Solid N H 2 COON H 4 is heated in a closed rigid container of volume 8.21 L at 500 K temperature as following: N H 2 COON H 4 ( s ) ⇌ 2 N H 3 ( g ) + C O 2 ( g ) If the equilibrium pressur

Question

Solid N H 2 ​ COON H 4 ​ is heated in a closed rigid container of volume 8.21 L at 500 K temperature as following: N H 2 ​ COON H 4 ​ ( s ) ⇌ 2 N H 3 ​ ( g ) + C O 2 ​ ( g ) If the equilibrium pressure is 1.5 a t m and all moles of N H 3 ​ present at equilibrium dissolved in one liter of water, and this solution is titrated with 2000 m L of 0.1 M H Cl solution. Now, 1000 m L of 0.1 M N a O H is added. What is the final pH of the final solution? [Given: p K a ​ ( N H 4 + ​ ) = 9 ]

TestHub · Accepted Answer

Total moles at equilibrium = 0.0821 × 500 1.5 × 8.21 ​ = 0.3 . Moles of NH₃ = 0.2 and moles of CO₂ = 0.1 . Moles of HCl = 0.1 × 2 = 0.2 . NH₃ and HCl are consumed completely and 0.2 moles of NH₄Cl is formed. Moles of NaOH added = 0.1 × 1 = 0.1 . NH₄Cl + NaOH ⟶ NH₄OH + NaCl 0.2 ​ 0.1 ​ 0 ​ 0 ​ 0.1 0 0.1 The final solution is a buffer solution, so the pH of the solution = pK a ​ ( NH 4 + ​ ) = 9 .

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