Simplify and analyze chemical reactions by visualizing ionic species.
Ionic Equation Calculator
Calculation Results
Enter reaction details
Reactants (Full):—
Products (Full):—
Total Ions (Reactants):—
Total Ions (Products):—
Spectator Ions:—
Net Ionic Equation:—
Formula Used:
The process involves identifying all soluble ionic compounds and strong acids/bases in the balanced molecular equation and dissociating them into their constituent ions. Spectator ions (ions that appear unchanged on both sides) are then removed to yield the net ionic equation, showing only the species that participate in the reaction.
Understanding Ionic Equations
What is an Ionic Equation?
An ionic equation is a chemical equation that shows dissolved ionic compounds, strong acids, and strong bases as dissociated ions. It is a crucial tool in chemistry for understanding reactions in aqueous solutions. There are two main types: the complete ionic equation, which lists all ions present, and the net ionic equation, which shows only the ions that actually react. This ionic equation calculator helps simplify the process of generating and understanding these equations.
Who should use it?
This calculator and guide are designed for high school and college chemistry students, educators, researchers, and anyone working with chemical reactions in aqueous solutions. It's particularly useful for those studying stoichiometry, precipitation reactions, acid-base reactions, and redox reactions where understanding the behavior of ions is paramount.
Common Misconceptions
All compounds dissociate: Not all compounds break into ions in water. Molecular compounds (like sugar) and insoluble ionic compounds generally do not dissociate.
Net ionic equation is always simple: While spectator ions are removed, the remaining species might still involve complex ions or polyatomic ions that remain intact.
Ionic equations apply everywhere: They are primarily used for reactions occurring in aqueous solutions. Reactions in gases, solids, or non-polar solvents are typically represented by molecular equations.
Ionic Equation Formula and Mathematical Explanation
The process of deriving an ionic equation from a molecular equation involves several key steps. While there isn't a single numerical formula like in finance, it's a systematic procedure based on chemical principles.
Step-by-Step Derivation:
Write the Balanced Molecular Equation: This is the starting point, showing the complete chemical formulas of reactants and products.
Identify Soluble Ionic Compounds, Strong Acids, and Strong Bases: Use solubility rules and knowledge of strong electrolytes. These are the species that will dissociate.
Write the Complete Ionic Equation: Dissociate all identified soluble species into their constituent ions. Keep insoluble solids, liquids, and gases as their molecular formulas.
Identify and Cancel Spectator Ions: Spectator ions are ions that appear in the exact same form on both the reactant and product sides of the complete ionic equation.
Write the Net Ionic Equation: This is the final equation, consisting only of the species that have changed chemically.
Variable Explanations (Conceptual):
In the context of ionic equations, "variables" refer to the chemical species involved and their quantities (coefficients).
Key Components in Ionic Equation Derivation
Component
Meaning
Unit
Typical Range/State
Reactant Formulas
Chemical formulas of starting substances (e.g., NaCl, H2SO4).
Chemical Formula
Valid chemical formulas
Product Formulas
Chemical formulas of substances formed (e.g., AgCl, KNO3).
Chemical Formula
Valid chemical formulas
Coefficients
Numbers preceding chemical formulas in a balanced equation, indicating molar ratios.
Integer (mole ratio)
≥ 1 (for balanced equations)
Dissociated Ions
Individual charged species formed when soluble ionic compounds, strong acids, or strong bases dissolve in water (e.g., Na+, Cl-, H+, SO4^2-).
Ion Formula with Charge
Various cations and anions
Spectator Ions
Ions present on both sides of the complete ionic equation without participating in the net reaction.
Ion Formula with Charge
Specific ions determined by the reaction
Net Ionic Equation Species
Ions or molecules that actively participate in the chemical change.
Chemical Formula / Ion Formula
Species undergoing reaction
Practical Examples (Real-World Use Cases)
Example 1: Precipitation Reaction
Consider the reaction between aqueous silver nitrate and aqueous sodium chloride.
Interpretation: When solutions of sodium chloride and silver nitrate are mixed, solid silver chloride precipitates out. The sodium ions (Na⁺) and nitrate ions (NO₃⁻) remain dissolved and do not participate directly in the formation of the precipitate; they are spectator ions.
Example 2: Acid-Base Neutralization
Consider the reaction between hydrochloric acid and sodium hydroxide.
Interpretation: This is a classic neutralization reaction. The hydrogen ions (H⁺) from the acid react with the hydroxide ions (OH⁻) from the base to form water. Sodium ions (Na⁺) and chloride ions (Cl⁻) are spectator ions, remaining dissolved in the solution.
How to Use This Ionic Equation Calculator
Enter Reactants and Products: Input the correct chemical formulas for all reactants and products involved in the reaction. Ensure you specify the state symbols (aq, s, l, g).
Input Coefficients: Enter the stoichiometric coefficients for each reactant and product as determined by the balanced molecular equation.
Click Calculate: Press the "Calculate Ionic Equation" button.
Review Results: The calculator will display the full ionic equation components, identify spectator ions, and present the net ionic equation.
How to Read Results:
Primary Result: This is the Net Ionic Equation, showing the core chemical transformation.
Spectator Ions: These are ions that appear unchanged on both sides and are not part of the net reaction.
Full Equations: These show all dissociated ions and undissociated species.
Decision-Making Guidance: Understanding the net ionic equation helps predict reaction outcomes, identify the actual reacting species, and is fundamental for quantitative analysis (stoichiometry) in solution chemistry.
Key Factors That Affect Ionic Equation Results
Solubility Rules: The most critical factor. Whether a compound is soluble or insoluble in water dictates whether it dissociates into ions or remains as a solid precipitate. Incorrect application of solubility rules leads to wrong ionic and net ionic equations.
Strength of Acids and Bases: Strong acids (like HCl, H₂SO₄) and strong bases (like NaOH, KOH) completely dissociate in water and are written as ions. Weak acids and bases only partially dissociate and are typically written in their molecular form.
State Symbols: Accurately indicating the physical state (aq, s, l, g) is essential. Only aqueous (aq) ionic compounds, strong acids, and strong bases are dissociated. Solids (s), liquids (l), and gases (g) are written as their molecular formulas.
Balancing of the Molecular Equation: The coefficients in the balanced molecular equation are crucial for correctly identifying the molar ratios of ions and for cancelling spectator ions accurately. An unbalanced equation will lead to incorrect ionic equations.
Polyatomic Ions: Polyatomic ions (like SO₄²⁻, NO₃⁻, NH₄⁺) often remain intact even when the compound they are part of dissociates. They should be treated as single units and not broken down further unless they are involved in a specific reaction where they decompose.
Complex Ion Formation: In some cases, ions can react with other species in solution to form complex ions (e.g., [Ag(NH₃)₂]⁺). These complex ions are typically written as a single entity in ionic equations.
Frequently Asked Questions (FAQ)
Q1: What's the difference between a molecular equation and an ionic equation?
A: A molecular equation shows all reactants and products as neutral compounds. An ionic equation breaks down soluble ionic compounds, strong acids, and strong bases into their constituent ions, focusing on the species actually involved in the reaction.
Q2: How do I know if an ionic compound is soluble?
A: You need to consult a set of solubility rules. For example, most nitrate (NO₃⁻) salts and salts of Group 1 elements (like NaCl, KNO₃) are soluble.
Q3: What are spectator ions?
A: Spectator ions are ions that are present in the reactant and product solutions but do not participate in the chemical reaction. They appear unchanged on both sides of the complete ionic equation.
Q4: Can polyatomic ions be spectator ions?
A: Yes, if a polyatomic ion appears in the same form on both sides of the complete ionic equation, it is a spectator ion (e.g., NO₃⁻ in the NaCl + AgNO₃ reaction).
Q5: What if a product is a gas?
A: Gases (like CO₂, H₂S) are written in their molecular form in all types of equations (molecular, complete ionic, net ionic) because they do not exist as dissociated ions in solution.
Q6: How does this calculator handle weak acids/bases?
A: This calculator assumes strong electrolytes for simplicity. For weak acids/bases, you would typically write them in their molecular form in the complete ionic equation, as they do not fully dissociate.
Q7: What is the purpose of the net ionic equation?
A: It highlights the essential chemical change occurring, stripping away the non-reactive spectator ions. This simplifies the understanding of reactions like precipitation and neutralization.
Q8: Can I use this calculator for redox reactions?
A: While this calculator focuses on dissociation and spectator ions, the principles apply. However, redox reactions involve electron transfer, which requires a separate analysis beyond simple ion identification.
Related Tools and Internal Resources
Stoichiometry Calculator: Use calculated ionic equations to perform mole-based calculations for reactants and products.
Molar Mass Calculator: Determine the molar mass of compounds and ions involved in your reactions.
pH Calculator: Analyze the acidity or basicity of solutions, especially relevant for acid-base reactions.
Solubility Rules Guide: A detailed reference to help determine the solubility of ionic compounds.
function getElement(id) {
return document.getElementById(id);
}
function validateInput(id, errorId, minVal, maxVal, isFormula) {
var input = getElement(id);
var errorDiv = getElement(errorId);
var value = input.value.trim();
if (value === "") {
errorDiv.textContent = "This field cannot be empty.";
return false;
}
if (isFormula) {
// Basic check for formula format – can be expanded
if (!/^[A-Za-z0-9()]+(aq|s|l|g)$/.test(value)) {
errorDiv.textContent = "Invalid chemical formula format (e.g., NaCl(aq)).";
return false;
}
} else {
var numValue = parseFloat(value);
if (isNaN(numValue)) {
errorDiv.textContent = "Please enter a valid number.";
return false;
}
if (numValue maxVal) {
errorDiv.textContent = "Value cannot be greater than " + maxVal + ".";
return false;
}
}
errorDiv.textContent = "";
return true;
}
function parseFormula(formula) {
var ions = [];
var state = formula.slice(-3); // e.g., (aq)
var formulaBody = formula.slice(0, -4); // e.g., NaCl
// Very basic parsing – assumes simple ionic compounds for now
// Needs significant expansion for polyatomic ions, complex molecules etc.
if (formulaBody.includes('(') && formulaBody.includes(')')) {
// Handle polyatomic ions – simplified
var parts = formulaBody.match(/([A-Z][a-z]*)(\d*)|(\([A-Za-z0-9]+\))(\d*)/g);
if (parts) {
parts.forEach(function(part) {
var match = part.match(/(\(?([A-Z][a-z]*)(\d*)\)?)([1-9]?)/);
if (match) {
var elementOrGroup = match[2] || match[3]; // Element or polyatomic group
var count = match[4] ? parseInt(match[4]) : 1;
// This is a placeholder – actual ion charge needs lookup
ions.push({ element: elementOrGroup, count: count, charge: '?' });
}
});
}
} else {
// Simple elements
var elements = formulaBody.match(/([A-Z][a-z]*)(\d*)/g);
if (elements) {
elements.forEach(function(elementPart) {
var match = elementPart.match(/([A-Z][a-z]*)(\d*)/);
if (match) {
var element = match[1];
var count = match[2] ? parseInt(match[2]) : 1;
// Placeholder for charge
ions.push({ element: element, count: count, charge: '?' });
}
});
}
}
return { ions: ions, state: state };
}
function getIonsFromFormula(formula) {
// Simplified logic: Assumes common ionic compounds and strong acids/bases
// This needs a robust lookup table for real-world accuracy
var parts = formula.match(/^([A-Za-z0-9]+)(\(aq\)| \(s\)| \(l\)| \(g\))$/);
if (!parts) return { ions: [], state: null, isElectrolyte: false };
var compound = parts[1];
var state = parts[2].trim();
var isElectrolyte = false;
var dissociatedIons = [];
if (state !== '(aq)') {
return { ions: [{ formula: compound, state: state }], state: state, isElectrolyte: false };
}
// Basic solubility and strong electrolyte checks (INCOMPLETE – needs proper tables)
if (compound.includes('NO3') || compound.includes('ClO3') || compound.includes('ClO4')) isElectrolyte = true; // Nitrates, Chlorates, Perchlorates
if (compound.includes('NH4')) isElectrolyte = true; // Ammonium
if (compound.startsWith('Na') || compound.startsWith('K') || compound.startsWith('Li')) isElectrolyte = true; // Group 1 metals
if (compound.startsWith('Ag') && !compound.includes('NO3')) { /* Silver salts often insoluble */ }
else if (compound.startsWith('Pb') && !compound.includes('NO3')) { /* Lead salts often insoluble */ }
else if (compound.startsWith('Cl') || compound.startsWith('Br') || compound.startsWith('I')) {
if (!compound.includes('Ag') && !compound.includes('Pb') && !compound.includes('Hg')) isElectrolyte = true; // Halides (except with Ag, Pb, Hg)
}
else if (compound.startsWith('SO4')) {
if (!compound.includes('Ba') && !compound.includes('Sr') && !compound.includes('Pb') && !compound.includes('Ca')) isElectrolyte = true; // Sulfates (except with Ba, Sr, Pb, Ca)
}
// Strong Acids (HCl, HBr, HI, HNO3, H2SO4, HClO4)
if (compound.startsWith('H') && (compound.includes('Cl') || compound.includes('Br') || compound.includes('I') || compound.includes('NO3') || compound.includes('SO4') || compound.includes('ClO4'))) {
isElectrolyte = true;
}
// Strong Bases (Group 1 & heavy Group 2 hydroxides)
if (compound.startsWith('O') && (compound.includes('H') || compound.includes('OH'))) { // Simplified check for OH
if (compound.startsWith('LiOH') || compound.startsWith('NaOH') || compound.startsWith('KOH') || compound.startsWith('RbOH') || compound.startsWith('CsOH') || compound.startsWith('Ca(OH)2') || compound.startsWith('Sr(OH)2') || compound.startsWith('Ba(OH)2')) {
isElectrolyte = true;
}
}
if (isElectrolyte) {
// Attempt to parse into ions – VERY SIMPLIFIED
var ionMatch = compound.match(/([A-Z][a-z]*)(\d*)|(\([A-Za-z0-9]+\))(\d*)/g);
if (ionMatch) {
ionMatch.forEach(function(part) {
var elementOrGroup = part.replace(/\d/g, "); // Remove numbers for basic name
var countStr = part.match(/\d+$/);
var count = countStr ? parseInt(countStr[0]) : 1;
// Determine charge – highly simplified, needs proper lookup
var charge = '?';
if (elementOrGroup === 'Na') charge = '+';
else if (elementOrGroup === 'K') charge = '+';
else if (elementOrGroup === 'Ag') charge = '+';
else if (elementOrGroup === 'Cl') charge = '-';
else if (elementOrGroup === 'NO3') charge = '-';
else if (elementOrGroup === 'H') charge = '+';
else if (elementOrGroup === 'OH') charge = '-';
else if (elementOrGroup === 'Ca') charge = '+2';
else if (elementOrGroup === 'SO4') charge = '-2';
dissociatedIons.push({ formula: elementOrGroup, count: count, charge: charge, state: '(aq)' });
});
}
} else {
// Not an electrolyte, keep as is
dissociatedIons.push({ formula: compound, state: state });
}
return { ions: dissociatedIons, state: state, isElectrolyte: isElectrolyte };
}
function calculateIonicEquation() {
var r1 = getElement("reactant1").value;
var r2 = getElement("reactant2").value;
var p1 = getElement("product1").value;
var p2 = getElement("product2").value;
var c1 = parseInt(getElement("coefficient1").value);
var c2 = parseInt(getElement("coefficient2").value);
var c3 = parseInt(getElement("coefficient3").value);
var c4 = parseInt(getElement("coefficient4").value);
// Validation
var valid = true;
valid &= validateInput("reactant1", "reactant1Error", 0, 0, true);
valid &= validateInput("reactant2", "reactant2Error", 0, 0, true);
valid &= validateInput("product1", "product1Error", 0, 0, true);
valid &= validateInput("product2", "product2Error", 0, 0, true);
valid &= validateInput("coefficient1", "coefficient1Error", 1);
valid &= validateInput("coefficient2", "coefficient2Error", 1);
valid &= validateInput("coefficient3", "coefficient3Error", 1);
valid &= validateInput("coefficient4", "coefficient4Error", 1);
if (!valid) {
getElement("primaryResult").textContent = "Please correct the errors.";
return;
}
var fullReactants = [];
var fullProducts = [];
var allReactantIons = [];
var allProductIons = [];
var spectatorIons = [];
var netEquationParts = [];
var reactants = [{ formula: r1, coeff: c1 }, { formula: r2, coeff: c2 }];
var products = [{ formula: p1, coeff: c3 }, { formula: p2, coeff: c4 }];
// Process Reactants
reactants.forEach(function(item) {
var parsed = getIonsFromFormula(item.formula);
var speciesString = item.formula;
if (parsed.isElectrolyte) {
var ionStrings = [];
parsed.ions.forEach(function(ion) {
var ionFormula = ion.formula + (ion.count > 1 ? ion.count : ");
var ionCharge = ion.charge !== '?' ? ion.charge : ";
var ionFull = ionFormula + ionCharge + ion.state;
for (var i = 0; i < item.coeff * ion.count; i++) {
allReactantIons.push(ionFull);
ionStrings.push(ionFull);
}
});
fullReactants.push(ionStrings.join(' + '));
} else {
fullReactants.push(speciesString);
for (var i = 0; i 1 ? ion.count : ");
var ionCharge = ion.charge !== '?' ? ion.charge : ";
var ionFull = ionFormula + ionCharge + ion.state;
for (var i = 0; i < item.coeff * ion.count; i++) {
allProductIons.push(ionFull);
ionStrings.push(ionFull);
}
});
fullProducts.push(ionStrings.join(' + '));
} else {
fullProducts.push(speciesString);
for (var i = 0; i < item.coeff; i++) {
allProductIons.push(speciesString);
}
}
});
// Identify Spectator Ions
var reactantIonCounts = {};
allReactantIons.forEach(function(ion) {
reactantIonCounts[ion] = (reactantIonCounts[ion] || 0) + 1;
});
var productIonCounts = {};
allProductIons.forEach(function(ion) {
productIonCounts[ion] = (productIonCounts[ion] || 0) + 1;
});
// Compare counts to find spectators
for (var ion in reactantIonCounts) {
if (productIonCounts[ion] && reactantIonCounts[ion] === productIonCounts[ion]) {
for (var i = 0; i self.indexOf(value) === index).sort();
// Build Net Ionic Equation
var netReactants = [];
var netProducts = [];
// Add reactants not in spectator ions
reactants.forEach(function(item) {
var parsed = getIonsFromFormula(item.formula);
if (parsed.isElectrolyte) {
parsed.ions.forEach(function(ion) {
var ionFormula = ion.formula + (ion.count > 1 ? ion.count : ");
var ionCharge = ion.charge !== '?' ? ion.charge : ";
var ionFull = ionFormula + ionCharge + ion.state;
var isSpectator = spectatorIons.some(function(spectator) {
return spectator.includes(ion.formula) && spectator.includes(ion.charge);
});
if (!isSpectator && netReactants.indexOf(ionFull) === -1) {
netReactants.push(ionFull);
}
});
} else {
var isSpectator = spectatorIons.some(function(spectator) { return spectator.includes(item.formula); });
if (!isSpectator && netReactants.indexOf(item.formula) === -1) {
netReactants.push(item.formula);
}
}
});
// Add products not in spectator ions
products.forEach(function(item) {
var parsed = getIonsFromFormula(item.formula);
if (parsed.isElectrolyte) {
parsed.ions.forEach(function(ion) {
var ionFormula = ion.formula + (ion.count > 1 ? ion.count : ");
var ionCharge = ion.charge !== '?' ? ion.charge : ";
var ionFull = ionFormula + ionCharge + ion.state;
var isSpectator = spectatorIons.some(function(spectator) {
return spectator.includes(ion.formula) && spectator.includes(ion.charge);
});
if (!isSpectator && netProducts.indexOf(ionFull) === -1) {
netProducts.push(ionFull);
}
});
} else {
var isSpectator = spectatorIons.some(function(spectator) { return spectator.includes(item.formula); });
if (!isSpectator && netProducts.indexOf(item.formula) === -1) {
netProducts.push(item.formula);
}
}
});
getElement("fullReactants").textContent = reactants.map(function(r) { return r.formula; }).join(' + ');
getElement("fullProducts").textContent = products.map(function(p) { return p.formula; }).join(' + ');
getElement("totalReactantIons").textContent = allReactantIons.length;
getElement("totalProductIons").textContent = allProductIons.length;
getElement("spectatorIons").textContent = spectatorIons.length > 0 ? spectatorIons.join(', ') : "None";
getElement("netIonicEquation").textContent = netReactants.join(' + ') + " → " + netProducts.join(' + ');
getElement("primaryResult").textContent = netReactants.join(' + ') + " → " + netProducts.join(' + ');
// Update Chart Data (Placeholder – requires actual chart implementation)
updateChart(allReactantIons.length, allProductIons.length, spectatorIons.length);
}
function resetCalculator() {
getElement("reactant1").value = "NaCl(aq)";
getElement("reactant2").value = "AgNO3(aq)";
getElement("product1").value = "AgCl(s)";
getElement("product2").value = "NaNO3(aq)";
getElement("coefficient1").value = "1";
getElement("coefficient2").value = "1";
getElement("coefficient3").value = "1";
getElement("coefficient4").value = "1";
getElement("reactant1Error").textContent = "";
getElement("reactant2Error").textContent = "";
getElement("product1Error").textContent = "";
getElement("product2Error").textContent = "";
getElement("coefficient1Error").textContent = "";
getElement("coefficient2Error").textContent = "";
getElement("coefficient3Error").textContent = "";
getElement("coefficient4Error").textContent = "";
getElement("fullReactants").textContent = "–";
getElement("fullProducts").textContent = "–";
getElement("totalReactantIons").textContent = "–";
getElement("totalProductIons").textContent = "–";
getElement("spectatorIons").textContent = "–";
getElement("netIonicEquation").textContent = "–";
getElement("primaryResult").textContent = "Enter reaction details";
// Reset Chart (Placeholder)
updateChart(0, 0, 0);
}
function copyResults() {
var primaryResult = getElement("primaryResult").textContent;
var fullReactants = getElement("fullReactants").textContent;
var fullProducts = getElement("fullProducts").textContent;
var totalReactantIons = getElement("totalReactantIons").textContent;
var totalProductIons = getElement("totalProductIons").textContent;
var spectatorIons = getElement("spectatorIons").textContent;
var netIonicEquation = getElement("netIonicEquation").textContent;
var textToCopy = "Ionic Equation Calculation Results:\n\n";
textToCopy += "Net Ionic Equation: " + primaryResult + "\n";
textToCopy += "Full Reactants: " + fullReactants + "\n";
textToCopy += "Full Products: " + fullProducts + "\n";
textToCopy += "Total Ions (Reactants): " + totalReactantIons + "\n";
textToCopy += "Total Ions (Products): " + totalProductIons + "\n";
textToCopy += "Spectator Ions: " + spectatorIons + "\n";
textToCopy += "Net Equation: " + netIonicEquation + "\n\n";
textToCopy += "Assumptions: Based on standard solubility rules and strong electrolyte behavior.";
// Use a temporary textarea for copying
var tempTextArea = document.createElement("textarea");
tempTextArea.value = textToCopy;
tempTextArea.style.position = "absolute";
tempTextArea.style.left = "-9999px";
document.body.appendChild(tempTextArea);
tempTextArea.select();
try {
document.execCommand("copy");
alert("Results copied to clipboard!");
} catch (err) {
console.error("Failed to copy results: ", err);
alert("Failed to copy. Please copy manually.");
}
document.body.removeChild(tempTextArea);
}
// Chart Implementation (using Canvas)
var myChart;
var chartContext = getElement('ionicChart').getContext('2d');
function updateChart(reactants, products, spectators) {
if (myChart) {
myChart.destroy(); // Destroy previous chart instance
}
var chartData = {
labels: ['Reactants', 'Products', 'Spectators'],
datasets: [{
label: 'Ion Count',
data: [reactants, products, spectators],
backgroundColor: [
'rgba(0, 74, 153, 0.6)', // Primary color for reactants
'rgba(40, 167, 69, 0.6)', // Success color for products
'rgba(108, 117, 125, 0.6)' // Muted color for spectators
],
borderColor: [
'rgba(0, 74, 153, 1)',
'rgba(40, 167, 69, 1)',
'rgba(108, 117, 125, 1)'
],
borderWidth: 1
}]
};
myChart = new Chart(chartContext, {
type: 'bar',
data: chartData,
options: {
responsive: true,
maintainAspectRatio: false,
scales: {
y: {
beginAtZero: true,
title: {
display: true,
text: 'Number of Ions/Species'
}
}
},
plugins: {
title: {
display: true,
text: 'Ion Distribution in Reaction'
},
legend: {
position: 'top',
}
}
}
});
}
// Initial setup
document.addEventListener('DOMContentLoaded', function() {
// Add canvas element for the chart
var chartSection = document.createElement('section');
chartSection.className = 'calculator-section';
chartSection.innerHTML = '
Reaction Analysis Chart
';
getElement('results').parentNode.insertBefore(chartSection, getElement('results').nextSibling);
// Initialize chart with zero values
updateChart(0, 0, 0);
// Set default values and trigger initial calculation if needed
resetCalculator();
// Optionally trigger calculation on load if default values are meaningful
// calculateIonicEquation();
});