Question
What is the pH of a $0.50 \mathrm{M}$ aqueous $\mathrm{NaCN}$ solution? $\mathrm{p} K_{\mathrm{b}}$ of $\mathrm{CN}^{-}$ is $4.70 .$$(\log 2=0.3)$(a) $3.0$(b) $11.0$(c) $4.7$(d) $9.3$
Step 1
CN- is the conjugate base of the weak acid HCN, and it will react with water to form HCN and OH- ions: CN- + H2O ⇌ HCN + OH- Show more…
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