Aqueous solutions of phosphoric acid and sodium nitrite are combined, and the following equilibrium is established. H₃PO₄(aq) + NO₂^-(aq) H₂PO₄^-(aq) + HNO₂(aq)
The equilibrium constant K_c for this reaction is greater than one. Based on this information, which of the following statements is correct?

Question

Aqueous solutions of phosphoric acid and sodium nitrite are combined, and the following equilibrium is established. H₃PO₄(aq) + NO₂^-(aq)

Aqueous solutions of phosphoric acid and sodium nitrite are combined, and the following equilibrium is established. H<sub>3</sub>PO<sub>4</sub>(aq) + NO<sub>2</sub><sup>-</sup>(aq) H<sub>2</sub>PO<sub>4</sub><sup>-</sup>(aq) + HNO<sub>2</sub>(aq) The equilibrium constant K<sub>c</sub> for this reaction is greater than one. Based on this information, which of the following statements is correct? A) Phosphoric acid is a weaker acid than nitrous acid. B) Nitrous acid is a weaker acid than water. C) The nitrite anion is a weaker base than the dihydrogen phosphate anion. D) The dihydrogen phosphate anion is a stronger acid than nitrous acid. E) Phosphoric acid is a stronger acid than nitrous acid.

H₂PO₄^-(aq) + HNO₂(aq)
The equilibrium constant K_c for this reaction is greater than one. Based on this information, which of the following statements is correct?

Quizplus · Accepted Answer

A larger value of the equilibrium constant indicates a higher degree of reaction favoring the products. This means that products are more stable than the reactants. As phosphoric acid and sodium nitrite combine to form the products H2PO4- and HNO2, respectively, it suggests that H2PO4- is more stable (or in other words, a stronger acid) than HNO2. Therefore, phosphoric acid is a stronger acid than nitrous acid.

Aqueous Solutions of Phosphoric Acid and Sodium Nitrite Are Combined