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
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![65
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?
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
--->](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2F1f031f2b-5e81-4f00-b3ee-8434daaaf638%2F71sgxks_processed.jpeg&w=3840&q=75)
![-10
For the following two salts: XY has KSP1 = 2.403 × 10 and XZ has
KSP2=4.750 x 10
-15
where X+ is a common cation and Y and Z are anions.
X+ (in solution with a anion that does not interfere in this process)
is added slowly to a flask originally containing 0.045 MY" (aq) and
0.175 MZ (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.
What is the concentration (mol/L) of Z remaining in the flask when
the more soluble salt XY starts to precipitate?
Assume that the additional X* containing solution makes only a
negligible change in total volume.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2F1f031f2b-5e81-4f00-b3ee-8434daaaf638%2Fvuajq4h_processed.jpeg&w=3840&q=75)
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