The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 4 .2×10 -4 M has to be indicated as acidic, basic or neutral. Concept Introduction: Dissociation constant of water: The dissociation of water can be given as H 2 O (l) + H 2 O (l) ⇄ H 3 O + (aq) + OH - (aq) The concentrations of H 3 O + and OH - at room temperature are 1 .0×10 -7 M each. [H 3 O + ] = [OH - ] = 1 .0×10 -7 If concentration of H 3 O + is higher than 1 .0×10 -7 M , it is said to be acidic solution. If concentration of OH − is higher than 1 .0×10 -7 M , it is said to be basic solution.
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 4 .2×10 -4 M has to be indicated as acidic, basic or neutral. Concept Introduction: Dissociation constant of water: The dissociation of water can be given as H 2 O (l) + H 2 O (l) ⇄ H 3 O + (aq) + OH - (aq) The concentrations of H 3 O + and OH - at room temperature are 1 .0×10 -7 M each. [H 3 O + ] = [OH - ] = 1 .0×10 -7 If concentration of H 3 O + is higher than 1 .0×10 -7 M , it is said to be acidic solution. If concentration of OH − is higher than 1 .0×10 -7 M , it is said to be basic solution.
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 4.2×10-4 M has to be indicated as acidic, basic or neutral.
Concept Introduction:
Dissociation constant of water:
The dissociation of water can be given as
H2O(l) + H2O(l)⇄H3O+(aq) + OH-(aq)
The concentrations of H3O+ and OH- at room temperature are 1.0×10-7 M each.
[H3O+] = [OH-] = 1.0×10-7
If concentration of H3O+ is higher than 1.0×10-7 M, it is said to be acidic solution.
If concentration of OH− is higher than 1.0×10-7 M, it is said to be basic solution.
(a)
Expert Solution
Explanation of Solution
Given,
Hydroxide ion concentration = 4.2×10-4 MIon product constant for water = 1.0×10−14 M
To calculate the molar hydronium ion concentration in aqueous solutions
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 4.2×10-4 M is 2.4×10-11 M.
The hydronium ion concentration is 2.4×10-11 M. As the concentration of H3O+ in aqueous solution is lesser than 1.0×10-7 M, the solution is basic.
(b)
Interpretation Introduction
Interpretation:
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 6.0×10-5 M has to be indicated as acidic, basic or neutral.
Concept Introduction:
Dissociation constant of water:
The dissociation of water can be given as
H2O(l) + H2O(l)⇄H3O+(aq) + OH-(aq)
The concentrations of H3O+ and OH- at room temperature are 1.0×10-7 M each.
[H3O+] = [OH-] = 1.0×10-7
If concentration of H3O+ is higher than 1.0×10-7 M, it is said to be acidic solution.
If concentration of OH− is higher than 1.0×10-7 M, it is said to be basic solution.
(b)
Expert Solution
Explanation of Solution
Given,
Hydroxide ion concentration = 6.0×10-5 MIon product constant for water = 1.0×10−14 M
To calculate the molar hydronium ion concentration in aqueous solutions
Kw=[H3O+][OH-][H3O+]=Kw[OH-][H3O+]=1.0×10-14M6.0×10-5 M[H3O+]=1.7×10-10 M
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 6.0×10-5 M is 1.1×10-10 M.
The hydronium ion concentration is 1.1×10-10 M. As the concentration of H3O+ in aqueous solution is lesser than 1.0×10-7 M, the solution is basic.
(c)
Interpretation Introduction
Interpretation:
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 3.4×10-9 M has to be indicated as acidic, basic or neutral.
Concept Introduction:
Dissociation constant of water:
The dissociation of water can be given as
H2O(l) + H2O(l)⇄H3O+(aq) + OH-(aq)
The concentrations of H3O+ and OH- at room temperature are 1.0×10-7 M each.
[H3O+] = [OH-] = 1.0×10-7
If concentration of H3O+ is higher than 1.0×10-7 M, it is said to be acidic solution.
If concentration of OH− is higher than 1.0×10-7 M, it is said to be basic solution.
(c)
Expert Solution
Explanation of Solution
Given,
Hydroxide ion concentration = 3.4×10-9 MIon product constant for water = 1.0×10−14 M
To calculate the molar hydronium ion concentration in aqueous solutions
Kw=[H3O+][OH-][H3O+]=Kw[OH-][H3O+]=1.0×10-14M3.4×10-9 M[H3O+]=2.9×10-6 M
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 3.4×10-9 M is 2.9×10-6 M.
The hydronium ion concentration is 2.9×10-6 M. As the concentration of H3O+ in aqueous solution is higher than 1.0×10-7 M, the solution is acidic.
(d)
Interpretation Introduction
Interpretation:
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 7.3×10-11 M has to be indicated as acidic, basic or neutral.
Concept Introduction:
Dissociation constant of water:
The dissociation of water can be given as
H2O(l) + H2O(l)⇄H3O+(aq) + OH-(aq)
The concentrations of H3O+ and OH- at room temperature are 1.0×10-7 M each.
[H3O+] = [OH-] = 1.0×10-7
If concentration of H3O+ is higher than 1.0×10-7 M, it is said to be acidic solution.
If concentration of OH− is higher than 1.0×10-7 M, it is said to be basic solution.
(d)
Expert Solution
Explanation of Solution
Given,
Hydroxide ion concentration = 7.3×10-11 MIon product constant for water = 1.0×10−14 M
To calculate the molar hydronium ion concentration in aqueous solutions
Kw=[H3O+][OH-][H3O+]=Kw[OH-][H3O+]=1.0×10-14M7.3×10-11 M[H3O+]=1.4×10-4 M
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 7.3×10-11 M is 1.4×10-4 M.
The hydronium ion concentration is 1.4×10-4 M. As the concentration of H3O+ in aqueous solution is higher than 1.0×10-7 M, the solution is acidic.
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