Question

Calculate [H +] and [OH﹘] Milk, pH = 6.36

Answer 1

`\begin{gathered} \begin{equation*} [H^+]=4.36*10^(-7)M \end{equation*} \\ \begin{equation*} [OH^-]=2.29*10^(-8)M \end{equation*} \end{gathered}`

Explanations:

The formula for calculating the pH of a solution is expressed as:

`pH=-log[H^+]`

Given the following parameter

pH =. 6.36

Substitute

`\begin{gathered} 6.36=-log[H^+] \\ log[H^+]=-6.36 \\ [H^+]=10^(-6.36) \\ [H^+]=4.36*10^(-7)M \end{gathered}`

Determine the concentration of [OH-] in the solution

`\begin{gathered} [H^+][OH^-]=1.0*10^(-14) \\ [OH^-]=(1.0*10^(-14))/([H^+]) \\ [OH^-]=(1.0*10^(-14))/(4.36*10^(-7)) \\ [OH^-]=0.229*10^(-14+7) \\ [OH^-]=0.229*10^(-7) \\ [OH^-]=2.29*10^(-8)M \end{gathered}`