What is [H3O+] for normal aspirin?
What is [HO-] in distilled water?
What is [H3O+] for shampoo?
What is the pOH of tap water?
What is the pOH of normal aspirin?
Regular aspirin will dissolve in water, which has a pH of approximately 7.0. This pH is found in the mouth.
Regular aspirin or buffered aspirin will dissolve in acid. An acidic pH is found in the stomach (pH < 4.0).
Enteric aspirin will dissolve in a base. A basic pH is found in the intestines (pH > 8.0).
As aspirin is a weak acid, [H3O+ ] must be calculated to find
pH
So ,pH and [H3O+] are related as . pH of asprin depends upn the
cncentration of its solution at a particular temperature.
Because,pH + pOH = 14,therefore you can find pOH of normal aspirin after Calculating the pH value.
For Distilled water and tap water, the pH value can vary from 0 to 14. As we know,Solutions with a pH between 0 and 7 are acidic, while those with a pH between 7 and 14 are basic. Pure distilled water should be neutral with a pH of 7, but because it absorbs carbon dioxide from the atmosphere, it's actually slightly acidic with a pH of 5.8.
To a very small but very important extent, water is a weak acid that ionizes to hydrogen and hydroxide ions.
In pure water, the hydrogen ion concentration, [H+], equals the hydroxide ion concentration, [OH-]. These concentrations can be calculated from the equation for the ionization of water.Let x equal the hydrogen ion concentration, [H+]. Then x also equals the hydroxide ion concentration, [OH-].
[H+][OH-] = | (x)(x) = 1 X 10-14 |
x2 = | 1 X 10-14 |
x = | 1 X 10-7 |
[H+] = | [OH-] = 1 X 10-7 M |
Hydroxide ion concentration in an acid solution the following relationships exist whenever water is present,Suppose the hydrogen ion concentration is 0.10 M,then
[H+][OH-] = 1 X 10-14 and pH + pOH = 14
[OH-] = | 1.0 X 10-14 /0.10 | = 1 X 10-13 M |
Suppose the pH of an acidic solution is 1.0.Then,
1.0 + pOH = 14 pOH = 13
If ,A shampoo has a pH of 8.56,then
[H3O+] = 10^-8.56 = 2.7 × 10^-9 M
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