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Chapter 14: Q2 CYL (page 765)

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

Short Answer

Expert verified

Hydronium [H3 O+] = 1.0× 10-11M

Step by step solution

01

To find the solution of hydroxide ion concentration of 0.001 M at 25̊C  

\begin{gathered} \left[ {O{H^ - }} \right] &= 0.001M \hfill \\K\omega & = \left[ {{H^ + }} \right]\left[ {o{H^ - }} \right] = 1{0^{ - 14}} \hfill \\ \left[ {{H^ + }} \right] &= \frac{{1{0^{ - 14}}}}{{[0H]}} &= \frac{{1{0^{ - 14}}}}{{0.001}}& = 1{0^{ - 11}}\;m \hfill \\ \left[ {{H_3}{o^ + }} \right] &= \left[ {{H^ + }} \right] &= 1.0 \times 1{0^{ - 11}}\;m \hfill \\ hydronium ion \left[ {{H_3}{o^ + }} \right] &= 1.0 \times 1{0^{ - 11}}M \hfill \\ \end{gathered}

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Most popular questions from this chapter

What are amphiprotic species? Illustrate with suitable equations.

A \({\bf{5}}{\bf{.36 g}}\) sample of \({\bf{N}}{{\bf{H}}_{\bf{4}}}{\bf{Cl}}\) was added to \({\bf{25}}.{\bf{0}}{\rm{ }}{\bf{mL}}\) of \({\bf{1}}{\bf{.00 M NaOH}}\) and the resulting solution diluted to\({\bf{0}}.{\bf{100}}{\rm{ }}{\bf{L}}\).

(a) What is the pH of this buffer solution?

(b) Is the solution acidic or basic?

(c) What is the pH of a solution that results when \({\bf{3}}.{\bf{00}}{\rm{ }}{\bf{mL}}\) of \({\bf{0}}.{\bf{034}}{\rm{ }}{\bf{M}}{\rm{ }}{\bf{HCl}}\) is added to the solution?

What is the ionization constant at \(2{5^o}C\) for the weak acid \({\left( {C{H_3}} \right)_2}NH_2^ + \), the conjugate acid of the weak base \({\left( {C{H_3}} \right)_2}NH\), \({K_b} = 5.9 \times 1{0^{ - 4}}\)?

Which base in Table 14.3 is most appropriate for preparation of a buffer solution with a pH of 10.65? Explain your choice.

Household ammonia is a solution of the weak base\(N{H_3}\) in water. List, in order of descending concentration, all of the ionic and molecular species present in a 1-M aqueous solution of this base.
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