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Question: Is \({H^ + }\) equal \(O{H^ - }\) ?...

Is H+{H^ + } equal OH−O{H^ - } ?

Explanation

Solution

There is a link between the [H+]\left[ {{H^ + }} \right] ion and the [OH−]\left[ {O{H^ - }} \right] ion, just as there is between pH and pOH. We spoke about how the other changed as the pH or pOH changed. This holds true for both the [H+]\left[ {{H^ + }} \right] and [OH−]\left[ {O{H^ - }} \right] ions. The [H+]\left[ {{H^ + }} \right] and [OH−]\left[ {O{H^ - }} \right] ions are measured by pH and pOH, therefore if pH and pOH change, so do the [H+]\left[ {{H^ + }} \right] and [OH−]\left[ {O{H^ - }} \right] ions.

Complete answer:
Acids and bases are commonly dissolved in water when making solutions. As a result, the solutions are referred to as "aqueous" solutions. In water, acids and bases behave like salts, dissociating or breaking apart into their ions. The pH or pOH is calculated by counting how many of these ions are present in a solution.
The hydrogen ion concentration, [H+]\left[ {{H^ + }} \right] , equals the hydroxide ion concentration, [OH−]\left[ {O{H^ - }} \right] , in pure water.
Let [H+]\left[ {{H^ + }} \right] be the concentration of hydrogen ions. The hydroxide ion concentration, [OH−]\left[ {O{H^ - }} \right] , is also equal to XX . We get by substituting into the equilibrium expression
[H+][OH−]=(X)(X)=1×10−14\left[ {{H^ + }} \right]\left[ {O{H^ - }} \right] = \left( X \right)\left( X \right) = 1 \times {10^{ - 14}}
X2=1×10−14{X^2} = 1 \times {10^{ - 14}}
X=1×10−7X = 1 \times {10^{ - 7}}
[H+]=[OH−]=1×10−7M\left[ {{H^ + }} \right] = \left[ {O{H^ - }} \right] = 1 \times {10^{ - 7}}M
The equation for water ionisation can be used to get these concentrations. Pure water has a pH of 7, which is the negative logarithm of 1×10−71 \times {10^{ - 7}} . The term "neutral" refers to a solution that is neither acidic nor basic. The concentration of hydrogen ions equals the concentration of hydroxide ions, and both are 1×10−71 \times {10^{ - 7}} M. Thus, pH = pOH = 7 in a neutral solution.

Note:
The hydrogen ion concentration is greater than the hydroxide ion concentration in an acidic solution; in other words, the hydrogen ion concentration is larger than 1×10−71 \times {10^{ - 7}} M and the hydroxide ion concentration is less than 1×10−71 \times {10^{ - 7}} M. A pH of less than 7 indicates an acidic solution.