# pH of KOH | Online Calculate pH and pOH of Potassium Hydroxide

Potassium hydroxide, KOH is a strong base and show great pH values in aqueous solution. In this tutorial, we are going to learn how to calculate pH of different concentration KOH aqueous solutions.

At the end of this tutorial, there is an online calculator which can be used to check your answers (pH values) after you finish your problems.

written by: Heshan Nipuna, last update: 03/06/2020

When calculating pH of KOH solutions, following theories and equations are important.

• Theory 1: KOH dissociates completely in the water to K+ and OH- ions.
• Theory 2: Due to complete dissociation, initial concentration of KOH is equal to OH- concentration.
• Equation 1: Relationship of pH + pOH = 14
• Equation 2: pH = -log10[H3O+(aq)]
• Equation 3: pOH = -log10[OH-(aq)]

Question #1

In the laboratory, there is a aqueous potassium hydroxide solution which was prepared by a student. In the label of the bottle, concentration was mentioned as 0.1 mol dm-3. Calculate the theoretical pH value of the KOH solution.

#### Steps to find pH of KOH solution

1. Find OH- concentration
2. Calculate pOH by OH- concentration
3. Calculate pH by pH + pOH = 14

According to the theory 1, OH- concentration is 0.1 mol dm-3

Now, you can use the equation 3 to calculate pOH with known OH- concentration.

pOH = -log10[OH-(aq)]

pOH = -log10[0.1]

pOH = 1

Now, use the equation 3 to find the pH

pH + pOH = 14

pH + 1 = 14

pH = 13

pH of 0.1 mol dm-3 KOH solution is 13.

Question #2

K = 39 , O = 16 , H = 1

## pH Calculator of KOH

In this calculator, we use several methods to calculate pH of KOH solution. You can use one of it according to the data you have.

1. When concentration of KOH in mol dm-3 is known
2. When amount (mol) of KOH and volume of solvent are known.
3. When mass of KOH is known and volume of solvent is known.

In our calculators pH of the neutral solution is 7 according to the 250C.

Method 1

Method 2

### Calculate pH when amount (mol) of KOH is known and volume of solute is known

We assume that after adding KOH, volume of solute is not changed much. So you can enter volume of solution as volume of solute.

Method 3

### Calculate pH when mass of KOH is known and volume of solute is known

We assume that after adding KOH, volume of solute is not changed much. So you can enter volume of solution as volume of solute.

### What is the relationship of concentration and pH value in KOH solutions.

We can take several KOH solutions and measure their pH values. Here are some KOH solutions with their concentration (mol dm-3).

• 0.1 mol dm-3 : pH = 13
• 0.01 mol dm-3 : pH = 12
• 0.001 mol dm-3 : pH = 11

When concentration of KOH decreases, pH also decreases.

Questions

.

### calculate the ph of the 1.0 * 10-2 mol-1 KOH

First step is calculate the pOH of KOH solution. pOH of 1.0 * 10-2 mol-1 is 2. Then, calculate the pH by using relation of pH + pOH = 14. So pH of the 1.0 * 10-2 mol-1 KOH is 12.

#### a solution of koh (strong base) has a pH= 12.64 what is the concentration of koh?

Because you know the pH value, you can find the pOH. pOH = 14 - pH . pOH of KOH solution is 1.36

Now use the pOH equation.

• pOH = -log10[OH-(aq)]
• 1.36 = -log10[OH-(aq)]
• [OH-(aq)] = 0.044 mol dm-3

OH- ion is provided by only KOH. Therefore concentration of KOH = 0.044 mol dm-3

#### Range of ph of koh solutions between 0.1 M - 0.0001 M

If concentration of KOH is 0.1 M, pH value may be 13. If concentation is 0.0001 M, pH value will be 10. Therefore, pH range of KOH solution will be 10-13.

#### Is potassium hydroxide ph is greater than ammonia

At most cases, this can be true because potassium hydroxide is a strong base. Ammonia give very less OH- ions in aqueous state.

#### I prepared a Potassium hydroxide and Barium hydroxide solution. Both have same concentrations. Which solutions will show higher pH value?

Both Potassium hydroxide and Barium hydroxide are strong bases. Though both have same concentration, their OH- concentration is not same.

Barium hydroxide is a strong base and dissociate like below.

Ba(OH)2 → Ba2+ + 2OH-

OH- concentration of Barium hydroxide is greater than OH- concentration of KOH. Therefore pH of Barium hydroxide solution is greater than KOH solution.

#### I have prepared a strong aqueous KOH solution. But, when I check pH, it shows me pH value just over 7.What may be the reasons for this error?

1. pH meter may be not calibrated properly.
2. Used KOH has been contaminated with impurities. So there is not KOH as thought.
3. Used water may be acidic. It results reacting with KOH and reduce amount of KOH.

### If same concentration KOH and Ba(OH)2 solution were prepared, who will show a higher pH?

OH- concentration of Ba(OH)2 solution is greater because when one mol of KOH dissociates, two moles of OH- are given. But, for KOH, one mol of KOH only give one mol of OH-.

### the relationship of potassium and ph

When potassium metal is added to water, a strong basic solution, KOH is formed. Due to this strong basic solution, pOH value will be low and pH value will be high.

### Related lewis structures

P2O5 lewis structure OH- lewis structure Ammonium ion (NH4+) lewis structure H2CO3 lewis structure