The value of [OH - ] in aqueous solutions with the hydronium ion concentration of 5 .5×10 -2 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 value of [OH - ] in aqueous solutions with the hydronium ion concentration of 5 .5×10 -2 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 value of [OH-] in aqueous solutions with the hydronium ion concentration of 5.5×10-2 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,
Hydronium ion concentration= 5.5×10-2 MIon product constant for water = 1.0×10−14 M
To calculate the molar hydronium ion concentration in aqueous solutions
Kw=[H3O+][OH-][OH-]=Kw[H3O+][OH-]=1.0×10-14M5.5×10-2M[OH-]=1.8×10-13 M.
The [OH-] in aqueous solutions with the hydronium ion concentration of 5.5×10-2 M is 1.8×10-13 M.
The hydronium ion concentration is 5.5×10-2 M and the hydroxide ion concentration is 1.8×10-13 M. As hydronium ion concentration is higher, the solution will be acidic.
(b)
Interpretation Introduction
Interpretation:
The value of [OH-] in aqueous solutions with the hydronium ion concentration of 9.4×10-5 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,
Hydronium ion concentration= 9.4×10-5 MIon product constant for water = 1.0×10−14 M
To calculate the molar hydronium ion concentration in aqueous solutions
Kw=[H3O+][OH-][OH-]=Kw[H3O+][OH-]=1.0×10-14M9.4×10-5M[OH-]=1.1×10-10 M.
The [OH-] in aqueous solutions with the hydronium ion concentration of 9.4×10-5 M is 1.1×10-10 M.
The hydronium ion concentration is 9.4×10-5 M and the hydroxide ion concentration is 1.1×10-10 M. As hydronium ion concentration is higher, the solution will be acidic.
(c)
Interpretation Introduction
Interpretation:
The value of [OH-] in aqueous solutions with the hydronium ion concentration of 2.3×10-7 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,
Hydronium ion concentration= 2.3×10-7 MIon product constant for water = 1.0×10−14 M
To calculate the molar hydronium ion concentration in aqueous solutions
Kw=[H3O+][OH-][OH-]=Kw[H3O+][OH-]=1.0×10-14M2.3×10-7 M[OH-]=4.3×10-8 M.
The [OH-] in aqueous solutions with the hydronium ion concentration of 2.3×10-7 M is 4.3×10-8 M.
The hydronium ion concentration is 2.3×10-7 M and the hydroxide ion concentration is 4.3×10-8 M. As hydronium ion concentration is higher, the solution will be acidic.
(d)
Interpretation Introduction
Interpretation:
The value of [OH-] in aqueous solutions with the hydronium ion concentration of 6.6×10-12 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,
Hydronium ion concentration= 6.6×10-12 MIon product constant for water = 1.0×10−14 M
To calculate the molar hydronium ion concentration in aqueous solutions
Kw=[H3O+][OH-][OH-]=Kw[H3O+][OH-]=1.0×10-14M6.6×10-12 M[OH-]=1.5×10-3 M.
The [OH-] in aqueous solutions with the hydronium ion concentration of 6.6×10-12 M is 1.5×10-3 M.
The hydronium ion concentration is 6.6×10-12 M and the hydroxide ion concentration is 1.5×10-3 M. As hydronium ion concentration is lesser, the solution will be basic.
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Given the equation of the line, y=150x-8.1221 (cells per mL is in 10^8), what is the CFU per mL of the original suspension if the thousand-fold dilution of that suspension has an absorbance of 0.3 at 600nm? *
A. 3.7 x 10^12
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