2 A particular vinegar solution has a H₂O concentration of 0.0185 M. What is the pOH of the solution? A) 10.7 B) 17.3 C) 12.3 D) 15.8 What mass of othuls
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.
![Hint: (molar mass of H-1, N-14g/mol), (R-0.0821 L.atm/K.mol), (The specific heat of water is 4.184J/g. C)
.
1) Estimate the temperature where AG=0 for the following reaction: (Given: AH--195 kJ and
AS-284.5 J/K) CAUTION: Beware of units.NH3(g) + HCl(g)->NH4Cl(s)
A) 685 K
B) 467 K
C) 582 K
D) 634 K
2) Consider the reaction represented by the equation: N₂(g) + 3H₂(g) <-> 2NH3(g) Calculate the
equilibrium pressures at a certain temperature: PNH,-3.7 x 10 atm, PN-8.9x10 atm, PH:-2.9x 10 atm
A) 6.3x10*
B) 2.9x104
C) 5.3x10
D) 4.9 x10
3) Consider the following reaction:
2 N₂O(g)
If the half-life for the reaction is 0.810 s, the rate constant is:
A) 1.1 s¹¹
B) 0.86 s¹
4) Calculate AG for the reaction
->
COⓇ
CO₂(g)
CO
C) + 1/202)
Ca) + O₂
+1/202- CO₂(g)
A) 523 kJ
2 NO(g) + O₂(g); rate=1
C) 0.69 s¹
AG=??
AG°-454.4 kJ
AG=-257.2 kJ
C) 197.2 kJ
k[N₂0]
B)-265.8 kJ
D) 651.6 kJ
5) The volume of a sample of nitrogen N₂ is 9 L at 31°C and 732 torr. What volume will it occupy at STP?
A) 6.59 L
B) 7.18 L
C) 6.90 L
D) 7.78 L
6)
Which of the following pure substances exhibits hydrogen bonding?
A) HCI
B) H₂S
C) CH₂
D) 0.32 s¹
D) H₂O
7)
A particular vinegar solution has a H₂O* concentration of 0.0185 M. What is the pOH of the solution?
A) 10.7
B) 17.3
C) 12.3
D) 15.8
8)
What mass of ethylene glycol (M.W. = 62.1 g/mol) antifreeze must be added to 8.0 liters of water to
produce a solution that freezes at -23.3 C degrees. Density of water is 1 g/ml and Kr-186° C/m.
A) 3.41 g
B) 6.22 Kg
C) 7.81 kg
=
D) 0.78 kg
11) The OH concentration in a 0.09M of Ca(OH)2 solution is
A) 0.0075 M
B) 0.18 M
9) How much heat is required to raise the temperature of 1.5 g of water from 25°C to 27°C?
A) 12.55 kJ
B) 6.27 kJ
C) 1.55 kJ
D) 40.5 kJ
10) Calculate the osmotic pressure associated with 90.0 g of an enzyme of molecular weight 98,000 g/mol
dissolved in 2900 mL of benzene at 30.0 °C.
A) 5.99 torr
B) 1.96 torr
C) 0.484 torr
D) 2.48 torr
C) 1.3x10-12 M
D) 1x107 M
12) A solution of 7.00 MHCHO2 is 0.57% ionized in water. Calculate the Ka value for the acid (HCHO₂).
A) 2.5x10-³
B) 0.2x10-³
C) 2.3x104
D) 0.23](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48079d7c-7248-4f29-b2fc-02e5764ca6aa%2F7f745839-2565-40f9-9d69-9ae4bab35d7c%2Fa5xeqlr_processed.jpeg&w=3840&q=75)
1. pH = - log[H+]
2. pH + pOH = 14
3. H3O+ <---> H2O + H+ Above ions are in spontaneous equilibrium therefore concentration of H+ ions will be equal to H3O+ ions.
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