Depends on the pH, at low pH (below pH 7), the H+ ion concentration is greater, and high pH the OH- ion concentration is greater
pH = - log([H+]) , pOH = - log([OH-] , pH + pOH = 14 [X] = concentration of X
By observing the [H+] ion concentration and [OH-] concentration in the aqueous solution. If the [H+] ion concentration is higher that the [OH-] ion concentration, it is acidic. Vice Versa for basic.
the H+ concentration and the OH- concentration
It increases the concentration of OH- in solution. (apex)
Isotonic
pH = - log([H+]) , pOH = - log([OH-] , pH + pOH = 14 [X] = concentration of X
The concentration of H+ or OH-.
By observing the [H+] ion concentration and [OH-] concentration in the aqueous solution. If the [H+] ion concentration is higher that the [OH-] ion concentration, it is acidic. Vice Versa for basic.
the H+ concentration and the OH- concentration
It increases the concentration of OH- in solution. (apex)
Isotonic
Kw=[OH-][H+] 1.0X10^-14=[OH-][1.3] [OH-]=(1.0X10^-14)/(1.3) [OH-]=7.7
No it is false -it has a high concentration of H+ ions
The concentration of H +, or OH - ions donated to the solution.
pH is defined as -log[H+]. This means that if one knows the concentration of hydrogen ion in solution, the pH is simply the negative logarithm (base 10) of that. Similarly, one can find the pOH simply by substituting the concentration of OH- for the concentration of H+ in the aforementioned formula.
An arrhenius acid is, by definition, a solution with a higher concentration of H+ ion than OH-.
pH=10, means the concentration of OH- ions is 0.0001 M and concentration of H+ ions is 0.0000000001M