A neutralization reaction is when an acid and also a base reaction to type water and a salt and involves the combination of H+ ions and also OH- ions to generate water. The neutralization the a strong acid and strong base has a pH equal to 7. The neutralization that a solid acid and also weak base will have actually a pH of less than 7, and also conversely, the result pH once a strong base neutralizes a weak acid will certainly be better than 7.

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When a equipment is neutralized, it means that salt are developed from same weights of acid and also base. The amount of acid required is the amount the would give one mole of proton (H+) and also the amount of base needed is the amount the would give one mole of (OH-). Since salts are formed from neutralization reactions with tantamount concentrations of weights that acids and bases: N components of mountain will always neutralize N parts the base.

Table (PageIndex1): The most common strong acids and bases. Most whatever else not in this table is taken into consideration to it is in weak. Strong AcidsStrong Bases

Strong Acid-Strong base Neutralization

Consider the reaction between (ceHCl) and also (ceNaOH) in water:

This deserve to be composed in terms of the ions (and canceled accordingly)

When the spectator ions room removed, the net ionic equation shows the (H^+) and (OH^-) ions developing water in a strong acid, solid base reaction:

(H^+_(aq) + OH^-_(aq) leftrightharpoons H_2O_(l) )

When a strong acid and a solid base fully neutralize, the pH is neutral. Neutral pH way that the pH is same to 7.00 in ~ 25 ºC. In ~ this allude of neutralization, there are equal amounts of (OH^-) and also (H_3O^+). Over there is no overfill (NaOH). The equipment is (NaCl) at the equivalence point. As soon as a strong acid fully neutralizes a solid base, the pH of the salt systems will always be 7.

Weak Acid-Weak base Neutralization

A weak acid, weak basic reaction can be shown by the net ionic equation example:

(H^+ _(aq) + NH_3(aq) leftrightharpoons NH^+_4 (aq) )

The equivalence suggest of a neutralization reaction is once both the acid and also the base in the reaction have been completely consumed and also neither the them room in excess. Once a strong acid neutralizes a weak base, the resulting solution"s pH will be less than 7. When a solid base neutralizes a weak acid, the result solution"s pH will be better than 7.

Table 1: pH levels at the Equivalence point Strength that Acid and BasepH Level
Strong Acid-Strong Base 7
Strong Acid-Weak Base 7
Weak Acid-Weak Base pH K_b) pH =7 if (K_a = K_b) pH >7 if (K_a


One the the many common and also widely used ways to complete a neutralization reaction is v titration. In a titration, an acid or a basic is in a flask or a beaker. Us will display two examples of a titration. The an initial will be the titration that an mountain by a base. The second will be the titration of a base by an acid.

Example (PageIndex1): Titrating a Weak Acid

Suppose 13.00 mL the a weak acid, v a molarity that 0.1 M, is titrated with 0.1 M NaOH. Just how would we attract this titration curve?


Step 1: First, we need to uncover out where our titration curve begins. To carry out this, we find the early stage pH that the weak acid in the beaker before any NaOH is added. This is the allude where ours titration curve will start. To uncover the initial pH, we very first need the concentration that H3O+.

Set up an ice table to uncover the concentration of H3O+:

(HX) (H_2O) (H_3O^+) (X^-)
Initial 0.1M
Change -xM +xM +xM
Equilibrium (0.1-x)M +xM +xM


Solve for pH:


Step 2: To accurately attract our titration curve, we have to calculate a data allude between the beginning point and the equivalence point. To execute this, we settle for the pH once neutralization is 50% complete.

Solve for the mole of OH- that is added to the beaker. We have the right to to execute by first finding the volume that OH- included to the acid at half-neutralization. 50% the 13 mL= 6.5mL

Use the volume and also molarity to solve for mole (6.5 mL)(0.1M)= 0.65 mmol OH-

Now, deal with for the mole of mountain to be neutralized (10 mL)(0.1M)= 1 mmol HX

Set increase an ice table to determine the equilibrium concentration of HX and also X:

(HX) (H_2O) (H_3O^+) (X^-)
Initial 1 mmol
Added Base 0.65 mmol
Change -0.65 mmol -0.65 mmol -0.65 mmol
Equilibrium 0.65 mmol 0.65 mmol

To calculation the pH at 50% neutralization, usage the Henderson-Hasselbalch approximation.


pH=pKa+ log<0.65mmol/0.65mmol>


Therefore, when the weak mountain is 50% neutralized, pH=pKa

Step 3: Solve because that the pH in ~ the equivalence point.

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The concentration the the weak mountain is half of its initial concentration as soon as neutralization is finish 0.1M/2=.05M HX

Set up an ice table to recognize the concentration that OH-:

Initial 0.05 M
Change -x M +x M +x M
Equilibrium 0.05-x M +x M +x M


Since Kw=(Ka)(Kb), we can substitute Kw/Ka in place of Kb to obtain Kw/Ka=(x^2)/(.05)


Step 4: Solve because that the pH after ~ a bit an ext NaOH is included past the equivalence point. This will provide us precise idea of whereby the pH levels off at the endpoint. The equivalence suggest is as soon as 13 mL that NaOH is added to the weak acid. Let"s find the pH ~ 14 mL is added.

Solve because that the mole of OH-

< (14 mL)(0.1M)=1.4; mmol OH^->

Solve because that the moles of acid

<(10; mL)(0.1;M)= 1;mmol ;HX>

collection up an ice cream table to recognize the (OH^-) concentration:

(HX) (H_2O) (H_3O^+) (X^-)
Initial 1 mmol
Added Base 1.4 mmol
Change -1 mmol -1 mmol 1 mmol
Equilibrium 0 mmol 0.4 mmol 1 mmol