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Chapter 14: Q14.3-44 E (page 830)

Both \(HF and HCN\)ionize in water to a limited extent. Which of the conjugate bases \(F - or CN - \), is the stronger base? See Table 14.3.

Short Answer

Expert verified

\(C{N^ - }\) is the stronger base.

Step by step solution

01

Define strong base

A strong base is a substance capable of removing a proton from a very weak acid. In water, they completely dissociate into their ions.

02

Compare the stronger base

We have to identify which of the conjucate bases \(F - or CN - \) is the stronger base. We know that the stronger an acid, the weaker is its conjugated base pair. To identify the stronger base, compare the \({K_b}\)values of weak bases and not weak acids. The stronger acids will have higher \({K_a}\)values. \(HF\) has a higher \({K_a}\) value than \(HCN.\) \(HF\) is a stronger acid than \(HCN\). \({F^ - }\) is a weaker base than \(C{N^ - }\) because its conjugated acid is a stronger acid than the conjugated acid of \(C{N^ - }.\)

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Most popular questions from this chapter

What are the\(pH\;and\;pOH\) of a solution of \(2.0\)\(M\)\(HCl\), which ionizes completely?

The pH of a \(0.20 - M\) solution of \(HF\) is \(1.92.\) Determine \({K_a}\) for \(HF\) from these data.

14.2 What is the hydronium ion concentration in an aqueous solution with a hydroxide ion concentration of 0.001 M at 25̊C?

Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:

\({\rm{\;(a)\;NO}}_2^ - + {{\rm{H}}_2}{\rm{O}} \to {\rm{HN}}{{\rm{O}}_2} + {\rm{O}}{{\rm{H}}^ - }\).

\({\rm{\;(b)\;HBr}} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_3}{{\rm{O}}^ + } + {\rm{B}}{{\rm{r}}^ - }\)

\({\rm{\;(c)\;H}}{{\rm{S}}^ - } + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_2}{\rm{S}} + {\rm{O}}{{\rm{H}}^ - }\)

\({\rm{\;(d)\;}}{{\rm{H}}_2}{\rm{PO}}_4^ - + {\rm{O}}{{\rm{H}}^ - } \to {\rm{HP}}{{\rm{O}}_4}^{2 - } + {{\rm{H}}_2}{\rm{O}}\)

\({\rm{\;(e)\;}}{{\rm{H}}_2}{\rm{PO}}_4^ - + {\rm{HCl}} \to {{\rm{H}}_3}{\rm{P}}{{\rm{O}}_4} + {\rm{C}}{{\rm{l}}^ - }\)

\({\rm{\;(f)\;}}{\left( {{\rm{Fe}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_5}({\rm{OH}})} \right)^{2 + }} + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{3 + }} \to {\left( {{\rm{Fe}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{3 + }} + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_5}({\rm{OH}})} \right)^{2 + }}\)

\({\rm{\;(g)\;C}}{{\rm{H}}_3}{\rm{OH}} + {{\rm{H}}^ - } \to {\rm{C}}{{\rm{H}}_3}{{\rm{O}}^ - } + {{\rm{H}}_2}\)

State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species.

\({\rm{\;(a)\;N}}{{\rm{H}}_3}\)

\({\rm{\;(b)\;HPO}}_4^ - \)

\({\rm{\;(c)\;B}}{{\rm{r}}^ - }\).

\({\rm{\;(d)\;N}}{{\rm{H}}_4} + \)

\({\rm{\;(e)\;ASO}}_4^{3 - }\).
See all solutions

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