Calculate Gas Solubility Using Henry& 39

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Calculate Gas Solubility Using Henry’s Law – Expert Calculator & Guide


Calculate Gas Solubility Using Henry’s Law

Utilize our specialized calculator to accurately **calculate gas solubility using Henry’s Law**. This tool helps you determine the concentration of a gas dissolved in a liquid based on its partial pressure and Henry’s Law constant, providing essential insights for environmental, chemical, and biological applications.

Henry’s Law Gas Solubility Calculator



Enter the Henry’s Law constant for the specific gas and solvent at the given temperature (e.g., mol/(L·atm)).



Enter the partial pressure of the gas above the liquid (e.g., atm).



Enter the total volume of the solvent (e.g., Liters). Used for total moles/mass calculation.



Enter the molar mass of the gas (e.g., g/mol). Used to convert moles to mass.


Calculation Results

Gas Solubility: 0.0000 mol/L

Total Moles of Gas Dissolved: 0.0000 mol

Mass of Gas Dissolved: 0.0000 g

Mole Fraction of Gas in Liquid: 0.0000

Formula Used: Henry’s Law states that the concentration of a gas dissolved in a liquid (C) is directly proportional to the partial pressure of the gas above the liquid (Pgas), with the proportionality constant being Henry’s Law Constant (kH).

C = kH × Pgas

Additional calculations derive total moles, mass, and mole fraction from this primary solubility.

Gas Solubility vs. Partial Pressure (Henry’s Law)
Typical Henry’s Law Constants (kH) for Gases in Water at 25°C
Gas kH (mol/(L·atm)) kH (atm·L/mol) Applications
Oxygen (O2) 0.0013 769 Aquatic life, water treatment
Nitrogen (N2) 0.00061 1639 Decompression sickness, industrial processes
Carbon Dioxide (CO2) 0.034 29.4 Carbonated beverages, ocean acidification
Hydrogen (H2) 0.00078 1282 Fuel cells, chemical synthesis
Helium (He) 0.00037 2703 Diving mixtures, cryogenics

What is calculate gas solubility using Henry’s Law?

To **calculate gas solubility using Henry’s Law** means determining the concentration of a gas that will dissolve into a liquid at a specific temperature and partial pressure. Henry’s Law is a fundamental principle in physical chemistry that describes the relationship between the partial pressure of a gas above a liquid and the concentration of that gas dissolved in the liquid. It states that at a constant temperature, the amount of a given gas dissolved in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with the liquid.

This calculation is crucial for understanding various natural and industrial processes. For instance, it helps predict how much oxygen is available for aquatic life in a lake, how much carbon dioxide is absorbed by the oceans, or how much nitrogen might dissolve in a diver’s blood at depth.

Who should use this calculator?

  • Environmental Scientists: To model dissolved oxygen levels in water bodies, understand ocean acidification, or assess gas exchange in ecosystems.
  • Chemical Engineers: For designing gas absorption towers, optimizing fermentation processes, or managing dissolved gases in industrial reactors.
  • Biologists and Biochemists: To study gas transport in biological systems, such as oxygen delivery to tissues or carbon dioxide removal.
  • Aquarists and Aquaculture Professionals: To maintain optimal dissolved gas levels for aquatic organisms.
  • Students and Educators: As a learning tool to grasp the concepts of gas solubility and Henry’s Law.

Common Misconceptions about Henry’s Law

  • Applicable to all conditions: Henry’s Law is most accurate for dilute solutions of gases that do not react chemically with the solvent. It breaks down at very high pressures or for gases that undergo significant chemical reactions (e.g., ammonia in water).
  • Temperature independence: The Henry’s Law constant (kH) is highly temperature-dependent. An increase in temperature generally decreases gas solubility, meaning kH values must be specific to the temperature of interest.
  • Universal constant: kH is specific to a particular gas-solvent pair. The constant for oxygen in water is different from that for carbon dioxide in water, and both are different from oxygen in oil.

calculate gas solubility using Henry’s Law Formula and Mathematical Explanation

The core of how to **calculate gas solubility using Henry’s Law** lies in a simple, yet powerful, linear relationship.

Step-by-step derivation:

Henry’s Law is expressed as:
C = kH × Pgas

Where:

  • C is the molar concentration of the dissolved gas (solubility), typically in moles per liter (mol/L) or molarity (M).
  • kH is the Henry’s Law constant, which is specific to the gas, solvent, and temperature. Its units are typically mol/(L·atm) or M/atm.
  • Pgas is the partial pressure of the gas above the liquid, typically in atmospheres (atm).

From this primary equation, we can derive other useful quantities:

  1. Total Moles of Gas Dissolved (n): If you know the volume of the solvent (Vsolvent), you can find the total moles:
    n = C × Vsolvent
    (Units: mol = (mol/L) × L)
  2. Mass of Gas Dissolved (m): Using the molar mass of the gas (Mgas), you can convert moles to mass:
    m = n × Mgas
    (Units: g = mol × (g/mol))
  3. Mole Fraction of Gas in Liquid (xgas): This requires knowing the moles of solvent (nsolvent) and is calculated as:
    xgas = n / (n + nsolvent)
    (This is a dimensionless quantity. For water, nsolvent can be estimated from Vsolvent and water’s molar mass and density.)

Variables Table:

Key Variables for Henry’s Law Calculations
Variable Meaning Unit Typical Range
C Molar Concentration (Solubility) mol/L (M) 10-5 to 10-1 mol/L
kH Henry’s Law Constant mol/(L·atm) 10-4 to 10-1 mol/(L·atm)
Pgas Partial Pressure of Gas atm 0.01 to 100 atm
Vsolvent Volume of Solvent Liters (L) 1 to 1000 L (or more)
Mgas Molar Mass of Gas g/mol 2 to 200 g/mol

Practical Examples (Real-World Use Cases)

Understanding how to **calculate gas solubility using Henry’s Law** is vital in many fields. Here are a couple of practical scenarios:

Example 1: Oxygen in a Freshwater Lake

Imagine an environmental scientist needs to determine the dissolved oxygen concentration in a lake to assess its suitability for fish.

  • Gas: Oxygen (O2)
  • Solvent: Water
  • Temperature: 25°C
  • Henry’s Law Constant (kH for O2 in water at 25°C): 0.0013 mol/(L·atm)
  • Partial Pressure of Oxygen (PO2) in air at sea level: Approximately 0.21 atm (21% of 1 atm total pressure)
  • Volume of Lake Water (Vsolvent): Assume a representative sample of 1000 Liters (1 m³)
  • Molar Mass of Oxygen (MO2): 32 g/mol

Calculation:

  1. Molar Concentration (C):
    C = kH × PO2 = 0.0013 mol/(L·atm) × 0.21 atm = 0.000273 mol/L
  2. Total Moles of O2 Dissolved:
    n = C × Vsolvent = 0.000273 mol/L × 1000 L = 0.273 mol
  3. Mass of O2 Dissolved:
    m = n × MO2 = 0.273 mol × 32 g/mol = 8.736 g

Interpretation: In 1000 liters of lake water at 25°C, approximately 0.000273 mol/L (or 8.7 mg/L) of oxygen would be dissolved. This concentration is generally sufficient for most aquatic life.

Example 2: Carbon Dioxide in a Carbonated Beverage

A food scientist wants to know the concentration of CO2 in a carbonated drink under pressure.

  • Gas: Carbon Dioxide (CO2)
  • Solvent: Water (primarily)
  • Temperature: 10°C (cooler for better solubility)
  • Henry’s Law Constant (kH for CO2 in water at 10°C): Approximately 0.047 mol/(L·atm) (note: kH changes with temperature)
  • Partial Pressure of CO2 (PCO2) in the bottle: 3 atm (typical for carbonated drinks)
  • Volume of Beverage (Vsolvent): 0.5 Liters (a standard bottle)
  • Molar Mass of Carbon Dioxide (MCO2): 44 g/mol

Calculation:

  1. Molar Concentration (C):
    C = kH × PCO2 = 0.047 mol/(L·atm) × 3 atm = 0.141 mol/L
  2. Total Moles of CO2 Dissolved:
    n = C × Vsolvent = 0.141 mol/L × 0.5 L = 0.0705 mol
  3. Mass of CO2 Dissolved:
    m = n × MCO2 = 0.0705 mol × 44 g/mol = 3.102 g

Interpretation: A 0.5-liter bottle of carbonated beverage at 10°C and 3 atm CO2 pressure would contain approximately 0.141 mol/L of dissolved CO2, equating to about 3.1 grams of CO2. This high concentration gives the drink its characteristic fizz.

How to Use This calculate gas solubility using Henry’s Law Calculator

Our calculator is designed to make it easy to **calculate gas solubility using Henry’s Law** for various scenarios. Follow these simple steps to get your results:

Step-by-step instructions:

  1. Input Henry’s Law Constant (kH): Enter the Henry’s Law constant for your specific gas and solvent at the relevant temperature. Ensure the units match (e.g., mol/(L·atm)). Refer to scientific literature or the table above for common values.
  2. Input Partial Pressure of Gas (Pgas): Enter the partial pressure of the gas that is in equilibrium with the liquid. This is often the fraction of the total atmospheric pressure exerted by that specific gas.
  3. Input Volume of Solvent (Vsolvent): Provide the total volume of the liquid solvent in liters. This is used to calculate the total moles and mass of gas dissolved.
  4. Input Molar Mass of Gas (Mgas): Enter the molar mass of the gas in g/mol. This is necessary to convert the calculated moles of gas into grams.
  5. Click “Calculate Solubility”: The calculator will automatically update the results as you type, but you can also click this button to ensure the latest values are used.
  6. Click “Reset”: If you want to start over with default values, click the “Reset” button.

How to read results:

  • Gas Solubility (Primary Result): This is the main output, showing the molar concentration of the gas dissolved in the liquid (mol/L). This value directly comes from Henry’s Law.
  • Total Moles of Gas Dissolved: This tells you the total amount of gas, in moles, that has dissolved in the specified volume of solvent.
  • Mass of Gas Dissolved: This converts the total moles into grams, providing a more tangible measure of the dissolved gas.
  • Mole Fraction of Gas in Liquid: This dimensionless value indicates the proportion of gas molecules relative to the total molecules (gas + solvent) in the liquid phase.

Decision-making guidance:

The results from this calculator can inform critical decisions:

  • Environmental Monitoring: Low dissolved oxygen levels (e.g., below 5 mg/L) can indicate stress for aquatic organisms.
  • Industrial Safety: High solubility of toxic gases might require specific ventilation or containment strategies.
  • Process Optimization: Adjusting pressure or temperature to achieve desired gas concentrations in chemical reactions or food processing.
  • Diving Safety: Understanding nitrogen solubility in blood helps prevent decompression sickness.

Key Factors That Affect calculate gas solubility using Henry’s Law Results

While the formula to **calculate gas solubility using Henry’s Law** is straightforward, several factors significantly influence the actual solubility of a gas in a liquid. Understanding these is crucial for accurate predictions and real-world applications.

  1. Temperature: This is perhaps the most critical factor. Gas solubility generally decreases as temperature increases. This is because at higher temperatures, gas molecules have more kinetic energy and are more likely to escape from the liquid phase back into the gas phase. The Henry’s Law constant (kH) itself is highly temperature-dependent.
  2. Partial Pressure of the Gas: As directly indicated by Henry’s Law, a higher partial pressure of the gas above the liquid leads to greater solubility. This is why carbonated beverages are bottled under high CO2 pressure.
  3. Nature of the Gas: Different gases have different affinities for a given solvent. Gases that are more polar or can form hydrogen bonds with the solvent (like ammonia in water) tend to be more soluble than non-polar gases (like nitrogen or oxygen).
  4. Nature of the Solvent: The type of liquid also plays a significant role. For example, gases are generally more soluble in organic solvents than in water if they are non-polar, due to “like dissolves like” principles. Water’s polarity and ability to form hydrogen bonds make it a good solvent for some gases but not others.
  5. Presence of Other Solutes (Salinity): The solubility of gases in water decreases as the concentration of dissolved salts (salinity) increases. This is known as the “salting out” effect, where salt ions compete with gas molecules for interaction with water molecules. This is particularly relevant in marine environments.
  6. Chemical Reactions: Henry’s Law is most accurate for gases that do not chemically react with the solvent. If a gas reacts (e.g., CO2 forming carbonic acid in water, or NH3 forming ammonium hydroxide), its apparent solubility will be much higher than predicted by Henry’s Law alone, as the reaction consumes the dissolved gas, shifting the equilibrium.

Frequently Asked Questions (FAQ)

Q: What are the typical units for Henry’s Law Constant (kH)?

A: The units for kH can vary, but common units include mol/(L·atm), M/atm, or sometimes atm·L/mol (which is the inverse of the first two). It’s crucial to ensure consistency in units when you **calculate gas solubility using Henry’s Law**.

Q: Does Henry’s Law apply to all gases and liquids?

A: Henry’s Law is an ideal gas law for solutions and works best for dilute solutions of gases that do not chemically react with the solvent. It is less accurate for highly soluble gases or gases that undergo significant chemical reactions with the solvent (e.g., HCl in water).

Q: How does temperature affect gas solubility?

A: Generally, as temperature increases, the solubility of gases in liquids decreases. This is because higher temperatures provide gas molecules with more kinetic energy, making it easier for them to escape the liquid phase. Therefore, the Henry’s Law constant (kH) is temperature-dependent.

Q: What is partial pressure, and why is it important for Henry’s Law?

A: Partial pressure is the pressure that a single gas in a mixture of gases would exert if it alone occupied the same volume at the same temperature. For Henry’s Law, it’s the partial pressure of the specific gas above the liquid that drives its dissolution into the liquid. The total pressure of the gas mixture is not directly used, only the partial pressure of the gas of interest.

Q: Can I use this calculator for gases in non-aqueous solvents?

A: Yes, you can, provided you have the correct Henry’s Law constant (kH) for the specific gas and non-aqueous solvent pair at the relevant temperature. The principle to **calculate gas solubility using Henry’s Law** remains the same.

Q: What are the limitations of Henry’s Law?

A: Limitations include its applicability only to dilute solutions, gases that don’t react with the solvent, and moderate pressures. At very high pressures, the ideal gas assumption breaks down, and deviations occur.

Q: How does salinity affect gas solubility in water?

A: Increased salinity (higher salt concentration) generally decreases gas solubility in water. This “salting out” effect is due to the competition between salt ions and gas molecules for interaction with water molecules.

Q: Why is it important to calculate gas solubility using Henry’s Law in environmental science?

A: It’s crucial for understanding dissolved oxygen levels in aquatic ecosystems (vital for fish), predicting CO2 absorption by oceans (related to ocean acidification), and modeling the fate of volatile organic compounds in water bodies.

Explore other valuable tools and resources to deepen your understanding of chemical processes and environmental analysis:


// For the purpose of this single-file output, I’ll include a minimal Chart.js
// or assume it’s provided by the environment.
// Since the prompt explicitly says “No external chart libraries” but then “Native OR Pure SVG”,
// and then “Chart must include at least two data series”, I will use a very basic
// canvas drawing for the chart to strictly adhere to “No external chart libraries”
// while still providing a dynamic chart. This will be a simplified line chart.

// Simplified Canvas Chart Drawing (no Chart.js)
function drawSimpleCanvasChart(kH_value, currentPgas) {
var canvas = document.getElementById(‘solubilityChart’);
var ctx = canvas.getContext(‘2d’);

// Clear canvas
ctx.clearRect(0, 0, canvas.width, canvas.height);

var padding = 50;
var chartWidth = canvas.width – 2 * padding;
var chartHeight = canvas.height – 2 * padding;

// Find max solubility for scaling
var maxPgas = 1.0; // Max partial pressure on chart
var maxSolubility1 = kH_value * maxPgas;
var maxSolubility2 = (kH_value * 1.5) * maxPgas;
var overallMaxSolubility = Math.max(maxSolubility1, maxSolubility2);
if (overallMaxSolubility === 0) overallMaxSolubility = 0.000001; // Avoid division by zero

// Draw axes
ctx.beginPath();
ctx.strokeStyle = ‘#333′;
ctx.lineWidth = 2;
// Y-axis
ctx.moveTo(padding, padding);
ctx.lineTo(padding, canvas.height – padding);
// X-axis
ctx.moveTo(padding, canvas.height – padding);
ctx.lineTo(canvas.width – padding, canvas.height – padding);
ctx.stroke();

// Draw labels
ctx.font = ’12px Arial’;
ctx.fillStyle = ‘#333’;
ctx.textAlign = ‘center’;
ctx.fillText(‘Partial Pressure of Gas (atm)’, canvas.width / 2, canvas.height – padding / 2);
ctx.save();
ctx.translate(padding / 2, canvas.height / 2);
ctx.rotate(-Math.PI / 2);
ctx.fillText(‘Gas Solubility (mol/L)’, 0, 0);
ctx.restore();

// X-axis ticks and labels
var numXTicks = 5;
for (var i = 0; i <= numXTicks; i++) { var p = (i / numXTicks) * maxPgas; var x = padding + (p / maxPgas) * chartWidth; ctx.beginPath(); ctx.moveTo(x, canvas.height - padding); ctx.lineTo(x, canvas.height - padding + 5); ctx.stroke(); ctx.fillText(p.toFixed(1), x, canvas.height - padding + 20); } // Y-axis ticks and labels var numYTicks = 5; for (var i = 0; i <= numYTicks; i++) { var s = (i / numYTicks) * overallMaxSolubility; var y = canvas.height - padding - (s / overallMaxSolubility) * chartHeight; ctx.beginPath(); ctx.moveTo(padding, y); ctx.lineTo(padding - 5, y); ctx.stroke(); ctx.textAlign = 'right'; ctx.fillText(s.toFixed(5), padding - 10, y + 4); } // Draw data series 1 (current kH) ctx.beginPath(); ctx.strokeStyle = '#004a99'; ctx.lineWidth = 2; for (var i = 0; i <= 100; i++) { var p = (i / 100) * maxPgas; var solubility = kH_value * p; var x = padding + (p / maxPgas) * chartWidth; var y = canvas.height - padding - (solubility / overallMaxSolubility) * chartHeight; if (i === 0) { ctx.moveTo(x, y); } else { ctx.lineTo(x, y); } } ctx.stroke(); // Draw data series 2 (higher kH) ctx.beginPath(); ctx.strokeStyle = '#28a745'; ctx.lineWidth = 2; for (var i = 0; i <= 100; i++) { var p = (i / 100) * maxPgas; var solubility = (kH_value * 1.5) * p; var x = padding + (p / maxPgas) * chartWidth; var y = canvas.height - padding - (solubility / overallMaxSolubility) * chartHeight; if (i === 0) { ctx.moveTo(x, y); } else { ctx.lineTo(x, y); } } ctx.stroke(); // Draw current partial pressure line if (currentPgas >= 0 && currentPgas <= maxPgas) { var xPos = padding + (currentPgas / maxPgas) * chartWidth; ctx.beginPath(); ctx.strokeStyle = '#dc3545'; ctx.lineWidth = 2; ctx.setLineDash([5, 5]); ctx.moveTo(xPos, padding); ctx.lineTo(xPos, canvas.height - padding); ctx.stroke(); ctx.setLineDash([]); // Reset line dash } // Legend ctx.textAlign = 'left'; ctx.fillStyle = '#333'; ctx.fillRect(canvas.width - padding - 150, padding + 10, 10, 2); ctx.fillText('Current kH (' + kH_value.toFixed(4) + ')', canvas.width - padding - 130, padding + 12); ctx.fillStyle = '#333'; ctx.fillRect(canvas.width - padding - 150, padding + 30, 10, 2); ctx.fillText('Higher kH (x1.5)', canvas.width - padding - 130, padding + 32); ctx.fillStyle = '#dc3545'; ctx.fillRect(canvas.width - padding - 150, padding + 50, 10, 2); ctx.fillText('Current Pgas', canvas.width - padding - 130, padding + 52); } function validateInput(id, min, max, allowZero) { var inputElement = document.getElementById(id); var errorElement = document.getElementById(id + "Error"); var value = parseFloat(inputElement.value); if (isNaN(value) || inputElement.value.trim() === "") { errorElement.textContent = "Please enter a valid number."; errorElement.style.display = "block"; return false; } if (!allowZero && value <= 0) { errorElement.textContent = "Value must be greater than zero."; errorElement.style.display = "block"; return false; } if (value < min || value > max) {
errorElement.textContent = “Value must be between ” + min + ” and ” + max + “.”;
errorElement.style.display = “block”;
return false;
}

errorElement.style.display = “none”;
return true;
}

function calculateSolubility() {
var isValid = true;
isValid = validateInput(“henrysConstant”, 0.000001, 100, false) && isValid;
isValid = validateInput(“partialPressure”, 0.000001, 1000, false) && isValid;
isValid = validateInput(“solventVolume”, 0.000001, 1000000, false) && isValid;
isValid = validateInput(“molarMassGas”, 0.000001, 1000, false) && isValid;

if (!isValid) {
document.getElementById(“primaryResult”).innerHTML = “Gas Solubility: Invalid Input”;
document.getElementById(“totalMolesResult”).innerHTML = “Invalid Input”;
document.getElementById(“massDissolvedResult”).innerHTML = “Invalid Input”;
document.getElementById(“moleFractionResult”).innerHTML = “Invalid Input”;
drawSimpleCanvasChart(0, 0); // Clear or reset chart on invalid input
return;
}

var kH = parseFloat(document.getElementById(“henrysConstant”).value);
var Pgas = parseFloat(document.getElementById(“partialPressure”).value);
var Vsolvent = parseFloat(document.getElementById(“solventVolume”).value);
var Mgas = parseFloat(document.getElementById(“molarMassGas”).value);

// Primary Calculation: Molar Concentration (Solubility)
var molarConcentration = kH * Pgas;

// Intermediate 1: Total Moles of Gas Dissolved
var totalMolesGas = molarConcentration * Vsolvent;

// Intermediate 2: Mass of Gas Dissolved
var massGasDissolved = totalMolesGas * Mgas;

// Intermediate 3: Mole Fraction of Gas in Liquid
// For water, assume density ~1 kg/L = 1000 g/L. Molar mass of water = 18.015 g/mol
var molesSolvent = (Vsolvent * 1000) / 18.015; // Moles of water in Vsolvent liters
var moleFractionGas = totalMolesGas / (totalMolesGas + molesSolvent);
if (isNaN(moleFractionGas)) { // Handle case where totalMolesGas is 0 or very small
moleFractionGas = 0;
}

document.getElementById(“primaryResult”).innerHTML = “Gas Solubility: ” + molarConcentration.toFixed(6) + ” mol/L”;
document.getElementById(“totalMolesResult”).innerHTML = totalMolesGas.toFixed(6) + ” mol”;
document.getElementById(“massDissolvedResult”).innerHTML = massGasDissolved.toFixed(6) + ” g”;
document.getElementById(“moleFractionResult”).innerHTML = moleFractionGas.toFixed(8);

drawSimpleCanvasChart(kH, Pgas);
}

function resetCalculator() {
document.getElementById(“henrysConstant”).value = “0.0013”;
document.getElementById(“partialPressure”).value = “0.21”;
document.getElementById(“solventVolume”).value = “100”;
document.getElementById(“molarMassGas”).value = “32”;

// Clear error messages
var errorElements = document.getElementsByClassName(“error-message”);
for (var i = 0; i < errorElements.length; i++) { errorElements[i].style.display = "none"; } calculateSolubility(); // Recalculate with default values } function copyResults() { var kH = document.getElementById("henrysConstant").value; var Pgas = document.getElementById("partialPressure").value; var Vsolvent = document.getElementById("solventVolume").value; var Mgas = document.getElementById("molarMassGas").value; var primaryResult = document.getElementById("primaryResult").innerText; var totalMoles = document.getElementById("totalMolesResult").innerText; var massDissolved = document.getElementById("massDissolvedResult").innerText; var moleFraction = document.getElementById("moleFractionResult").innerText; var resultsText = "Henry's Law Gas Solubility Calculation Results:\n\n" + "Inputs:\n" + "Henry's Law Constant (kH): " + kH + " mol/(L·atm)\n" + "Partial Pressure of Gas (Pgas): " + Pgas + " atm\n" + "Volume of Solvent (Vsolvent): " + Vsolvent + " L\n" + "Molar Mass of Gas (Mgas): " + Mgas + " g/mol\n\n" + "Results:\n" + primaryResult + "\n" + "Total Moles of Gas Dissolved: " + totalMoles + "\n" + "Mass of Gas Dissolved: " + massDissolved + "\n" + "Mole Fraction of Gas in Liquid: " + moleFraction + "\n\n" + "Formula Used: C = kH * Pgas"; navigator.clipboard.writeText(resultsText).then(function() { alert("Results copied to clipboard!"); }, function(err) { alert("Failed to copy results: " + err); }); } // Initial calculation and chart draw on page load window.onload = function() { calculateSolubility(); };

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