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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

Explain why the ionization constant, \({K_a}\), for\({H_2}S{O_4}\) is larger than the ionization constant for \({H_2}S{O_3}\).

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

Saccharin, \({{\bf{C}}_{\bf{7}}}{{\bf{H}}_{\bf{4}}}{\bf{NS}}{{\bf{O}}_{\bf{3}}}{\bf{H}}\), is a weak acid\(\left( {{\bf{Ka = 2}}{\bf{.1 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}} \right)\). If \({\bf{0}}.{\bf{250}}{\rm{ }}{\bf{L}}\) of diet cola with a buffered pH of \({\bf{5}}.{\bf{48}}\) was prepared from \({\bf{2}}.{\bf{00}}{\rm{ }} \times {\rm{ }}{\bf{1}}{{\bf{0}}^{ - {\bf{3}}}}{\bf{g}}\) of sodium saccharide, \({\bf{Na}}\left( {{{\bf{C}}_{\bf{7}}}{{\bf{H}}_{\bf{4}}}{\bf{NS}}{{\bf{O}}_{\bf{3}}}} \right)\), what are the final concentrations of saccharine and sodium saccharide in the solution?

Explain why the neutralization reaction of a weak acid and a strong base gives a weakly basic solution

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(a)\(KI\)

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(d)\(NaOH\)

(e)\(N{H_4}Cl\)
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