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Chapter 14: Q14.3-48 E (page 830)

Are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in water directly proportional or inversely proportional? Explain your answer.

Short Answer

Expert verified

The concentrations of hydronium ion and hydroxide ion are inversely proportional in a water solution of an acid or a base.

Step by step solution

01

Ionization Constant

The ionization constant of water is defined by its name—it is constant at the given temperature.

02

Explanation

  • The ionization constant of water is \( > {K_w} = c\left( {{H_3}{O^ + }} \right)c\left( {O{H^ - }} \right).\)
  • The definition of ionization constant implies that no matter whether a solution is an acid or a base, the products of the concentrations of hydronium ion and hydroxide ion will remain the same.
  • Therefore, if the concentration of a hydronium ion rises, the concentration of a hydroxide ion will fall, and vice versa.
  • Hence, they are inversely proportional.

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Most popular questions from this chapter

A buffer solution is prepared from equal volumes of \({\bf{0}}.{\bf{200}}{\rm{ }}{\bf{M}}\) acetic acid and \({\bf{0}}.{\bf{600}}{\rm{ }}{\bf{M}}\) sodium acetate. Use \({\bf{1}}.{\bf{80}}{\rm{ }} \times {\rm{ }}{\bf{1}}{{\bf{0}}^{ - {\bf{5}}}}\) as Ka for acetic acid.

(a) What is the pH of the 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 \({\bf{0}}.{\bf{200}}{\rm{ }}{\bf{L}}\) of the original buffer?

Which acid in Table 14.2 is most appropriate for preparation of a buffer solution with a pH of 3.1? Explain your choice.

Calculate the concentration of each species present in a \(0.010M\) solution of phthalic acid, \({C_6}{H_4}{\left( {C{O_2}H} \right)_2}\).

\(\begin{array}{*{20}{c}}{{C_6}{H_4}{{\left( {C{O_2}H} \right)}_2}(aq) + {H_2}O(l) \rightleftharpoons {H_3}{O^ + }(aq) + {C_6}{H_4}\left( {C{O_2}H} \right){{\left( {C{O_2}} \right)}^ - }(aq)}&{{K_a} = 1.1 \times 1{0^{ - 3}}} \\ {{C_6}{H_4}\left( {C{O_2}H} \right)\left( {C{O_2}} \right)(aq) + {H_2}O(l) \rightleftharpoons {H_3}{O^ + }(aq) + {C_6}{H_4}{{\left( {C{O_2}} \right)}_2}^{2 - }(aq)}&{{K_a} = 3.9 \times 1{0^{ - 6}}} \end{array}\)

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

The ionization constant of lactic acid, \(C{H_3}CH(OH)C{O_2}H\), an acid found in the blood after strenuous exercise, is \(1.36 \times 1{0^{ - 4}}\). If \(20.0\;g\) of lactic acid is used to make a solution with a volume of \(1.00L\), what is the concentration of hydronium ion in the solution?
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