You wish to quantify the amount of silver in 25.0 mL of a silver nitrate solution. You perform a precipitation of titration of the silver solution with 24.8 mL of 0.0220 M K₂SO4, at which point the endpoint of the titration has occurred and the silver solid has precipitated out. The reaction proceeds as: 2AgNO3(aq) + K₂SO4 (aq) → Ag₂SO4(s) + 2KNO3(aq) The solid Ag₂SO4 precipitate in the reaction beaker is in equilibrium with dissolved silver ions even though the endpoint of the titration has been reached. What is the molar concentration of Ag+ ions still in solution? The Kp for Ag₂SO, is 1.5 x 105. You may neglect activity under these conditions. A) 0.015 M B) 0.031 M C) 0.0039 M D) 7.5 x 10¹6 M
You wish to quantify the amount of silver in 25.0 mL of a silver nitrate solution. You perform a precipitation of titration of the silver solution with 24.8 mL of 0.0220 M K₂SO4, at which point the endpoint of the titration has occurred and the silver solid has precipitated out. The reaction proceeds as: 2AgNO3(aq) + K₂SO4 (aq) → Ag₂SO4(s) + 2KNO3(aq) The solid Ag₂SO4 precipitate in the reaction beaker is in equilibrium with dissolved silver ions even though the endpoint of the titration has been reached. What is the molar concentration of Ag+ ions still in solution? The Kp for Ag₂SO, is 1.5 x 105. You may neglect activity under these conditions. A) 0.015 M B) 0.031 M C) 0.0039 M D) 7.5 x 10¹6 M
Chemistry
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ISBN:9781305957404
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Chapter1: Chemical Foundations
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![You wish to quantify the amount of silver in 25.0 mL of a silver nitrate solution. You perform a
precipitation of titration of the silver solution with 24.8 mL of 0.0220 M K₂SO4, at which point
the endpoint of the titration has occurred and the silver solid has precipitated out. The reaction
proceeds as:
2AgNO3(aq) + K₂SO4 (aq) →→ Ag₂SO₂ (s) + 2KNO3(aq)
The solid Ag₂SO4 precipitate in the reaction beaker is in equilibrium with dissolved silver ions
even though the endpoint of the titration has been reached. What is the molar concentration of
Ag+ ions still in solution? The Kp for Ag₂SO4 is 1.5 x 105. You may neglect activity under these
conditions.
A) 0.015 M
B) 0.031 M
C) 0.0039 M
D) 7.5 x 10¹6 M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6b272b9a-6c91-4391-aa2a-c8dbecce5196%2F8a498d35-6db4-4c7e-ab0d-f950396b1a46%2Fq2xp7ta_processed.jpeg&w=3840&q=75)
Transcribed Image Text:You wish to quantify the amount of silver in 25.0 mL of a silver nitrate solution. You perform a
precipitation of titration of the silver solution with 24.8 mL of 0.0220 M K₂SO4, at which point
the endpoint of the titration has occurred and the silver solid has precipitated out. The reaction
proceeds as:
2AgNO3(aq) + K₂SO4 (aq) →→ Ag₂SO₂ (s) + 2KNO3(aq)
The solid Ag₂SO4 precipitate in the reaction beaker is in equilibrium with dissolved silver ions
even though the endpoint of the titration has been reached. What is the molar concentration of
Ag+ ions still in solution? The Kp for Ag₂SO4 is 1.5 x 105. You may neglect activity under these
conditions.
A) 0.015 M
B) 0.031 M
C) 0.0039 M
D) 7.5 x 10¹6 M
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