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:

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

Determine the pH of each of the following solutions.

2.05×10^{−2} M KOH

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.

What professor is this problem relevant for?

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