Final answer:
The K₁ of formic acid can be calculated using the given pK₁ of 3.75, resulting in a value of approximately 1.78 x 10⁻⁴.
Step-by-step explanation:
Formic acid, with a provided pK₁ of 3.75, demonstrates its acidic strength through the calculation of the acid dissociation constant (K₁). The relationship K₁ = 10⁻¹⁶ⁱ²;π₁₃₁₁, where π₁₃₁₁ is the pK₁ value, is employed. By substituting pK₁ = 3.75 into the formula, K₁ is determined to be 10⁻³.75, yielding a numerical value of approximately 1.78 x 10⁻⁴. This outcome signifies the acid's weak nature, reflecting its limited tendency to donate protons in an aqueous environment.
The lower the K₁, the weaker the acid, highlighting formic acid's relatively modest capacity for proton donation when compared to stronger acids. Understanding such constants is crucial in assessing the behavior of acids in various chemical reactions and their impact in aqueous solutions.