A conductivity test of a dilute solution of nitrous acid (HNO 2(aq)) has very low electrical conductivity (the bulb on the tester glows dimly) and the pH is measured to be about 4. The same concentration of a nitric acid (HNO3(aq)) solution makes the conductivity tester’s bulb glow brightly and has a pH of less than 1. Explain the difference between these two acids.
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.
1. A conductivity test of a dilute solution of nitrous acid (HNO 2(aq)) has very low electrical conductivity (the bulb on the tester glows dimly) and the pH is measured to be about 4. The same concentration of a nitric acid (HNO3(aq)) solution makes the conductivity tester’s bulb glow brightly and has a pH of less than 1. Explain the difference between these two acids.
2. Design an experiment using sequential qualitative analysis to determine whether a solution contains acetate or carbonate ions. Include both written instructions and a diagram of your experiment. For each stage of the test, write net ionic equations for the reaction that produces the precipitate.
3. Use the following experimental titration data to calculate the concentration of the acid being analysed.
Observations: The initial solution of acetic acid (HC2H3O2) is clear and colourless. A few drops of phenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide (concentration 2.50 x 10-4 mol/L) is used as the titrant. As the mixture reaches the endpoint, flashes of pink colour are seen and the titrant is added drop by drop. The endpoint is reached when one drop of titrant turns the mixture a pale pink colour that does not fade.
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