91Ó°ÊÓ

Identify the conjugate acid-base pairs in this reaction. \(\mathrm{NH}_{3}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}^{-} \rightarrow \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}+\mathrm{NH}_{2}^{-}\)

The concentration of commercial HCl is about \(12 \mathrm{M}\). What is its \(\mathrm{pH}\) and \(\mathrm{pOH}\) ?

What are \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) in a \(6.02 \times 10^{-4} \mathrm{M}\) solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\) ?

A lab technician mixes a solution of \(0.55 \mathrm{M} \mathrm{HNO}_{3}\). Is the resulting \(\mathrm{H}^{+}\) concentration greater than, equal to, or less than 0.55 M? Explain your answer.

Identify the conjugate acid-base pairs in this reaction. $$ \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}+\mathrm{C}_{2} \mathrm{O}_{4}^{2-} \rightarrow \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}+\mathrm{HC}_{2} \mathrm{O}_{4}^{-} $$

If a solution has a pOH of 13.09 , what is its \(\mathrm{pH},\left[\mathrm{H}^{+}\right],\) and \(\left[\mathrm{OH}^{-}\right] ?\)

The concentration of concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is about \(18 \mathrm{M}\). Assuming only one \(\mathrm{H}^{+}\) comes off the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) molecule, what is its \(\mathrm{pH}\) and \(\mathrm{pOH}\) ? What would the \(\mathrm{pH}\) and \(\mathrm{pOH}\) be if the second \(\mathrm{H}^{+}\) were also ionized?

If \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{NH}\) is dissociated only to an extent of \(0.077 \%,\) what are \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) in a 0.0955 M solution of \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{NH} ?\)