there are more H+ ions in a pH 2 solution that in a pH 4 solution. The hydrogen ion (H+ ion) is responsible for the acidity of a substance and so, the more of it there is, the more acidic it is (higher acidity= lower pH) :)
1000 times more at pH = 10
(Calculation: 10-[pH2-pH1] = 10-(13-10) = 103 )
The ion H+ concentration is higher in the ratio 100:1.
100
pH = 2
10000
x10
pH is -log10[H3O+]; the negative logarithm (with base 10) of the hydronium concentration (hydrogen ions do not float around on their own. Instead they attach to a water molecule and become a hydronium ion).
When an aqueous solution of sodium hydroxide is electrolyzed, hydrogen is produced at the cathode because hydrogen can be produced at a lower voltage than can sodium, and the supply of hydrogen from the water of the solution is sufficient to consume all the current supplied. When molten sodium chloride is electrolyzed, however, sodium is produced at the cathode.
Usually hydrogen will evolve from the cathode and oxygen from the anode, but if zinc is the anode, it may dissolve to produce zinc ions in the solution either instead of or along with oxygen evolving.
All acidic substances contain hydrogen. Not only this, but acidic substances must be able to "donate" a hydrogen ion (proton) to an aqueous solution. In case you needed to know, bases are the same, except instead of hydrogen, they have hydroxide (OH).
You can dilute by adding distilled water. When diluting, be sure to add the solution to water several times instead of adding water to the solution (especially if it is highly concentrated).
It's not that the concentration of H+ ions goes up because pH goes up. Instead, the pH goes down because H+ concentration increases. I know that's a really subtle difference, but it is crucial. If you're good at math this may help: pH= -log [H+] where [H+] simply means concentration of hydrogen ions. So, you can see from this formula that as the concentration of hydrogen ions increase, the pH will decrease because it is a negative log. You can also see that the pH is a function of hydrogen concentration. I hope that clears some ideas up for you. Good luck!
pH is -log10[H3O+]; the negative logarithm (with base 10) of the hydronium concentration (hydrogen ions do not float around on their own. Instead they attach to a water molecule and become a hydronium ion).
When an aqueous solution of sodium hydroxide is electrolyzed, hydrogen is produced at the cathode because hydrogen can be produced at a lower voltage than can sodium, and the supply of hydrogen from the water of the solution is sufficient to consume all the current supplied. When molten sodium chloride is electrolyzed, however, sodium is produced at the cathode.
Usually hydrogen will evolve from the cathode and oxygen from the anode, but if zinc is the anode, it may dissolve to produce zinc ions in the solution either instead of or along with oxygen evolving.
Molten salt electrolysis is used to obtain sodium and chlorine. Electrolysis of the water solution is used to obtain sodium hydroxide and hydrogen.
All acidic substances contain hydrogen. Not only this, but acidic substances must be able to "donate" a hydrogen ion (proton) to an aqueous solution. In case you needed to know, bases are the same, except instead of hydrogen, they have hydroxide (OH).
Helium is used instead of hydrogen because it is nonflammable.
when an aqueous solution is used, hydrogen gas is evolved at cathode, instead of depositing sodium metal.
Water that contains hydrogen-2 instead of hydrogen-1 is called heavy water.
Hydrogen does not support burning, instead it completely burns.
You can dilute by adding distilled water. When diluting, be sure to add the solution to water several times instead of adding water to the solution (especially if it is highly concentrated).
The text is asking why a solution of oleic acid that has been weakened with water is used instead of pure oleic acid. Oleic acid is a type of fatty acid commonly found in animal and vegetable fats and oils. Diluting the solution may be necessary for certain applications to achieve a desired concentration or to prevent adverse effects.