Chapter 14 Acids and Bases
Which of the three acid definitions is the broadest? Explain.
Polyprotic acids are acids that donate more than one protons (hydrogen ions) per molecule. This definition is by far the most broad since it does not specify the amount of protons releases with each acid.
What determines the strength of an Arrhenius base? Give one example each of an aqueous solution of a strong base and an aqueous solution of a weak base.
Arrhenius base strength is determined by the amount of increase of hydroxide concentration in aqueous solution. Strong bases are bases that ionize completely in aqueous solution would be NaOH and a weak base which only releases a few hydroxide ions would be NH₃
Distinguish between binary acids and oxyacids in terms of their component elements and the systems used in naming them. Give three examples of each type of acid
Binary acids are composed of mainly two elements : hydrogen and a more electronegative element. They typically end with the suffix "ic" and begin with the prefix "hydro" and end with the work "acid". Oxyacids, on the other hand, have three elements: hydrogen, oxygen, and some nonmetal. The higher the subscript of the nonmetal follows with the suffix "ic" and the lower subscript ends with the suffix "ous".
Identify and describe the characteristic properties of five common acids used in industry. Give some examples of typical uses of them.
Five common acids used for industrial purposes include sulfuric acid, nitric acid, acetic acid, hydrochloric acid, and hydrofloric acid. Sulfuric acid is used to oxygen iron during steel manufacturing. Nitric acid use is common in the production of fertilizers. Acetic acids are used as solutions of PVC plastic in gelatin. Hydrofloric acid is used in making teflon and prozac.
Compare the general properties of acids with the general properties of bases
General properties of acids include their available reactivity with most metals to form hydrogen gas, having a sour taste, feeling sticky, and usually are gases or liquids. Properties of bases include feeling slippery, tasting bitter, reacting with both oils and greases and are frequently solid states of matter.
write formulas for the following oxyacids:perbromic acid, cholorous acid, phosphoric acid, hypocholorous acid
HBrO₄, H₃Po₄, HClO₂, HClO
Although HCl exhibits properties of an arrhenius acid, pure hydrochloric gas and HCl dissolved in a nonpolar solvent exhibit none of the properties of an arrhenius acid. Explain why.
HCl exhibits nonpolar covalent bonding so the HCl soultion wold possess more arrhenius basic properties. This could lead to an increased concentration of hydroxide ions in aqueous solution.
Write formulas for the following binary acids:hydrofluoric acid, hydroiodic acid
HF, and HI
Distinguish between a monoprotic, a diprotic acid, and a triprotic acid. Give an example of each.
Monoprotic acids donate one hydrogen ions per molecule. Diprotic acids donate two hydrogen ions (protons) per molecule. H₂SO₄ is diprotic and HF is monoprotic. Triprotic acids are acids that donate three protons per molecule. H₃PO₄ is triprotic.
What distinguishes strong acids from weak acids? Give two examples each of strong acids and weak acids.
Strong acids are acids that ionize completely in aqueous solution. On the other hand, weak acids are acids in which only a few hydrogen ions are released in an aqueous solution. Strong acids include hydroiodic acid, hydrobromic acid, hydrochloric acid and trichloroatic acid.
H₃PO₄, which contains three hydrogen atoms per molecule, is a weak acid, whereas HCl, which contains only one hydrogen atom per molecule is a strong acid. Explain why.
Weak acids are acids that only releases a few hydrogen ions in aqueous solution. In this way, phosphoric acids contain more hydrogen ions that have not dissolved completely. On the other hand, hydrochloric acid has ionized more completely leading to only one hydrogen atom per molecule.
Name each of the following binary acids:
a. HCl-hydrochloric acid b. H₂S-hydrosulfuric acid
Name each of the following oxyacids:
a. HNO₃-nitric acid b. H₂SO₃-sulfurous acid c. HClO₃-sulfuric acid d. HNO₃-nitrous acid
