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65 What is the minimum concentration of NH3 (mmol/L) needed to prevent Ağci(s) from precipitating from a 0.91 L solution containing 0.116 mol AgNO3 and 0.016 mol NaCl? Ksp of AgCl = 1.388 x 10-8 72046109.59 Kf of [Ag[NH3]2] = 1.496 x 107 between Ag & NH3 ---> The complex ion formed

65 What is the minimum concentration of NH3 (mmol/L) needed to prevent Ağci(s) from precipitating from a 0.91 L solution containing 0.116 mol AgNO3 and 0.016 mol NaCl? Ksp of AgCl = 1.388 x 10-8 72046109.59 Kf of [Ag[NH3]2] = 1.496 x 107 between Ag & NH3 ---> The complex ion formed

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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**Problem Statement:** What is the minimum concentration of NH₃ (mmol/L) needed to prevent AgCl(s) from precipitating from a 0.91 L solution containing 0.116 mol AgNO₃ and 0.016 mol NaCl? **Given Data:** - \( K_{sp} \) of AgCl = \( 1.388 \times 10^{-8} \) - \( K_f \) of \([ \text{Ag[NH}_3]_2 ]^+ = 1.496 \times 10^7 \) This is the complex ion formed between Ag and NH₃. --- **Note:** There is a calculation or reference (possibly a solution step) written as: 72046 / 109.59. This likely pertains to further solving the problem related to concentrations or equilibrium constants. --- This transcribed and explained problem setup would be used to educate on concepts such as solubility product constant (\( K_{sp} \)), formation constant (\( K_f \)), and the role of complex formation in preventing precipitation.
Transcribed Image Text:**Problem Statement:** What is the minimum concentration of NH₃ (mmol/L) needed to prevent AgCl(s) from precipitating from a 0.91 L solution containing 0.116 mol AgNO₃ and 0.016 mol NaCl? **Given Data:** - \( K_{sp} \) of AgCl = \( 1.388 \times 10^{-8} \) - \( K_f \) of \([ \text{Ag[NH}_3]_2 ]^+ = 1.496 \times 10^7 \) This is the complex ion formed between Ag and NH₃. --- **Note:** There is a calculation or reference (possibly a solution step) written as: 72046 / 109.59. This likely pertains to further solving the problem related to concentrations or equilibrium constants. --- This transcribed and explained problem setup would be used to educate on concepts such as solubility product constant (\( K_{sp} \)), formation constant (\( K_f \)), and the role of complex formation in preventing precipitation.
**Solubility and Precipitation of Salts** For the following two salts: 1. XY has \( K_{sp1} = 2.403 \times 10^{-10} \) 2. XZ has \( K_{sp2} = 4.750 \times 10^{-15} \) where \( X^+ \) is a common cation and \( Y^- \) and \( Z^- \) are anions. **Process:** - \( X^+ \) (in solution with an anion that does not interfere in this process) is added slowly to a flask originally containing 0.045 M \( Y^- \) (aq) and 0.175 M \( Z^- \) (aq). - Thus, XZ and XY may precipitate when their concentration reaches the solubility limit for either. The more insoluble of the two salts, XZ, precipitates first. **Question:** What is the concentration (mol/L) of \( Z^- \) remaining in the flask when the more soluble salt XY starts to precipitate? *Assumption: The addition of the \( X^+ \) containing solution makes only a negligible change in total volume.*
Transcribed Image Text:**Solubility and Precipitation of Salts** For the following two salts: 1. XY has \( K_{sp1} = 2.403 \times 10^{-10} \) 2. XZ has \( K_{sp2} = 4.750 \times 10^{-15} \) where \( X^+ \) is a common cation and \( Y^- \) and \( Z^- \) are anions. **Process:** - \( X^+ \) (in solution with an anion that does not interfere in this process) is added slowly to a flask originally containing 0.045 M \( Y^- \) (aq) and 0.175 M \( Z^- \) (aq). - Thus, XZ and XY may precipitate when their concentration reaches the solubility limit for either. The more insoluble of the two salts, XZ, precipitates first. **Question:** What is the concentration (mol/L) of \( Z^- \) remaining in the flask when the more soluble salt XY starts to precipitate? *Assumption: The addition of the \( X^+ \) containing solution makes only a negligible change in total volume.*
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