During the reaction, $4\mathrm{.}90mol$ of $HCl$ are produced. Calculate the final $pH$ of the reaction solution. Assume that the $HCl$ is completely neutralized by the buffer.

Express your answer using two decimal places.

$pH=$

Previous Answers

X Incorrect; Try Again; $4$ attempts remaining

Review your calculations and make sure you round to $3$ significant figures in the last step.

A biochemical reaction takes place in a $1\mathrm{.}00mL$ solution of $0\mathrm{.}0250M$ phosphate buffer initially at $pH=7\mathrm{.}43.$

$\backslash$table$[[$Acid $($Proton Donor$),$Conjugate Base $($Proton Acc,,$p{K}_a,K_a(M)$

Please help!