MISSED THIS? Watch

KCV: Finding pH and pH Changes in Buffer Solutions, IWE Calculating the pH of a Buffer Solution as an Equilibrium Problem and with the Henderson$-$Hasselbalch Equation

IWE Calculating the pH Change in a Buffer Solution after the Addition of a Small Amount of Strong. Acid or Base Read Section $18\mathrm{.}2.$ You can click on the Review link to access the section in your eText.

Part A

For $450\mathrm{.}0mL$ of pure water, calculate the initial $pH$ and the final $pH$ after adding $1\mathrm{.}8{10}^{-2}$mol of $HCl.$

Express your answers to two decimal places. Enter your answers numerically separated by a comma.

Part B

For $450\mathrm{.}0mL$ of a buffer solution that is $0\mathrm{.}135M$ in $H{C}_2{H}_3{O}_2$ and $9\mathrm{.}00{10}^{-2}M$ in $Na{C}_2{H}_3{O}_2,$ calculate the initial $pH$ and the final $p.$ after adding $1\mathrm{.}8{10}^{-2}$ mol of $HCl(K_a(H{C}_2{H}_3{O}_2)=1\mathrm{.}8{10}^{-5})$

Express your answers using two decimal places separated by a comma.

Reguest Answor

Part C

For $450\mathrm{.}0mL$ of a buffer solution that is $0\mathrm{.}185M$ in $C{H}_{3}C{H}_{2}N{H}_2$ and $0\mathrm{.}135M$ in $C{H}_{3}C{H}_{2}N{H}_{3}Cl,$ calculate the initial $pH$ and the fina $pH$ after adding $1\mathrm{.}8{10}^{-2}$mol of $HCl.)$

Express your answers using two decimal places separated by a comma.