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Chapter 14: QCYL (page 768)

Check your learning the ion product of water at \(8{0^^\circ }C\) is \(2.4 \times 1{0^{ - 13}}.\) What are the concentrations of hydronium and hydroxide ions in pure water at\(8{0^^\circ }C\) ?

Short Answer

Expert verified

Kw is called the equilibrium constant of water means dissociation and ionization of water at 25 Celsius which accounts to about 10-14 at 25 degrees centigrade.

\(\left[ {{H^ + }} \right] = {K_w}\left[ {{H^ + }} \right] = \sqrt {2.44 \times 1{0^{ - 13}}} \)

\(\left[ {O{H^ - }} \right] = 4.94 \times 1{0^{ - 7}}moles/lit\)

Step by step solution

01

Kw value  based on the question given above

\(\) \(\begin{array}{l}{K_W} = \left[ {{H^ + }} \right]\left[ {O{H^ - }} \right]\\{K_w} = 2.44 \times 1{0^{ - 13}} \\\end{array}\)

02

STEP:2 To find the concentration of hydroxide ion:

For pure water hydroxide and hydrogen concentration are equal which is given as

\(\begin{array}{l}For pure water \left[ {{H^ + }} \right] = \left[ {O{H^ - }} \right]\\\left[ {{H^ + }} \right] = {K_w}\left[ {{H^ + }} \right] = \sqrt {2.44 \times 1{0^{ - 13}}} \\ = 4.94 \times 1{0^{ - 7}} moles / it \\\left[ {O{H^ - }} \right] = 4.94 \times 1{0^{ - 7}} moles/lit \end{array}\)

Thus hydroxide ion concentration is\(4.94 \times 1{0^{ - 7}} moles/lit \)

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Most popular questions from this chapter

What is the effect on the concentration of ammonia, hydroxide ion, and ammonium ion when the following are added to a basic buffer solution of equal concentrations of ammonia and ammonium nitrate:

(a)\(KI\)

(b)\(N{H_3}\)

(c)\(HI\)

(d)\(NaOH\)

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

Calculate the concentration of each species present in a \(0.050 - M\) solution of \({H_2}\;S. \)

Use this list of important industrial compounds (and Figure 14.8) to answer the following questions regarding: \(CaO,Ca{(OH)_2},NaOH,C{H_3}C{O_2}H,{H_2}C{O_3},HF,HN{O_2},{H_3}P{O_4},HCl,HN{O_3},{H_2}S{O_4},N{H_3}\) (a) Identify the strong Brønsted-Lowry acids and strong Brønsted-Lowry bases. (b) List those compounds in (a) that can behave as Brønsted-Lowry acids with strengths lying between those of \({H_3}{O^ + }and\;{H_2}O\). (c) List those compounds in (a) that can behave as Brønsted-Lowry bases with strengths lying between those

\({H_2}O\;and\;O{H^ - }\)

What is the ionization constant at 25oC for the weak acid \(C{H_3}NH_3^ + \), the conjugate acid of the weak base \(C{H_3}N{H_2}\)\({K_b} = 4.4 \times 1{0^{ - 4}}\) ,.

Predict which acid in each of the following pairs is the stronger and explain your reasoning for each. \(\;(a)\;{H_2}O\;or\;HF,\;(b)\;B{(OH)_3}\;or\;Al{(OH)_3},\;(c)\;HSO_3^ - or\;HSO_4^ - ,\;(d)\;N{H_3}\;or\;{H_2}S,\;(e)\;{H_2}O\;or\;{H_2}Te\)
See all solutions

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