16. What is the K, expression for the dissolution of nickel (II) phosphate in water? [N₁"][PO] [Ni, (PO₂)₂] [N][PO] d. [Ni'1'[PO]' a. b. [Ni²] [PO] [Ni, (PO₂)₂] C. e. [Ni, (PO.):1/ runtil the solution becomes saturated. The [Y] in the saturated
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.
![16. What is the K expression for the dissolution of nickel (II) phosphate in water?
a. [N][PO]
[N][PO]
[Ni, (PO₂)₂]
b. [NiT [PO]
[Ni,(PO4)₂]
d. [NiT [PO]
17. Solid yttrium fluoride (YF:) is added to pure water until the solution becomes saturated. The [Y] in the saturated
solution is found to be 4.23 x10 M. What is the value of K for YF?
a. 8.64x10
b.
3.20x10
c. 1.61x10
d. 7.57x10-17
e. 1.79x10-11
18. Which of the following correctly ranks the salts in terms of increasing molar solubility?
Pbl
K=9.8x10
a. TII<Pbl < Agl
b. Pbl <TII < Agl
Agt
Kip-8.5x10-17
a. 2.45x10³
c. Pbl: <Agl<TII
d. TII Agl< Pbl₂
b. 4.97x1019
e. [Ni,(PO₂):1/
19. In which of the following solutions will cadmium iodate (Cd(103)2, Kp = 2.5x105) be the least soluble?
e. 0.10 M NaCl
a. 0.10 M Cd(NO₂)2
b. 0.10 M NalO;
c. Pure water
d. A solution with pH = 1
TII
Kp = 5.5x10
20. Solutions can be analyzed for sulfate content using gravimetric analysis by precipitation of sulfate ions as BaSO
(K=1.08x100). If a solution has a [SO] of 2.10x10 M, what [Ba], in M, will be required to initiate
precipitation?
a. 2.10x10
b. 5.14x10
d. 1.04x10-5 e. 4.41x10³
c. 2.27x10
21. Given the following reactions and equilibrium constants:
e. Agl<TII < Pbl₂
Ag, CO, (s) = 2Ag (ag) + CO (aq)
[Ag(NH₂),] (aq) = Ag (aq) + 2NH₂(aq)
Calculate the value of Ke for the reaction of silver carbonate with ammonia to form the silver ammine complex:
Ag,CO,(s)+4NH, (aq) = 2[Ag(NH;) ] (@g) +CO} (aq)
c. 1.44x10+
d. 2.92x10-26 e. 1.18x107
22. Given the unbalanced equation V,05 + W VO+WO₂,
acidic solution, what will the coefficient of H₂O(l) be?
a. 2
c. 4
b. 3
Kp -8.46-10-12
K₁=5.88-10-8
when the overall reaction equation is balanced in
d. S e. There is no H₂O in the balanced equation](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F43965b80-42e8-41df-9b51-2c2200725cfe%2Fb689b989-d09d-4b05-b4cd-899cd2f77ab4%2Fapxufc9_processed.jpeg&w=3840&q=75)
![1.
ANS: E
2.
ANS: E
3. ANS: B
4.
ANS: A
5.
ANS: D
ANS: B
ANS: A
ANS: E
6.
7.
8.
9.
ANS: B
10.
ANS: D
11. ANS: B
12. ANS: E
13. ANS: A
14. ANS: A
15. ANS: A
ANS: D
ANS: A
18.
ANS: E
19.
ANS: B
20. ANS: B
21. ANS: A
22. ANS: C
16.
17.
23. ANS: C
24. ANS: C
25. ANS: C](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F43965b80-42e8-41df-9b51-2c2200725cfe%2Fb689b989-d09d-4b05-b4cd-899cd2f77ab4%2Fneoiq3g_processed.jpeg&w=3840&q=75)
![](/static/compass_v2/shared-icons/check-mark.png)
Step by step
Solved in 3 steps with 1 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)