System: H⁺ - NH₄⁺ - Na⁺ - SO₄²⁻ - NO₃⁻ - Cl⁻ - H₂O

For mixtures, select the method for estimating density from the following properties of the pure aqueous electrolytes:

specific volume, at the total solute mass fraction	Vφ, at constant Im
ρ, at the total solute mass fraction	Vφ, at constant Ix

(Symbol ρ is density, V^φ is apparent molar volume, and I_m and I_x are the molal and mole fraction ionic strength, respectively. The total solute mass fraction is the sum of the mass fractions of all solutes present in the solution. See the methods page for further details.)

Temperature (K):   

Concentration unit:    molality,     molarity,     weight percent.

Enter the ion concentrations:

Notes: volume properties of the individual electrolytes are based on available data, including measurements for supersaturated solutions and extensions to the pure melt (100 wt%) using methods described in ref. (1). The densities of mixtures are estimated by first determining the system composition in term of electrolytes, and then using one of the four methods above to estimate the mixture properties from those of the individual solutes.

System:  H⁺ - NH₄⁺ - HSO₄⁻ - SO₄²⁻ - H₂O, at 298.15 K

Concentration unit:    molality,      molarity,      weight percent of solute.

Total solute concentration:   

Mole fraction of acid in the solute:   

Notes: the total solute concentration (above) is that of the solute (NH₄)_(2-n)H_nSO₄, where 0 ≤ n ≤ 2. The mole fraction of acid in the solute, which specifies the relative amounts of H₂SO₄ and (NH₄)₂SO₄ present, is equal to n/2. For example, n = 1.0 for ammonium bisulphate, NH₄HSO₄. For letovicite ((NH₄)_(1.5)H_0.5SO₄) the mole fraction of acid in the solute is equal to 0.25. The molar mass of letovicite is 123.626 g based upon this formula, and a 1.0 molal solution contains 11.002 wt% of the salt.

System:  NH₄HSO₄ - H₂O, at 298.15 K

Concentration unit:    molality,     molarity,     weight percent of solute.

Solute concentration:   

Notes: the concentration (above) is that of the solute ammonium bisulphate, NH₄HSO₄. The molar mass of NH₄HSO₄ is 115.11 g, and a 1.0 molal solution contains 10.323 wt% of solute. Calculations can be carried out for up 100 wt% of the salt (the hypothetical pure melt).

System:  NaHSO₄ - H₂O, at 298.15 K

Concentration unit:    molality,     molarity,     weight percent of solute.

Solute concentration:   

Notes: the concentration (above) is that of the solute sodium bisulphate, NaHSO₄. The molar mass of NaHSO₄ is 120.061 g, and a 1.0 molal solution contains 10.719 wt% of solute. Calculations can be carried out for up 100 wt% of the salt (the hypothetical pure melt).

System:  NaOH - H₂O, at 298.15 K

Concentration unit:    molality,     molarity,     weight percent of solute.

Solute concentration:   

Notes: the concentration (above) is that of the solute sodium hydroxide, NaOH. The molar mass of NaOH is 39.997 g, and a 1.0 molal solution contains 3.846 wt% of solute. Calculations can be carried out for up 100 wt% of the salt (the hypothetical pure melt).

System:  NH₃ - H₂O, at 298.15 K

Concentration unit:    molality,     molarity,     weight percent of solute.

Solute concentration:   

Notes: the concentration (above) is that of ammonia, NH₃. The molar mass of NH₃ is 17.0306 g, and a 1.0 molal solution contains 1.675 wt% of solute. Calculations can be carried out for up 100 wt% of the solute (the pure liquid).