🤓 Based on our data, we think this question is relevant for Professor Hershberger-Kilyanek's class at UARK.

Determine the pH of each of the following solutions.

2.05×10^{−2} M KOH

We’re being asked to **d****etermine the pH** of** 2.05 × 10**^{−2 }**M KOH** solution.

Recall that the **pH and pOH **of a compound determine its acidity and basicity.

• **pH**

▪ pH stands for the negative logarithmic function of hydronium ion concentration**▪** can be calculated using the following equation:

$\overline{){\mathbf{pH}}{\mathbf{=}}{\mathbf{-}}{\mathbf{log}}{\mathbf{}}\left[{\mathbf{H}}^{\mathbf{+}}\right]}$

Take note that: **[H ^{+}] = [H_{3}O^{+}]**

• **pOH**

▪ pOH stands for the negative logarithmic function of hydroxide concentration**▪** can be calculated using the following equation:

$\overline{){\mathbf{pOH}}{\mathbf{=}}{\mathbf{-}}{\mathbf{log}}{\mathbf{}}\left[{\mathbf{OH}}^{\mathbf{-}}\right]}$

Strong Acid-Base Calculations

Strong Acid-Base Calculations

Strong Acid-Base Calculations

Strong Acid-Base Calculations

Strong Acid-Base Calculations