Question
Hydrazine, $\mathrm{N}_{2} \mathrm{H}_{4}$, is weak base with $K_{\mathrm{b}}=1.3 \times 10^{-6} .$ Fill in the iCe table and write the equation needed to solve for the concentration of hydroxide ion in a $0.10 \mathrm{M}$ solution.
Step 1
Step 1: First, we write the ionization equation for hydrazine, $\mathrm{N}_{2} \mathrm{H}_{4}$, in water: \[\mathrm{N}_{2} \mathrm{H}_{4} + \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{N}_{2} \mathrm{H}_{5}^{+} + \mathrm{OH}^{-}\] Show more…
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Hydrazine, $\mathrm{N}_{2} \mathrm{H}_{4},$ can interact with water in two steps. $$ \begin{aligned} \mathrm{N}_{2} \mathrm{H}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) & \rightleftarrows \mathrm{N}_{2} \mathrm{H}_{5}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \\ K_{\mathrm{bl}} &=8.5 \times 10^{-7} \\ \mathrm{N}_{2} \mathrm{H}_{5}^{+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) & \rightleftarrows \mathrm{N}_{2} \mathrm{H}_{6}^{2+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \\ K_{\mathrm{b} 2} &=8.9 \times 10^{-16} \end{aligned} $$ (a) What is the concentration of $\mathrm{OH}^{-}, \mathrm{N}_{2} \mathrm{H}_{5}^{+},$ and $\mathrm{N}_{2} \mathrm{H}_{6}{ }^{2+}$ in a $0.010 \mathrm{M}$ aqueous solution of hydrazine? (b) What is the $\mathrm{pH}$ of the $0.010 \mathrm{M}$ solution of hydrazine?
Hydrazine, $\mathrm{N}_{2} \mathrm{H}_{4},$ can interact with water in two steps. $$\begin{aligned} \mathrm{N}_{2} \mathrm{H}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) & \rightleftharpoons \mathrm{N}_{2} \mathrm{H}_{5}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \\ K_{\mathrm{b} 1} &=8.5 \times 10^{-7} \\ \mathrm{N}_{2} \mathrm{H}_{5}^{+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) & \rightleftarrows \mathrm{N}_{2} \mathrm{H}_{6}^{2+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \\ K_{\mathrm{b} 2} &=8.9 \times 10^{-16} \end{aligned}$$ (a) What is the concentration of $\mathrm{OH}^{-}, \mathrm{N}_{2} \mathrm{H}_{5}^{+}$ and $\mathrm{N}_{2} \mathrm{H}_{6}^{2+}$ in a $0.010 \mathrm{M}$ aqueous solution of hydrazine? (b) What is the $\mathrm{pH}$ of the 0.010 M solution of hydrazine?
Hydrazine, $\mathrm{N}_{2} \mathrm{H}_{4}$, is a base that ionizes to give $\mathrm{N}_{2} \mathrm{H}_{5}{ }^{+}$ and $\mathrm{OH}^{-}\left(K_{b}=1.7 \times 10^{-6}\right)$. You add magnesium sulfate to a hydrazine solution. Calculate the concentration of $\mathrm{Mg}^{2+}$ ion when magnesium hydroxide, $\mathrm{Mg}(\mathrm{OH})_{2},$ just begins to precipitate from $0.20 \mathrm{M} \mathrm{N}_{2} \mathrm{H}_{4} . K_{s p}$ for $\mathrm{Mg}(\mathrm{OH})_{2}$ is $1.8 \times 10^{-11}$.
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