = 15*m

What is Ionic Strength?

Ionic Strength of a solution is a measure of the electrical intensity due to the presence of ions in the solution. It is given as half of the sum of all the terms obtained by multiplying the molality of each ion by the square of its valency. In other words, ionic strength is the cumulative measure of both charges on the ion as well as its concentration in the solution. The concept of ionic strength is always applicable to strong electrolytes (i.e salts) and it cannot be applied to weak electrolytes.

How to Calculate Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same?

Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same calculator uses ionic_strength = 15*Molality to calculate the Ionic strength, The Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same formula is defined as fifteen times the molality of a bi-trivalent electrolyte. Ionic strength and is denoted by I symbol.

How to calculate Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same using this online calculator? To use this online calculator for Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same, enter Molality (m) and hit the calculate button. Here is how the Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same calculation can be explained with given input values -> 0.51 = 15*0.034.

FAQ

What is Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same?
The Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same formula is defined as fifteen times the molality of a bi-trivalent electrolyte and is represented as I = 15*m or ionic_strength = 15*Molality. Molality is defined as the total number of moles of solute per kilograms of solvent present in the solution.
How to calculate Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same?
The Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same formula is defined as fifteen times the molality of a bi-trivalent electrolyte is calculated using ionic_strength = 15*Molality. To calculate Ionic strength of bi-trivalent electrolyte if molality of cation and anion are same, you need Molality (m). With our tool, you need to enter the respective value for Molality and hit the calculate button. You can also select the units (if any) for Input(s) and the Output as well.
How many ways are there to calculate Ionic strength?
In this formula, Ionic strength uses Molality. We can use 6 other way(s) to calculate the same, which is/are as follows -
  • ionic_strength = (1/2)*(Molality of cation*((Valencies of cation)^2)+Molality of anion*((Valencies of anion)^2))
  • ionic_strength = (1/2)*(Molality of cation*((Valencies of cation)^2)+Molality of anion*((Valencies of anion)^2))
  • ionic_strength = (4*Molality)
  • ionic_strength = (1/2)*(Molality of cation*((Valencies of cation)^2)+(2*Molality of anion*((Valencies of anion)^2)))
  • ionic_strength = 3*Molality
  • ionic_strength = (1/2)*(2*Molality of cation*((Valencies of cation)^2)+3*Molality of anion*((Valencies of anion)^2))
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