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In a titration of unknown triprotic acid, H3A, 63.5 mL of 0.556 M calcium hydroxide are needed to neutralize 25.0 mL of the acid. Which is the balanced chemical reaction for this process? Note that A represents any anion with -3 charge. О 2НЗА(aq) + 3Саa(ОН)2(aq) — Саз А2(ag) + 6H20(0 НзА(ag) + 3CаОН(aq) — зСаА(aq) + зн200 НзА(аq) + CаOH(aq) — СаА (аq) + H20Ф H3A(aq) + Ca(OH)2(aq) → CaA2(aq) + H20(1) HзА(ag) + Ca(ОН)2(ag) — Саз А2(aq) + H200

In a titration of unknown triprotic acid, H3A, 63.5 mL of 0.556 M calcium hydroxide are needed to neutralize 25.0 mL of the acid. Which is the balanced chemical reaction for this process? Note that A represents any anion with -3 charge. О 2НЗА(aq) + 3Саa(ОН)2(aq) — Саз А2(ag) + 6H20(0 НзА(ag) + 3CаОН(aq) — зСаА(aq) + зн200 НзА(аq) + CаOH(aq) — СаА (аq) + H20Ф H3A(aq) + Ca(OH)2(aq) → CaA2(aq) + H20(1) HзА(ag) + Ca(ОН)2(ag) — Саз А2(aq) + H200

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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**Balanced Chemical Reaction for Titration of Triprotic Acid** In a titration of unknown triprotic acid, H₃A, 63.5 mL of 0.556 M calcium hydroxide are needed to neutralize 25.0 mL of the acid. Which is the balanced chemical reaction for this process? Note that A represents any anion with a -3 charge. Options: 1. \(2H_3A(aq) + 3Ca(OH)_2(aq) \rightarrow Ca_3A_2(aq) + 6H_2O(l)\) 2. \(H_3A(aq) + 3CaOH(aq) \rightarrow 3CaA(aq) + 3H_2O(l)\) 3. \(H_3A(aq) + Ca(OH)_2(aq) \rightarrow CaA(aq) + H_2O(l)\) 4. \(H_3A(aq) + Ca(OH)_2(aq) \rightarrow CaA_2(aq) + H_2O(l)\) 5. \(H_3A(aq) + Ca(OH)_2(aq) \rightarrow Ca_3A_2(aq) + H_2O(l)\) **Explanation:** In this problem, it is essential to write the correct balanced chemical reaction for the titration of the triprotic acid H₃A with calcium hydroxide \(Ca(OH)_2\). The term "triprotic" indicates that the acid can donate three protons (H⁺ ions). Balanced chemical equations must follow the law of conservation of mass and charge. By examining each provided option: 1. \(2H_3A(aq) + 3Ca(OH)_2(aq) \rightarrow Ca_3A_2(aq) + 6H_2O(l)\) This reaction correctly balances the number of H⁺ ions from the triprotic acid with the OH⁻ ions from calcium hydroxide, producing water and the corresponding anion-cation complex. Let's affirm the balancing: - Reactants: \(H_3A\) x 2 (providing \(H^+\) x 6) and \(Ca(OH)_2\) x 3 (providing \(OH^-\) x 6). - Products:
Transcribed Image Text:**Balanced Chemical Reaction for Titration of Triprotic Acid** In a titration of unknown triprotic acid, H₃A, 63.5 mL of 0.556 M calcium hydroxide are needed to neutralize 25.0 mL of the acid. Which is the balanced chemical reaction for this process? Note that A represents any anion with a -3 charge. Options: 1. \(2H_3A(aq) + 3Ca(OH)_2(aq) \rightarrow Ca_3A_2(aq) + 6H_2O(l)\) 2. \(H_3A(aq) + 3CaOH(aq) \rightarrow 3CaA(aq) + 3H_2O(l)\) 3. \(H_3A(aq) + Ca(OH)_2(aq) \rightarrow CaA(aq) + H_2O(l)\) 4. \(H_3A(aq) + Ca(OH)_2(aq) \rightarrow CaA_2(aq) + H_2O(l)\) 5. \(H_3A(aq) + Ca(OH)_2(aq) \rightarrow Ca_3A_2(aq) + H_2O(l)\) **Explanation:** In this problem, it is essential to write the correct balanced chemical reaction for the titration of the triprotic acid H₃A with calcium hydroxide \(Ca(OH)_2\). The term "triprotic" indicates that the acid can donate three protons (H⁺ ions). Balanced chemical equations must follow the law of conservation of mass and charge. By examining each provided option: 1. \(2H_3A(aq) + 3Ca(OH)_2(aq) \rightarrow Ca_3A_2(aq) + 6H_2O(l)\) This reaction correctly balances the number of H⁺ ions from the triprotic acid with the OH⁻ ions from calcium hydroxide, producing water and the corresponding anion-cation complex. Let's affirm the balancing: - Reactants: \(H_3A\) x 2 (providing \(H^+\) x 6) and \(Ca(OH)_2\) x 3 (providing \(OH^-\) x 6). - Products:
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