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Chapter 9: QCE (page 207)

What is the pH of a solution prepared by dissolving $1.23 g$ of
2-nitrophenol (FM 139.11) in 0.250 L?

Short Answer

Expert verified

The $PH$ of $1.23 g$ of 2-nitrophenol in $0.250 L$ is $4.34$

Step by step solution

01

Define the formula to find PH.

The formula PH of the solution

$PH = {logA}_{H^{+}} PH = \log {[H^{+}]}_{{yH}^{+}}$

02

Calculate thePHof 1.23gof 2 -nitrophenol 0.250 L.

Given Formula mass $= 139.11$

Acid-equilibria constant, $= 139.11$

Mass of 2-nitrophenol $= 1.23 g$

Volume of 2-nitrophenol $0.250 L$

The formal concentration $F_{HA}$ .

$F_{HA} = \frac{1.23 g / (139.11 g / mol)}{0.250 L} F_{HA} = 0.0354 M HA 鈬� H^{+} + A^{-} F - x \frac{x^{2}}{0.0354 - x} = 5.89 脳 10^{- 8} M x 鈮� \sqrt{(0.0354) (5.89 脳 10^{- 8})} x = 4.57 脳 10^{- 5} M$

The of 2-nitrophenol .

$PH = - \log [H^{-}] PH = - \log (4.57 脳 10^{- 5} M) PH = 4.34$

Thus, the $PH$ of $1.23 g$ of 2-nitrophenol in $0.250 L$ is $4.34$

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Most popular questions from this chapter

(Without activities), calculate the pH of

(a) $1.0 脳 10^{- 8} MHBr$

(b) role="math" localid="1654840353627" $1.0 脳 10^{- 8} {MH}_{2} {SO}_{4}$ $(H_{2} {SO}_{4}$ dissociates completely to $2 H^{+}$ plus ${SO}_{4}^{2 -}$ at this low concentration).

A solution with an ionic strength of $0.10 M$ containing $0.0100 M$ phenylhydrazine has a pH of 8.13. Using activity coefficients correctly, find ${pK}_{a}$ for the phenylhydrazinium ion found in phenylhydrazine hydrochloride. Assume that $Y_{{BH}^{+}} = 0.80$

Find the pH of 0.050 M triethylammonium bromide.

A buffer was prepared by dissolving 0.100 mole of the weak acid $H A (K_{a} = 1.00 脳 10^{- 5})$ plus 0.050 mole of its conjugate base ${Na}^{+} A^{-}$ in 1.00 L. Find the pH

${Cr}^{3 +}$ is acidic by virtue of the hydrolysis reaction ${Cr}^{3 +} H_{2} O \overset{K_{aI}}{鈬�} Cr {(OH)}^{2 +} + H^{+}$ . [Further reactions produce $Cr {(OH)}_{2,}^{+} Cr {(OH)}_{3}$ and.] Find the value role="math" localid="1654864894349" $K_{aI}$ of in Figure 6-9. Considering only the $K_{aI}$ reaction, find pH value ofrole="math" localid="1654865110221" $0.010 MCr {({CIO}_{4})}_{3}$ What fraction of chromium is in the formrole="math" localid="1654865163335" $Cr {(OH)}^{2 +}$ ?

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