consider the reaction of 75.0 ml of 0.350 m c₅h₅n (kb = 1.7 x 10⁻⁹) with 100.0 ml of 0.425 m hcl.\nwhat…

consider the reaction of 75.0 ml of 0.350 m c₅h₅n (kb = 1.7 x 10⁻⁹) with 100.0 ml of 0.425 m hcl.\nwhat would the total volume of the solution be after the reaction, in ml?

consider the reaction of 75.0 ml of 0.350 m c₅h₅n (kb = 1.7 x 10⁻⁹) with 100.0 ml of 0.425 m hcl.\nwhat would the total volume of the solution be after the reaction, in ml?

Answer

Explanation:

Step1: Add the volumes

When two solutions are mixed, the total volume ( V_{total}) is the sum of the volumes of the individual solutions. (V_{total}=V_1 + V_2) where (V_1 = 75.0\space mL) (volume of (C_5H_5N) solution) and (V_2=100.0\space mL) (volume of (HCl) solution)

Step2: Calculate the total volume

Substitute the values into the formula: (V_{total}=75.0\space mL+ 100.0\space mL) (V_{total}=175.0\space mL)

Answer:

(175.0\space mL)