The half-life of a reaction, t1/2, is the time required for one-half of a reactant to be consumed. It is the time during which the amount of reactant or its concentration decreases to one-half of its initial value.

Determine the half-life for the reaction in Part B using the integrated rate law, given that the initial concentration is 1.90mol?L?1 and the rate constant is 0.0016mol?

The half life of the reaction is 593.8 seconds

Explanation:

We are given:

Rate constant =

The formula for determining the unit of 'k' is:

where, n = order of reaction

The unit of concentration is, M or mole/L

The unit of time is, second or 's'

Evaluating the value of 'n' from above equation:

The reaction is zero order reaction.

The equation used to calculate half life for zero order kinetics:

where,

k = Rate constant =

= initial concentration = 1.90 mol/L

Putting values in above equation, we get:

Hence, the half life of the reaction is 593.8 seconds

the ratio of the conjugate base to the acid required to attain the desired ph.

the answer is option a.