Calculate pH of Strong Bases | NaOH, KOH

Calculate pH of Strong Bases | NaOH, KOH

Strong bases dissociate completely to hydroxyl ions and related cations in the water. Strong bases show higher pH values than weak bases (such as aqueous ammonia solution). Sodium hydroxide (NaOH), potassium hydroxide (KOH), barium hydroxide are famous strong bases. From those two strong bases, NaOH and KOH has lot of uses in laboratories and chemical industries.

In this tutorial, we will learn following sections of chemistry of bases (alkali)

  1. Calculate pOH valie and pH value when concentration of base is known
  2. Calculate concentration of strong base when pH or pOH values are given.

What are the strong bases or strong alkalis?

Strong bases dissociate completely in water. Some of strong bases are NaOH, KOH, Ba(OH)2. In water, these bases dissociate into metal cation and OH- ion. As an example, NaOH dissociates completely to Na+ ion and OH- ion.

General equation of strong acid dissociation

MOH(aq) → M+(aq) + OH-(aq)

NaOH(aq) → Na+(aq) + OH-(aq)

KOH(aq) → K+(aq) + OH-(aq)

Strong Bases

Following metal hydroxides dissolve very well in water and give strong alkaline solution.

Calculate pH of NaOH solution

pH is mainly changed due to change of concentration of the solution. The concentration of the base increases, it results increase of pH.

pH and pOH

pH is defined for expressing H3O+ concentration and pOH is defined for expressing OH- concentration.

In calculating pH of NaOH solution, first, we have to calculate the pOH value. We have a relationship between pH and pOH as below.

pH + pOH = pKa

pKa is a constant to a certain temperature and pKa = 14 at 250C. So at 250C,

pH + pOH = 14

We can use two methods to calculate pH of basic solution.

  1. Calculate pOH of the base and then pH
  2. Calculate [H3O]+(aq), then calculate the pH

How about the pH of aqueous ammonium hydroxide and sodium hydroxide?

Ammonium hydroxide is a weak base give less hydroxyl ion concentration. But sodium hydroxide is a strong acid and completely dissociate to sodium ion and hydroxyl ions.

When hydroxyl ion concentration is high, its basic strength is higher and has a high pH value.

Method 1

Calculate pOH of strong base and pH

The formula of pOH,

pOH = -log10[OH-(aq)]

calculating pOH is a logarithmic one.

Then use the expression of

pH + pOH = pKw

to calculate pH. The sum of pH + pOH become 14 when room temperature is 250C. In other temperatures, we have to give the related value of that temperature.

Method 2

Calculate [H3O]+(aq) and then pH

There is a relation between [H3O]+(aq) and [OH]-(aq) in aqueous solution.

Relationship of [H3O]+(aq) and [OH]-(aq)

[H3O]+(aq) * [OH]-(aq) = Kw

Kw = constant

At 250Kw,
Kw = 1.0 * 10-14mol2 dm-6

When we know [OH]-(aq), using this equation, we can easily calculate the [H3O]+(aq).

Then, we can use pH equation, to calculate pH.

pH = -log10[H3O+(aq)]


pKw = -log10[Ka]

Calculate pH of strong bases | NaOH, KOH

Example 1

Calculate pH of 0.1 moldm-3 NaOH solution

The room temperature is 250C.
Note : M = mol dm-3

We solve this example according to method 1.

NaOH dissociate completely into Na+(aq) & OH-(aq) ions in water.

NaOH dissiciation in water

We have to calculate concentration of OH-(aq) to calculate pH.

strong alkaline dissociation table

First we calculate pOH and then calculate the pH using the relationship of pH and pOH

Calculate pOH

pOH = -log(OH-(aq))
pOH = -log ( 0.1)
pOH = 1

relation of pH and pOH

pH + pOH = 14 (at 250C)
pH + 1 = 14
pH = 13

Let's solve example 1 according to method 2.

We know the concentration of OH- ions

[OH-(aq)] = 0.1 moldm-3

Use the relation of,

[H3O]+(aq) * [OH]-(aq) = Kw

at 250C, Kw = 1.0 * 10-14mol2 dm-6

[H3O]+(aq) * 0.1 = 1.0 * 10-14

[H3O]+(aq) = 1.0 * 10-13

Now, we know the concentration of [H3O]+(aq), therefore we can use pH equation,

pH = -log10[H3O+(aq)]

pH = -log10(1.0 * 10-13)

pH = 13

Example 2

Calculate concentration of KOH when pH 10 at 250C

Here, we are given the pH value. We have to calculate the concentration of KOH. If we know the pH value, we can calculate pOH from pH + pOH = 14 at 250C.

So pOH = 4

From pOH equation, we can calculate OH- concentration.

  • pOH = -log10[OH-(aq)]
  • 4 = -log10[OH-(aq)]
  • [OH-(aq)] = 0.0001 mo dm-3

Example 3

Calculate pH of 0.01 moldm-3 NaOH solution

Here only changes the concentration of NaOH. We studied, NaOH completely dissociate in the water. Therefore,
[OH]-(aq) = 0.01 moldm-3

Then substitute [OH]-(aq) to the pOH equation.

pOH = -log(OH-(aq))
pOH = -log ( 0.01)
pOH = 2

relation of pH and pOH

pH + pOH = 14 (at 250C)
pH + 2 = 14
pH = 12

pH variation against concentration of base

When OH- concentration of aqueous solution is reduced by 10 times, pH is decreased by a 1.

At 250C, pH + pOH = 14

pH variation against concentration of base

Example 3

Calculate pH of 0.1 moldm-3 of Ba(OH)2

Ba(OH)2 is a strong base. Therefore it dissociate completely in water to Ba2+(aq) and OH- ions.

barium hydroxide dissociation

Dissociation of Ba(OH)2

When one Ba(OH)2 molecule dissociate, one Ba2+ ion and two OH- ions are given. See the stoichiometry ratio.

Dissociation of Ba(OH)2

[OH-(aq)] = 0.2 moldm-3

Then substitute [OH]-(aq) to the pOH equation.

pOH = -log(OH-(aq))

pOH = -log ( 0.2)

pOH = 0.7

relation of pH and pOH

pH + pOH = 14 (at 250C)

pH + 0.7 = 14

pH = 13.3

Example 4

Calculate concentration and pH of NaOH solution

4g of solid NaOH are dissolved in water and then diluted the mixture upto 250cm3. Calculate the concentration of OH- ions and pH of solution.

NaOH solution diluting

First, number of moles(n) of dissolved NaOH should be calculated.

Molecular weight of NaOH

NaOH = 23 + 16 + 1
NaOH = 40 g mol-1

number of moles of dissolved NaOH, nNaOH

nNaOH = 4 g / 40 gmol-1
nNaOH = 0.1 mol

Calculate the concentration now

[NaOH(aq)] = 0.1mol / 0.25 dm3
[NaOH(aq)] = 0.4 mol dm-3
[OH-(aq)] = 0.4 mol dm-3

pOH = -log(OH-(aq))
pOH = -log ( 0.4)
pOH = 0.4

pH = 13.6


Is 12.0 mol l-1 OH- ion concentration is strong base?

Yes. it is.

If pH of a solution of the strong base NaOH is known, which property of the solution can be calculated?

If pH value is high, we know, pH value will completely depend on the concentration of NaOH. Otherwise we have to consider dissociation of water to calculate OH- concentration.

  • If pH is higher (above 9), we can directly calculate OH- concentration from pOH = -log10[(OH-)].
  • To find the pOH, use the relationship of pH + pOH = pKa.
  • Also you can calculate concentration of [H3O+] from pH value.

Is pH value of different NaOH and KOH solutions equal or not when their concentrations are equal.?

Both NaOH and KOH are strong bases and dissociate completely in the water. So when NaOH and KOH concentrations are equal, after the dissociation, hydroxyl ion concentration is also same. Therefore pH of both solution is equal.

But, basic strength of KOH is much higher than NaOH.

NaOH ph level

pH of dilute NaOH solutions are usually above 10 if concnetration of NaOH is higher than 0.0001 mol dm-3

How much pH of 0.1 mol dm-3 KOH

pOH is 1 and pH = 13

0.01 moldm-3 naoh ph

pOH of 0.01 mol dm-3 NaOH = 2

pH of 0.01 mol dm-3 NaOH = 12


calculate the ph of a 0.02 mol dm-3 sodium hydroxide solution in water at 250C given that it contains a 0.02 mol dm-3 of hydroxide ions

When sodium hydroxide solution is dissolved in water it dissociates completely to sodium ion and hydroxyl ions. According to the balanced equation, concentraion of hydroxyl ions is equal to the concentration of sodium hydroxide.

Therefore, pH of 0.02 mol dm-3 sodium hydroxide is 1.69

If OH- has a concentration of 0.00092832 at 250C, what is pH?

OH- concentration = 0.00092832 mol dm-3. Substitute this in pOH equation. Then you can use pH + pOH = 14 eqution. At 250C, pH + pOH = 14

which is stronger base KOH or Ni(OH)2?

Nickel hydroxide (Ni(OH)2) is a green color precipitate and give very less OH- amount to water. Therefore, Ni(OH)2 is a weak basic solution. But, KOH is highly soluble in water and dissociates completely in water to give a strong basic solution.

what is the concentration of Mg(OH)2 in a solution with a ph of 8.3?

Magnesium hydroxide is a white color precipitate and give very less OH- amount to water. Therefore, OH- concentration is low and show pH values are not higher as NaOH, KOH solutions. According to the given pH, we can calculate what is the concentration of Mg(OH)2.

  • pOH + pH = 14
  • pOH + 8.3 = 14
  • pOH = 5.7

  • pOH = -log(OH-(aq))
  • 5.7 = -log(OH-(aq))
  • OH-(aq) = 2 * 10-6 mol dm-3

Assuming all OH- ions exist in water are given by Mg(OH)2 (not from water ionization)

Because, we know the OH- concentration, we can calculate concentration of Mg(OH)2.

  • concentration of Mg(OH)2 = 2 * 10-6 mol dm-3 / 2
  • concentration of Mg(OH)2 = 1 * 10-6 mol dm-3 / 2

pH of 0.32 M Mg(OH)2

Magnesium hydroxide (Mg(OH)2) is not asoluble hydroxide in water. It forms a weak basic solution. First, you should know that, is it possible to have a concentration like 0.32 M of 0.32 M Mg(OH)2. You can calculate that from using solubility data of inorganic compounds.

Is KOH a strong base

Yes. KOH is a strong base and it completely dissociates to K+ and OH- ions in the water.

calculate the ph of naoh

Just like KOH, substitute hydroxyl ion concentration given by NaOH to the pOH equation. Then substitute pOH value to the pH + pOH = 14 equation and find pH of NaOH.

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