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Credit) Use the References to access important values if needed for this question. t 25 °C of an aqueous solution of the sodium salt of hydrocyanic acid (NaCN) is 11.15. Calculate the concentration of CN" in this solution, in moles per liter. K, for HCN is equal to 6.2x10-10 M

Credit) Use the References to access important values if needed for this question. t 25 °C of an aqueous solution of the sodium salt of hydrocyanic acid (NaCN) is 11.15. Calculate the concentration of CN" in this solution, in moles per liter. K, for HCN is equal to 6.2x10-10 M

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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### Additional Extra Credit **Educational Task:** *Use the References to access important values if needed for this question.* The pH at 25 °C of an aqueous solution of the sodium salt of hydrocyanic acid (NaCN) is **11.15**. Calculate the concentration of \( \text{CN}^- \) in this solution, in moles per liter. \( K_a \) for HCN is equal to \( 6.2 \times 10^{-10} \). \[ \text{Concentration:} \, \boxed{ \hspace{2em} } \, \text{M} \]
Transcribed Image Text:### Additional Extra Credit **Educational Task:** *Use the References to access important values if needed for this question.* The pH at 25 °C of an aqueous solution of the sodium salt of hydrocyanic acid (NaCN) is **11.15**. Calculate the concentration of \( \text{CN}^- \) in this solution, in moles per liter. \( K_a \) for HCN is equal to \( 6.2 \times 10^{-10} \). \[ \text{Concentration:} \, \boxed{ \hspace{2em} } \, \text{M} \]
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Here the pH of aqueous solution of NaCN is 11.15 at 25°C. We have to determine concentration of CN-1 . Given Ka HCN= 6.2×10-10.

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