Titration Examples in Chemistry

Start with the recap, study the fully worked examples, then use the practice problems to check your understanding of Titration.

This page combines explanation, solved examples, and follow-up practice so you can move from recognition to confident problem-solving in Chemistry.

Concept Recap

A lab technique for finding an unknown solution concentration by gradually adding a solution of known concentration until the reaction is complete.

Slowly adding a known solution to an unknown one until the reaction is just complete — the volume used reveals the concentration.

Read the full concept explanation →

How to Use These Examples

Read the first worked example with the solution open so the structure is clear.
Try the practice problems before revealing each solution.
Use the related concepts and background knowledge badges if you feel stuck.

What to Focus On

Core idea: Titration starts by identifying solute, solvent, amount, volume, and the concentration unit.

Common stuck point: Students often know a formula related to titration but skip the recognition step: Am I tracking solute, solvent, total solution, concentration, dissolving, or dilution rather than just naming a mixture? That leads to a correct-looking substitution attached to the wrong chemical model.

Sense of Study hint: Ask: Am I tracking solute, solvent, total solution, concentration, dissolving, or dilution rather than just naming a mixture?

Common Mistakes to Watch For

Before you work through the examples, skim the mistake guide so you know which shortcuts and sign errors to avoid.

pH Mistakes

Worked Examples

Example 1

medium

Worked example: pick the better indicator for a weak acid - strong base titration: methyl orange (pH 3-5) or phenolphthalein (pH 8-10)?

Answer

\text{Phenolphthalein}

First step

Weak acid + strong base equivalence pH > 7.

See the full worked solution + why-it-works coaching

SetupKey insightWhy it worksCommon pitfallConnection

Unlock answer keys One Family plan — every worked solution, all subjects

Example 2

medium

Worked example:

25.0\text{ mL}

0.100\text{ M}

HCl

is titrated with

0.100\text{ M}

NaOH

. How many mL of base have been added at the half-equivalence point?

Example 3

challenge

Worked example: a

1.000\text{ g}

aspirin tablet (

M = 180.2\text{ g/mol}

, monoprotic) requires

24.0\text{ mL}

0.200\text{ M}

NaOH

to reach equivalence. What percent by mass is aspirin?

Practice Problems

Try these problems on your own first, then open the solution to compare your method.

Example 1

medium

30\text{ mL}

0.20\text{ M}

NaOH

neutralizes

25\text{ mL}

HNO_3

(

1:1

). Find the acid concentration.

Example 2

easy

In a

1:1

acid-base titration,

25\text{ mL}

0.10\text{ M}

acid is neutralized by

0.20\text{ M}

base. What volume of base is needed?

Example 3

easy

A titration uses

30\text{ mL}

0.10\text{ M}

NaOH

to neutralize

20\text{ mL}

HCl

. Find the

HCl

concentration (

1:1

Example 4

easy

What does the equivalence point of a titration represent?

Example 5

easy

In titration, is the unknown found by adding a solution of known or unknown concentration?

Example 6

easy

50\text{ mL}

0.20\text{ M}

acid is titrated with

0.50\text{ M}

base (

1:1

). What volume of base reaches equivalence?

Example 7

easy

Why is an indicator used in an acid-base titration?

Example 8

easy

At the equivalence point of a strong acid-strong base titration, what is the approximate pH?

Example 9

easy

M_AV_A = M_BV_B

, if both volumes are equal, how do the concentrations compare (

1:1

Example 10

medium

25\text{ mL}

H_2SO_4

is neutralized by

50\text{ mL}

0.10\text{ M}

NaOH

. Find the acid concentration. (

H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O

)

Example 11

medium

How many moles of

HCl

are in

40\text{ mL}

0.25\text{ M}

HCl

Example 12

medium

20\text{ mL}

0.15\text{ M}

Ba(OH)_2

is titrated with

HCl

. What volume of

0.30\text{ M}

HCl

reaches equivalence? (

Ba(OH)_2 + 2HCl \rightarrow BaCl_2 + 2H_2O

)

Example 13

medium

0.500\text{ g}

sample of

KHP

(

M=204\text{ g/mol}

) is titrated with

NaOH

. How many moles of

NaOH

are needed (

1:1

Example 14

medium

10\text{ mL}

0.40\text{ M}

HCl

is diluted to

40\text{ mL}

, then titrated with

0.20\text{ M}

NaOH

(

1:1

). What volume of base is needed?

Example 15

medium

In a

1:1

titration,

0.0030\text{ mol}

of base neutralizes an acid in

25\text{ mL}

. What is the acid concentration?

Example 16

medium

15\text{ mL}

0.20\text{ M}

NaOH

neutralizes

30\text{ mL}

of acetic acid (

1:1

). Find the acid concentration.

Example 17

medium

22.0\text{ mL}

NaOH

titrates

25.0\text{ mL}

0.110\text{ M}

HCl

(

1:1

). Find the

NaOH

concentration.

Example 18

challenge

25.0\text{ mL}

H_3PO_4

requires

45.0\text{ mL}

0.100\text{ M}

NaOH

to fully neutralize all three protons. Find the acid concentration. (

H_3PO_4 + 3NaOH \rightarrow Na_3PO_4 + 3H_2O

)

Example 19

challenge

0.612\text{ g}

impure

KHP

(

M=204

) sample needs

28.0\text{ mL}

0.100\text{ M}

NaOH

(

1:1

). What is the percent purity of

KHP

Example 20

challenge

20.0\text{ mL}

0.150\text{ M}

H_2SO_4

is titrated with

0.200\text{ M}

KOH

. What volume of

KOH

reaches the second equivalence point? (

H_2SO_4 + 2KOH \rightarrow K_2SO_4 + 2H_2O

)

Example 21

easy

20\text{ mL}

0.10\text{ M}

acid is titrated with

0.10\text{ M}

base (

1:1

). What volume of base reaches equivalence?

Example 22

easy

40\text{ mL}

0.10\text{ M}

HCl

needs how many mL of

0.20\text{ M}

NaOH

(

1:1

Example 23

easy

At the equivalence point of a strong acid - weak base titration, is the pH less than, equal to, or greater than 7?

Example 24

easy

At the equivalence point of a weak acid - strong base titration, is the pH less than, equal to, or greater than 7?

Example 25

easy

10\text{ mL}

0.50\text{ M}

NaOH

neutralizes

25\text{ mL}

HCl

(

1:1

). Find the

HCl

concentration.

Example 26

medium

15.0\text{ mL}

H_2SO_4

requires

40.0\text{ mL}

0.150\text{ M}

NaOH

to fully neutralize. Find the acid concentration.

Example 27

medium

25.0\text{ mL}

HCl

sample requires

18.5\text{ mL}

0.100\text{ M}

NaOH

at equivalence (

1:1

). Find

[HCl]

Example 28

medium

What volume of

0.200\text{ M}

HCl

is needed to neutralize

30.0\text{ mL}

0.100\text{ M}

Ba(OH)_2

? (

Ba(OH)_2 + 2HCl \rightarrow BaCl_2 + 2H_2O

)

Example 29

medium

32.0\text{ mL}

0.250\text{ M}

H_2SO_4

requires

V

mL of

0.400\text{ M}

KOH

at equivalence (

1:2

). Find

V

Example 30

medium

0.250\text{ g}

sample of

KHP

(

M = 204\text{ g/mol}

) is titrated with

NaOH

, requiring

22.0\text{ mL}

(

1:1

). Find

[NaOH]

Example 31

medium

50.0\text{ mL}

0.0500\text{ M}

H_2SO_4

needs how many mL of

0.100\text{ M}

NaOH

at equivalence (

1:2

Example 32

medium

28.5\text{ mL}

0.120\text{ M}

NaOH

neutralizes

25.0\text{ mL}

of acetic acid (

1:1

). Find

[CH_3COOH]

Example 33

medium

How many moles of acid are in

35.0\text{ mL}

0.300\text{ M}

H_2SO_4

, and how many moles of

H^+

are available?

Example 34

medium

20.0\text{ mL}

0.150\text{ M}

acid is diluted to

100\text{ mL}

, then titrated with

0.0500\text{ M}

NaOH

(

1:1

). What volume of base is needed?

Example 35

hard

A 0.450 g sample of impure

KHP

(

M = 204

) requires

20.5\text{ mL}

0.100\text{ M}

NaOH

(

1:1

). Find the percent purity.

Example 36

hard

25.0\text{ mL}

H_3PO_4

requires

36.0\text{ mL}

0.250\text{ M}

NaOH

to fully neutralize all three protons (

1:3

). Find

[H_3PO_4]

Example 37

hard

30.0\text{ mL}

0.120\text{ M}

H_2SO_4

is titrated with

0.150\text{ M}

NaOH

. What volume of

NaOH

is needed to reach equivalence? (

H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O

)

Example 38

hard

15.0\text{ mL}

0.250\text{ M}

Ba(OH)_2

is titrated with

0.200\text{ M}

HNO_3

. What volume of

HNO_3

reaches equivalence? (

Ba(OH)_2 + 2HNO_3 \rightarrow Ba(NO_3)_2 + 2H_2O

)

Example 39

hard

In a titration,

25.0\text{ mL}

of a

0.100\text{ M}

weak acid

HA

(

pK_a = 4.74

) is half-neutralized by

0.100\text{ M}

NaOH

. What is the pH?

Example 40

hard

30.0\text{ mL}

0.150\text{ M}

HCl

is mixed with

20.0\text{ mL}

0.200\text{ M}

NaOH

. Find the pH of the resulting solution.

Example 41

challenge

20.0\text{ mL}

0.100\text{ M}

H_2SO_4

is titrated with

0.200\text{ M}

KOH

. What volume of

KOH

reaches the second equivalence point? (

H_2SO_4 + 2KOH \rightarrow K_2SO_4 + 2H_2O

)

← Back to Titration Formula Explained Common Mistakes Practice Mode

Related Concepts

Concentration Neutralization Mole pH

Background Knowledge

These ideas may be useful before you work through the harder examples.

concentrationneutralizationmole