Balance the following equations: (d) Na 2 CO 3 (aq) + HCl(aq) → NaCl(aq) + H 2 O(l) + CO 2 (g)

Hey everyone. We're asked to balance the following chemical reaction. We can start by counting the number of atoms we have on both sides. Starting off with our calcium in our react inside we have three of calcium, two of nitrogen, two of hydrogen and one of oxygen. Looking at our product side, we have one of calcium, one of nitrogen, five of hydrogen and two of oxygen. We can start off by balancing out our calcium by adding a three prior to our calcium hydroxide. When we do this, we end up with three of calcium, nine of hydrogen and six of oxygen. Looking at our nitrogen, we can balance this out by adding a two prior to our ammonia. When we add this to, we change our nitrogen into two And we also change our hydrogen from a nine into a 12. Now to finish off this question, we can balance off our hydrogen and oxygen by adding a six prior to our water. So we end up with 12 of hydrogen and six of oxygen and this will be our final balanced chemical equation. So I hope this made sense. And let us know if you have any questions

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 12d

Chapter 3, Problem 12d

Balance the following equations: (d) Na₂CO₃(aq) + HCl(aq) → NaCl(aq) + H₂O(l) + CO₂(g)

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Identify the reactants and products in the chemical equation: \( \text{Na}_2\text{CO}_3 (aq) + \text{HCl} (aq) \rightarrow \text{NaCl} (aq) + \text{H}_2\text{O} (l) + \text{CO}_2 (g) \).

List the number of each type of atom on both sides of the equation to determine which are unbalanced.

Start by balancing the sodium (Na) atoms. There are 2 Na atoms in \( \text{Na}_2\text{CO}_3 \), so you need 2 NaCl on the product side.

Next, balance the chlorine (Cl) atoms. Since you have 2 NaCl, you need 2 HCl on the reactant side to balance the Cl atoms.

Finally, check the balance of hydrogen (H) and oxygen (O) atoms. Ensure that the number of each type of atom is equal on both sides of the equation.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.

Types of Chemical Reactions

Understanding the types of chemical reactions, such as acid-base reactions, is crucial for balancing equations. In the given equation, sodium carbonate (Na2CO3) reacts with hydrochloric acid (HCl) to produce sodium chloride (NaCl), water (H2O), and carbon dioxide (CO2). Recognizing the reactants and products helps in determining how to balance the equation effectively.

State Symbols in Chemical Equations

State symbols indicate the physical state of the reactants and products in a chemical equation: (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solutions. In the provided equation, recognizing that Na2CO3 and HCl are in aqueous solution while CO2 is a gas is important for understanding the reaction conditions and the nature of the products formed.

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Balance the following equations: (c) Al(OH)₃(s) + H₂SO₄(l) → Al₂(SO₄)₃(s) + H₂O(l)

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