Indicate whether each of the solutions in Problem 10-65 is acidic, basic, or neutral. a. 3.5 × 10 −3 M b. 4.7 × 10 −6 M c. 1.1 × 10 −8 M d. 8.7 × 10 −10 M
Indicate whether each of the solutions in Problem 10-65 is acidic, basic, or neutral. a. 3.5 × 10 −3 M b. 4.7 × 10 −6 M c. 1.1 × 10 −8 M d. 8.7 × 10 −10 M
Indicate whether each of the solutions in Problem 10-65 is acidic, basic, or neutral.
a. 3.5 × 10−3 M
b. 4.7 × 10−6 M
c. 1.1 × 10−8 M
d. 8.7 × 10−10 M
(a)
Expert Solution
Interpretation Introduction
Interpretation:
The molar hydronium ion concentration in aqueous solutions formed with the hydroxide ion concentration of 3.5×10-3 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.
Explanation of Solution
Given,
Hydroxide ion concentration = 3.5×10-3 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 3.5×10-3 M is 2.9×10-12 M.
The hydronium ion concentration is 2.9×10-12 M. As the concentration of H3O+ in aqueous solution is lesser than 1.0×10-7 M, the solution is basic.
(b)
Expert Solution
Interpretation Introduction
Interpretation:
The molar hydronium ion concentration in aqueous solutions formed with the hydroxide ion concentration of 4.7×10-6 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.
Explanation of Solution
Given,
Hydroxide ion concentration = 4.7×10-6 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+]=1.0×10-14M4.7×10-6M[H3O+]=2.1×10-9 M
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 4.7×10-6 M is 2.1×10-9 M.
The hydronium ion concentration is 2.1×10-9 M. As the concentration of H3O+ in aqueous solution is lesser than 1.0×10-7 M, the solution is basic.
(c)
Expert Solution
Interpretation Introduction
Interpretation:
The molar hydronium ion concentration in aqueous solutions formed with the hydroxide ion concentration of 1.1×10-8 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.
Explanation of Solution
Given,
Hydroxide ion concentration = 1.1×10-8 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+]=1.0×10-14M1.1×10-8M[H3O+]=9.1×10-7 M
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 1.1×10-8 M is 9.1×10-7 M.
The hydronium ion concentration is 9.1×10-7 M. As the concentration of H3O+ in aqueous solution is higher than 1.0×10-7 M, the solution is acidic.
(d)
Expert Solution
Interpretation Introduction
Interpretation:
The molar hydronium ion concentration in aqueous solutions formed with the hydroxide ion concentration of 8.7×10-10 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.
Explanation of Solution
Given,
Hydroxide ion concentration = 8.7×10-10 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+]=1.0×10-14M8.7×10-10M[H3O+]=1.1×10-5 M
The molar hydronium ion concentration in aqueous solutions with the hydroxide ion concentration of 8.7×10-10 M is 1.1×10-5 M.
The hydronium ion concentration is 1.1×10-5 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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