Which of the following statements is/are true for a 0.10 M solution of a weak acid HA?

[H+] >> [A−]
[H+] = [A−]
The pH is 1.00.
The pH is less than 1.00

Struggling with going from molarity of solution to the concentrations of individual parts of the reaction ([HA}, {H^+], [A^-].)

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

"record the time to complete a chemical reaction" would most likely be part of a lab procedure.

0.88m hope i am correct : )