HCN (aq) + HCO3(aq) → CN- (aq) + H₂CO3(aq) If K <1,what is the (a) strongest acid and the strongest base 2A Which of the species in # 1 can act as both a Bronsted acid and a Bronsted base
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.
![Chapter -
4A Given:
HCN (aq) + HCO 3 (aq) → CN- (aq) + H₂CO3 (aq)
If K <1, what is the (a) strongest acid
and the strongest base
2A Which of the species in # 1 can act as both a Bronsted acid and a Bronsted base
?
BA solution of 8.0 M formic acid (HCOOH) is 0.47 % ionized. What is the pH of the solution and Ka
of HCOOH ?
What is the pH of 0.10 M sodium carbonate solution ?Ka1 = 4.3 x 107 and Ka2= 5.6x10-¹¹ for
H₂CO3(aq)
What is the pH of a solution prepared by mixing 50.0 mL of a 0.10M solution of HF with 25.0 mL
of a 0.20M solution of NaF? pka of HF = 3.14
€ What is the pH of the solution prepared by adding 5.00 mL of 0.10M NaOH to solution in #5?
F How much solid NaCN must be added to 1.0 L of a 0.50M HCN solution to give a pH of 7.00 ?
Ka HCN= 6.2 x 10-10.
We add some ammonium sulfate to water .What is the nature of the solution ,neutral, acidic, or
basic. Write the hydrolysis equations and using Ka (NH4* )= 5.6x10-10 and Kb (SO42) -8.3x10-¹3
Explain your reasoning.
H. 0.0100 mole of a weak acid (HA) was dissolved in water to make a 100.0 mL solution. A titration
was performed using 0.100 M NaOH.After 40.00 mL of base was added the pH was 4.00. What is
the Ka of the acid HA?
Calculate the pH at the equivalence point when 0.104 g sodium acetate (MM-82.0,Kb-5.6x10-10)
Is dissolved in water to make 25.0 mL of solution and titrated with 0.0996M HCL (aq)
A solution is 0.10M in FeCl₂. What is the pH necessary to just prevent the formation of iron (II)
sulfide when the solution is saturated with H₂S ? Ka1, H₂S= 1.00 x107,Ka2, HS-= 1.3 x10-13; Ksp
FeS=4.9x10-18](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdc1887eb-3481-4b27-95d7-11eb29d76f4f%2F455cc570-f7c4-4420-a4d3-03d607186acc%2Flkf55t7_processed.jpeg&w=3840&q=75)
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