Question

question 1
what is the complete ionic equation for the reaction of na₂co₃ and hcl in water?
dont forget to balance the reaction equation.

○ 2na⁺(aq) + co₃²⁻(aq) + 2h⁺(aq) + 2cl⁻(aq) ==> 2na⁺(aq) + 2cl⁻(aq) + h₂co₂(aq)
○ 2na⁺(aq) + co₃²⁻(aq) + 2h⁺(aq) + 2cl⁻(aq) ==> 2nacl(aq) + co₂(g) + h₂o(l)
○ 2na⁺(aq) + co₃²⁻(aq) + 2h⁺(aq) + 2cl⁻(aq) ==> 2na⁺(aq) + 2cl⁻(aq) + co₂(g) + h₂o(l)
○ 2na⁺(aq) + co₃²⁻(aq) + 2h⁺(aq) + 2cl⁻(aq) ==> 2nacl(s) + co₂(g) + h₂o(l)
○ na₂co₃(aq) + 2hcl(aq) ==> 2nacl(aq) + co₂(g) + h₂o(l)

Explanation:

To determine the complete ionic equation, we first recall that soluble ionic compounds dissociate into ions in water. \( \text{Na}_2\text{CO}_3 \) (aq) dissociates into \( 2\text{Na}^+ \) (aq) and \( \text{CO}_3^{2-} \) (aq), and \( \text{HCl} \) (aq) dissociates into \( \text{H}^+ \) (aq) and \( \text{Cl}^- \) (aq). The reaction produces \( \text{NaCl} \) (aq, which dissociates into \( \text{Na}^+ \) and \( \text{Cl}^- \)), \( \text{CO}_2 \) (g), and \( \text{H}_2\text{O} \) (l).

• The first option is incorrect because \( \text{H}_2\text{CO}_2 \) is not a product (the reaction produces \( \text{CO}_2 \) and \( \text{H}_2\text{O} \) from \( \text{H}_2\text{CO}_3 \) decomposition, not \( \text{H}_2\text{CO}_2 \)).
• The second option is incorrect because \( \text{NaCl} \) (aq) should be dissociated into ions in a complete ionic equation, not written as a formula unit.
• The third option is correct: reactants dissociate into ions, and products \( \text{Na}^+ \) (aq), \( \text{Cl}^- \) (aq), \( \text{CO}_2 \) (g), and \( \text{H}_2\text{O} \) (l) are shown, with \( \text{NaCl} \) dissociated into ions.
• The fourth option is incorrect because \( \text{NaCl} \) is soluble and should be in aqueous (dissociated) form, not solid.
• The fifth option is a molecular equation, not a complete ionic equation.

Answer:

The correct option is: \( 2\text{Na}^+_{(aq)} + \text{CO}_3^{2-}_{(aq)} + 2\text{H}^+_{(aq)} + 2\text{Cl}^-_{(aq)} ==> 2\text{Na}^+_{(aq)} + 2\text{Cl}^-_{(aq)} + \text{CO}_{2(g)} + \text{H}_2\text{O}_{(l)} \) (the third option in the list)