Question

Use the concentrations given to determine whether each of the following is acidic, neutral, or basic.A. [H+] = 4.3 × 10-3 mol/LB. [H+] = 9.8 × 10-12 mol/LC. [OH-] = 4.8 × 10-2 mol/L

Answer 1

We have the concentration of H+ ions, from these concentrations we can find the pH values of the solutions with the following equation:

`pH=-log\lbrack H^+\rbrack`

Where [H+] is the concentration of H+ ions.

Now, the acidity or basicity of a solution depends on the pH value. A solution above 7 will be basic, below 7 will be acidic, and equal to 7 will be neutral.

Let's determine the pH value for each solution:

`\begin{gathered} pH=-log\lbrack4.3*10^(-3)mol/L\rbrack \\ pH=2.4 \end{gathered}`
`\begin{gathered} pH=-log\lbrack9.8*10^(-12)mol/L\rbrack \\ pH=11.0 \end{gathered}`
`\begin{gathered} pH=-log\lbrack4.8*10^(-2)mol/L\rbrack \\ pH=1.3 \end{gathered}`

So, we have that:

A. [H+] = 4.3 × 10-3 mol/L. pH=2.4. Acidic

B. [H+] = 9.8 × 10-12 mol/L pH = 11.0 Basic

C. [OH-] = 4.8 × 10-2 mol/L pH=1.3 Acidic