Arrange the following 0.1 M solutions in order of increasing pH NaCH3COO, HCl, HCN, NaOH, NH3, NaCN, KNO3, NH4Cl, H2SO3, NaHCO3, Na3PO4 and CH3COOH. (give a brief explanation as to why it is the position, e.g. strong acid/base, larger Ka or Kb etc.) Hint: read through the ‘useful information at the end of the lab’ In the case of the diprotic species (e.g. H2SO3 the major contribution to acidity comes from the first proton loss. The second typically a makes a much smaller contribution) H2SO3: This is a weak acid with Ka1 = 1.7 x 10-2. (This is the dissociation constant associated with the loss of the first proton) CH3COOH: This is a weak acid with Ka = 1.8 x 10-5. HCN: This is a weak acid with Ka = 5.8 x 10-10. Hydrogen carbonate is a weak base with Kb = 2.3 x 10-8. NH3: This is a weak base with Kb = 1.8 x 10-5. Na3PO4: The phosphate ion is a weak base with Kb = 2.2 x 10-2
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.
Arrange the following 0.1 M solutions in order of increasing pH NaCH3COO, HCl, HCN, NaOH, NH3, NaCN, KNO3, NH4Cl, H2SO3, NaHCO3, Na3PO4 and CH3COOH. (give a brief explanation as to why it is the position, e.g. strong acid/base, larger Ka or Kb etc.) Hint: read through the ‘useful information at the end of the lab’
In the case of the diprotic species (e.g. H2SO3 the major contribution to acidity comes from the first proton loss. The second typically a makes a much smaller contribution)
H2SO3: This is a weak acid with Ka1 = 1.7 x 10-2. (This is the dissociation constant associated with the loss of the first proton)
CH3COOH: This is a weak acid with Ka = 1.8 x 10-5.
HCN: This is a weak acid with Ka = 5.8 x 10-10.
Hydrogen carbonate is a weak base with Kb = 2.3 x 10-8.
NH3: This is a weak base with Kb = 1.8 x 10-5.
Na3PO4: The phosphate ion is a weak base with Kb = 2.2 x 10-2
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