consider the following equilibrium system: ocl⁻(aq) + hc₇h₅o₂(aq) ⇌ hocl(aq) + c₇h₅o₂⁻(aq) k_eq = 2.1×10³ at…

consider the following equilibrium system: ocl⁻(aq) + hc₇h₅o₂(aq) ⇌ hocl(aq) + c₇h₅o₂⁻(aq) k_eq = 2.1×10³ at equilibrium, a. products are favoured and hocl is the stronger acid. b. reactants are favoured and hocl is the stronger acid. c. products are favoured and hc₇h₅o₂ is the stronger acid. d. reactants are favoured and hc₇h₅o₂ is the stronger acid.

consider the following equilibrium system: ocl⁻(aq) + hc₇h₅o₂(aq) ⇌ hocl(aq) + c₇h₅o₂⁻(aq) k_eq = 2.1×10³ at equilibrium, a. products are favoured and hocl is the stronger acid. b. reactants are favoured and hocl is the stronger acid. c. products are favoured and hc₇h₅o₂ is the stronger acid. d. reactants are favoured and hc₇h₅o₂ is the stronger acid.

Answer

Explanation:

Step1: Analyze equilibrium constant

The equilibrium constant $K_{eq}=2.1\times 10^{3}$. Since $K_{eq}> 1$, the forward - reaction is favored, so products are favored at equilibrium.

Step2: Determine stronger acid

In an acid - base reaction, the stronger acid reacts to form the weaker acid. Here, $HC_{7}H_{5}O_{2}$ donates a proton to $OCl^{-}$. So $HC_{7}H_{5}O_{2}$ is the stronger acid.

Answer:

C. products are favoured and $HC_{7}H_{5}O_{2}$ is the stronger acid.