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.
![of the Clements
3. The reaction 2HCN
PHcx = 0.45 atm
a) Is reaction at equilibrium?
C₂N₂ + H₂ (K = 0.17) is performed with PC2N2 = P2 = 0.32 atm and
b) If not, which way will it shift?
c) What will the equilibrium pressures be?
4. Which direction would the reaction 4NH3 + 30₂ 2N₂ + 6H₂O (AH = -1530 kJ) shift if:
a) N₂ is added b) pressure is lowered c) temperature is raised d) O₂ is removed
5. Label the conjugate acid-base pair for each of the following:
a) HNO, + OH = NO; + H,O b) C,H,NH, +CH,CO; =CH,NH, +CH,CO,H
6. Calculate the pH of the following solutions:
a) 5.2 x 104 HNO3
b) 0.11 M solution of HC,H,O, (K = 8.0 x 10¹5)
7. A 0.10 M solution of NaOH is used to titrate 20 mL of 0.18 M HCHO₂ (K = 1.8 x104):
a) What volume of NaOH is required to reach the equivalence point?
b) What is the pH at the midpoint of the titration?
c) What is the pH at the equivalence point?
8. A buffer is made by adding 8.5 grams of formic acid (HCHO₂, K = 1.9 x 104) to 0.2 moles of its
conjugate base in 500 mL of water.
a) What is the pH of the buffer?
b) What will the pH be after 0.02 moles of NaOH, a strong base, are added?
9. What is the maximum concentration of A1³+ which can exist in a solution with a pH of 9.7 (Ksp Al(OH)
= 2 x 10-³¹)?
10. The compound MgF₂ has K= 7 x 10-¹¹. What is the solubility of MgF₂ in pure water?
11: For each of the following; give the name, geometry, coordination number for the central cation and
draw and identify any possible isomers:
a) [Cr(CN),(H₂O)]²-
b) [Ni(H₂O)₂Br₂]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7120606c-99fa-4a80-8ac4-42c015833f0a%2F4434db68-4a81-4c5b-8adb-1b07dad374f6%2Ffrpmzc_processed.jpeg&w=3840&q=75)
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