What is the approximate concentration of free Cu²+ ion at equilibrium when 1.05x10-2 mol copper(II) nitrate is added to 1.00 L of solution that is 1.270 M in NH3. For [Cu(NH3)4]²+, Kf = 2.1×10¹³. [Cu²+] = M
What is the approximate concentration of free Cu²+ ion at equilibrium when 1.05x10-2 mol copper(II) nitrate is added to 1.00 L of solution that is 1.270 M in NH3. For [Cu(NH3)4]²+, Kf = 2.1×10¹³. [Cu²+] = M
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![What is the approximate concentration of free Cu²+ ion at equilibrium
when 1.05x10-² mol copper(II) nitrate is added to 1.00 L of
solution that is 1.270 M in NH3. For [Cu(NH3)4]²+, Kƒ = 2.1×10¹³.
[Cu²+] =
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9be9f06a-e87d-4b56-9338-85b6933acfe1%2F12c5a020-e897-46fe-a36d-7107053973fd%2Fhsyjenn_processed.png&w=3840&q=75)
Transcribed Image Text:What is the approximate concentration of free Cu²+ ion at equilibrium
when 1.05x10-² mol copper(II) nitrate is added to 1.00 L of
solution that is 1.270 M in NH3. For [Cu(NH3)4]²+, Kƒ = 2.1×10¹³.
[Cu²+] =
M
![In the presence of excess OH, the Zn²+(aq) ion forms a hydroxide complex ion,
2-
Zn(OH)4²-. Calculate the concentration of free Zn²+ ion when 1.23×10-² mol ZnSO4(s)
is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.10). For
2-
Zn(OH)4²¯, Kf = 4.6×10¹7.
[Zn²+] =
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9be9f06a-e87d-4b56-9338-85b6933acfe1%2F12c5a020-e897-46fe-a36d-7107053973fd%2Fkshjf6_processed.png&w=3840&q=75)
Transcribed Image Text:In the presence of excess OH, the Zn²+(aq) ion forms a hydroxide complex ion,
2-
Zn(OH)4²-. Calculate the concentration of free Zn²+ ion when 1.23×10-² mol ZnSO4(s)
is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.10). For
2-
Zn(OH)4²¯, Kf = 4.6×10¹7.
[Zn²+] =
M
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