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Determination and Calculation of pH of Various Solutions

pH is a measure of the hydrogen ion concentration [ 𝐻 + ] [H + ] in a solution and indicates whether a solution is acidic, basic, or neutral. It is a logarithmic scale ranging from 0 to 14:

pH < 7 → Acidic solution

pH = 7 → Neutral solution

pH > 7 → Basic (alkaline) solution

The pH can be calculated using the formula:

pH = − log ⁡ 10 [ 𝐻 + ] pH=−log 10

[H + ]

Similarly, for basic solutions, pOH can be calculated and related to pH:

pH + pOH = 14 pH+pOH=14

This experiment helps students understand acid-base chemistry and develop skills in measuring pH both experimentally and theoretically.

To determine the pH of given acidic, basic, and neutral solutions.

To calculate pH from hydrogen ion concentration.

To compare experimental pH readings with theoretical values.

To understand the significance of pH in chemical and biological systems.

Apparatus: Beakers, pipettes, test tubes, glass rods, pH meter (or pH paper), measuring cylinders.

Chemicals:

Hydrochloric acid (HCl) of known concentration

Sodium hydroxide (NaOH) of known concentration

Distilled water

Buffer solutions (optional)

Indicators: Litmus paper (red and blue) or universal indicator solutio

Preparation of solutions

Prepare 0.1 N HCl and 0.1 N NaOH solutions.

Take 50 mL of each solution in separate beakers.

Measurement using pH meter

Calibrate the pH meter using standard buffer solutions (pH 4, 7, 10).

Immerse the electrode into the solution and record the pH reading.

Measurement using indicators

Dip litmus paper or universal indicator into the solution.

Observe the color change and match with standard color chart to estimate pH.

Calculation of pH

Use the formula pH = − log ⁡ 10 [ 𝐻 + ] pH=−log 10

[H + ] to calculate theoretical pH for each solution.

For NaOH, calculate pOH first: [ 𝑂 𝐻 − ] = Concentration of NaOH [OH − ]=Concentration of NaOH

Then, pH = 14 − pOH pH=14−pOH

Record results

Prepare a table of observed pH, calculated pH, and compare results.

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