The Ionic Product of Water, pH, pOH & pH Scale Explained 🔬 | Unlock the Secrets of Chemistry for MDCAT & ECAT Success 💥

👋 Welcome to Inamjazbi’s Chemistry Corner! 🌟
Are you ready to unlock the secrets of the pH scale, pOH, and the ionic product of water? Dive into today’s post, where we break down essential concepts that will help you ace your MDCAT and ECAT chemistry exams. Whether you're preparing for exams or just passionate about chemistry, this guide is for you! 🔬✨

Let’s dive in and make chemistry easy and fun! 🎯

#Inamjazbi #LearnChemistry #pH #pOH #IonicProductOfWater #ChemistryForMDCAT #ChemistryForECAT #StudyWithInamjazbi #ScienceMadeEasy #MDCAT #ECAT #ChemistryExamPreparation #AcidBaseChemistry #ChemicalEquilibrium #ChemistryBlog

🌟 The Ionic Product of Water, pH, pOH & pH Scale Explained 🔬 | Unlock the Secrets of Chemistry for MDCAT & ECAT Success 💥

🧪📚 Ionic Product of Water (Basis of pH Scale)

In the study of acid-base reactions in aqueous solution, the important quantity is the [H⁺] or H⁺ ions concentration. [In aqueous solution, the H⁺ ion concentration can range from 10¹ M to 10⁻¹⁵ M (10⁻¹⁴ M in most books). A Danish biochemist Soren Sorensen in 1909 proposed a logarithmic acidity scale called pH scale to compress this enormous range on the basic of auto-ionization or self-dissociation of water].

Pure water is a very weak electrolyte as it is ionized to a very small extent and only partially ionizes into H⁺ and OH⁻ ions. [It is about 2 × 10⁻⁷ % dissociated into its ions at 25°C i.e. 1 in every 2 × 10⁶ (2 million) molecules of water are split up into ions at 298 K]. The auto-ionization equilibrium of water is characterized by an equilibrium constant (Kc) at a given temperature. Since a very small fraction of water molecules are ionized, the concentration of unionized water molecules is in large excess and is virtually constant. Thus expressing the protons as H⁺ rather than H₃O⁺, we can write the Kc for auto-ionization for water as:

Since the concentration of water is in large excess, it remains constant. The equilibrium constant expression for the reaction is:

The equation constant (Kw) is called Ionic Product of water or Ionic-Product constant or Dissociation constant of water which is “The product of molar concentration of hydrogen ion; [H⁺] and hydroxide ion [OH⁻] at a particular temperature( at 25°C) and it is equal to 1 × 10⁻¹⁴ mol²/dm⁶”. This constant determines absolutely the relative [H⁺] and [OH⁻] ions in water at this temperature. [This figure means that approximately 1 in every 5 × 10⁸ molecules at water is split up into ions at 298 K. There are approximately 6 x 10⁶ H⁺ ions in every dm³ of water].

Putting this value in the above equation, we get:

In pure water at 25°C, concentration of H⁺ and OH⁻ ions would always be equal and found to be 1 × 10⁻⁷ mol/dm³ (M). [That is why water is neutral at 25°C].

[H+] = 1 × 10⁻⁷ and [OH⁻] = 1 × 10⁻⁷

Kw = [H⁺] [OH⁻] ⇒ (1 × 10⁻⁷ ) × (1 × 10⁻⁷ ) ⇒ 1 × 10⁻¹⁴ mol²/dm⁶ (M²)

Thus pH of neutral solution can be calculated as:

pH = – log [H⁺] ⇒ pH – log [10⁻⁷] ⇒ pH = – (–7) log 10 ⇒ pH = 7 × 1 (∵ log 10 = 1) ⇒ pH = 7

Thus the pH of a neutral solution is always 7. Acidic solutions have pH values less than 7 whereas basic solutions have pH values greater than 7. If the solution is acidic, then [H⁺] > [OH⁻] and if the solution is basic then [H⁺] < [OH⁻] but the ionic product Kw remains constant at 1 x 10⁻¹⁴ M² at 298K. For neutral solution [H⁺] = [OH⁻] = 1 × 10⁻⁷M.

In pure water; [H⁺] = [OH⁻] = 10⁻⁷ mol/dm³

So,

pH = –log[H⁺] ⇒ –log(10⁻⁷) ⇒ – (–7) log10 ⇒ 7 x 1 pH = 7

Similarly,

pOH = –log[OH⁻] ⇒ –log(10⁻⁷) ⇒ – (–7) log10 ⇒ 7 x 1 pOH = 7

Thus, the sum of pH and pOH of solution is 14. i.e. pH + pOH = 14.

🔥Proof Relation; pH + pOH = 14

The fact can be proved mathematically as

Kw = [H⁺] [OH⁻] = 1 x 10⁻¹⁴

Taking log on both sides

log[H⁺] log [OH⁻] = Log 1 x 10⁻¹⁴

log[H⁺] + log [OH⁻] =–14 Log 10

Multiplying both sides by (–)

–log[H⁺] + {–log [OH⁻] } = – (–14)

–log[H⁺] + {–log [OH⁻] } = 14

But

–log[H⁺] = pH

–log [OH⁻] = pOH

pH + pOH = 14

🧪📚 pH and pH Scale

🔥Definition of pH

In aqueous solutions, the concentration of H⁺ ions can range from 10¹ to10⁻¹⁵ M (10⁻¹⁴ M in most books). It is convenient to compress this complex enormous range by introducing a logarithmic acidity scale called pH (means power of hydrogen) proposed by the Danish Chemist S.P.L. Sorensen in 1909. Thus pH is a convenient method of expressing acidity or basicity of solutions. pH is a measure of the strength of an acid or a base. In 1909, S.P.L. Sorensen proposed a pH scale in order to better express the concentration of of H⁺ ion aqueous solution.

pH is an abbreviation for power of H⁺ ion concentration. pH of a solution is defined as the negative logarithm of the molar hydrogen ions concentration [H⁺] (in mol/litre) of a solution. [In other words pH is the logarithm of the reciprocal of molar hydrogen ion concentration [H⁺] of a solution]. pH values range from 0-14.

pH = log 1/[H⁺] or pH = log 1 – log [H⁺] ⇒pH = 0 – log [H⁺] ⇒ pH = – log [H⁺]

For Example

(i) a concentration of 1 × 10⁻⁷ M of H⁺ ions of solution becomes a pH of 7 (showing a neutral solution because the concentration of OH⁻ ions would also equal to 1 × 10⁻⁷ M).

(ii) Similarly, concentration of 1 × 10⁻⁷ M of H⁺ ions giving a pH of 3 (showing an acidic solution).

🔥Definition of pOH

The basic character of solution is expressed by pOH, which is the negative logarithm to the base 10 of molar hydroxide ions concentration [OH⁻] of a solution. i.e. pOH = -log [OH⁻]

pH + pOH = 14

The sum of pH and pOH of a solution at 25°C is 14. i.e. pH + pOH = 14.

🔥Range of H⁺ ion concentration and Range of pH

H⁺ ion concentration can range from 10 M to less than 10⁻¹⁵ M. However, the most commonly encountered H⁺ ion concentrations are less than 10⁰ M (1 M) to 10⁻¹⁴M, so the pH function is defined with a negative sign in order to produce a number that is positive in most cases, which otherwise would be negative due to small value of [H⁺]. Since H+ ion concentration of a solution ranges between 100 to 10⁻¹⁴, so value of pH ranges between 0 to 14. (However a strongly acidic solution theoretically have a pH less than zero. e.g. a 10 M HCl solution has a theoretical pH = -1. Similarly, a strongly alkaline solution may have a pH value greater than 14).

🔥Unit of pH

The pH value of a solution is a dimensionless quantity as we cannot take the logarithm of units.

🔥Nature of pH

pH is an intensive quantity.

🔥Relationship between pH and [H⁺]

pH increases as [H⁺] decreases i.e. a high pH means a low concentration of H⁺ ions and vice-versa.

🔥pH–scale

The concentration of hydrogen ions in an aqueous solution can be expressed in terms of pH scale. pH-scale is a logarithmic acidity scale that is simply a number ranges 0-14 by means of which acidity or basicity i.e. pH of a solution is indicated.

🔥pH of Acids and Bases

An acid solution contains H⁺ ions concentration more than 10⁻⁷ M (i.e. 10⁻⁶, 10⁻⁵..... 10⁰) while a basic solution contains H⁺ ions concentration less than 10⁻⁷ M (i.e. 10⁻⁸, 10⁻⁹ ..... 10⁻¹⁰). A neutral solution has H⁺ ions concentration exactly 10⁻⁷ M. The pH of acidic solution is less than 7, pH of basic solution is more than 7, whereas for neutral solution the value of pH is 7.

1. Neutral solutions have pH = 7 (having [H⁺] = 10⁻⁷ M).

2. Acidic solutions always have pH values less than 7. A low pH values lesser than 7 (having [H⁺] greater than 10⁻⁷ M) indicates an acid solution.

3. Basic solutions always have a pH greater than 7. A high pH values greater than 7 (having [H⁺] lesser than 10⁻⁷ M) indicates a basic solution.

⚡Acidic solution ; [H⁺] > 1.0 × 10⁻⁷ M; [OH⁻] < 1.0 × 10⁻⁷ M; pH < 7.00

⚡Basic solution ; [H⁺] < 1.0 × 10⁻⁷ M; [OH⁻] > 1.0 × 10⁻⁷ M; pH > 7.00

⚡Neutral solution ; [H⁺] = 1.0 × 10⁻⁷ M; [OH⁻] = 1.0 × 10⁻⁷ M; pH = 7.00

🔥Applications and significance

1. The pH is a convenient method of expressing acidity or basicity (alkanity) of solution. pH denotes the logarithmic H⁺ ion concentration and its value decides the acidic or basic character of a solution.

2. pH is a measure of the strength of an acid or a base.

3. The pH information and pH control is necessary for water treatment, swimming pool managements, soil conditioning, food processing, corrosion control, electroplating and food preservation.

4. The concept of pH plays an essential role in the field of biology. The pH values of various body fluids is an important guide for a doctor in diagnosing and treating many diseases. The maintenance of pH of human blood is necessary for life. The pH of human blood is normally maintained by the body between 7.35 and 7.45. If the blood pH drops to 7 (as in some illness), the patient may go into coma and may slip into death. If the pH rises more than 7.7-7.8, then a patient suffers from diabetes, vomiting and diarrhea.

🌍 pH Values of Common Substances 🍎🍋

⚡pH of Various Biological Fluids 🧬

Gastric Juice/ Stomach 🍽️: 1.2 - 2.0 (Strongly acidic)

Lemon Juice 🍋: 2.3 (Acidic)

Vinegar 🍶: 2.8 - 3.0 (Acidic)

Grape Juice/Wine 🍇🍷: 3.2 (Acidic)

Grapefruit 🍊: 3.1 (Acidic)

Apples 🍎: 2.9 - 3.3 or 3.1 (Acidic)

Orange Juice 🍊: 3.5 (Acidic)

Cherries 🍒: 3.6 (Acidic)

Tomato Juice 🍅: 4.0 - 4.2 (Slightly acidic)

Banana 🍌: 4.6 - 4.8 (Slightly acidic)

Human Urine 🚻: 5.0 - 7.0 (Slightly acidic to neutral)

Black Coffee ☕: 5.0 (Slightly acidic)

Water Exposed to Air 🌬️: 5.5 (Slightly acidic)

Wheat Flour 🌾: 5.5 - 6.5 (Slightly acidic)

Rain 🌧️: 5.8 - 6.0 (Slightly acidic)

Butter 🧈: 6.1 - 6.4 (Slightly acidic)

Dates 🌴: 6.2 - 6.4 (Slightly acidic)

Cow Milk 🐄🥛: 6.5 (Slightly acidic)

Saliva 💦: 6.4 - 6.9 (Neutral to slightly acidic)

Human Blood 🩸: 7.35 - 7.45 (Neutral)

Egg White 🍳: 7.8 (Slightly alkaline)

⚡pH of Various Inorganic Fluids 🌡️

1M HCl Solution 🧪: 1.0 (Strongly acidic)

0.1M HCl Solution 🧪: 1.1 (Strongly acidic)

H₂SO₄ (Sulfuric Acid) 🧴: 1.2 (Strongly acidic)

Cola/ Soda drinks 🥤: 3.0 (Acidic)

0.1 M CH₃COOH 🍶: 2.9 (Acidic)

Pure Water 💧: 7.0 (Neutral)

Tears 😢: 7.4 (Neutral)

Sea Water 🌊: 7.9 - 8.4 (Slightly alkaline)

Baking Soda (NaHCO₃) 🥣: 8.3 - 8.5 (Basic)

Borax 🧴: 9.2 (Basic)

Lime Water 🌿: 10.5 (Alkaline)

Milk of Magnesia 🧴: 10.6 (Alkaline)

Household Ammonia 🧴: 11.5 - 12.0 (Alkaline)

Limestone 🏔️: 11.6 (Alkaline)

Household Bleach 🧼: 12.6 (Alkaline)

0.1M NaOH Solution 💧: 13.0 (Strongly alkaline)

1M NaOH Solution 🧴: 14.0 (Strongly alkaline)

Milk 🥛: 6.5 - 7 (Neutral to slightly acidic)

Pure Ammonia (NH₃) 🧴: 11 - 12 (Basic)

Baking Soda (NaHCO₃) 🥣: 8.3 (Basic)

🔥Determination of pH of a solution

pH of a solution can be measured by four methods:

1. By using acid-base indictors

2. By using universal indicator;

3. By using pH-paper

4. By using pH-meter;

pH values is related to the universal indicator colours as follows:

The most widely used method for the approximate determination of pH is with the pH-paper. The pH-paper is made by treating paper strips with several different indictors that is used to estimate pH. pH can be estimated by dipping the pH-paper in a given solution then by matching the colour appearing on the pH-paper with the coloured pH-paper strip that corresponds to a known pH.

🔥 pH and Its Importance in Chemistry 🔬

💥 Acid-Base Reactions ⚖️

The pH helps determine whether a solution will act as an acid or a base during chemical reactions.

💥 Biological Systems 💚

The pH of blood and stomach acid plays a vital role in enzyme activity and digestion.

💥 Agriculture 🌾

pH affects the availability of nutrients to plants. Soil with pH too high or too low can result in poor crop growth.

🔥Applications of pH in Daily Life 🌎

💥 Cleaning 🧼: Many household cleaning products are basic to help remove dirt and grease.

💥 Swimming Pools 🏊‍♂️: The pH of pool water must be between 7.2 and 7.8 to avoid skin irritation.

💥 Food & Drink 🍏: The pH of beverages like soda and coffee determines their acidity.

🔥Significance of pH in Biological Systems 🌱

💥 Human Blood 🩸:

The pH of blood must be around 7.35 - 7.45 to maintain proper metabolic function.

💥 Stomach Acid 🍽️:

The stomach has a very low pH (1.5 - 3.5) due to hydrochloric acid, which helps in digestion and killing harmful microbes.

How pH Affects the Rate of Reactions ⏱️

💥 Acid-Catalyzed Reactions: Acids often speed up reactions by donating protons (H⁺).

💥 Enzyme Activity: Enzymes that help with digestion and metabolism work best at specific pH values.

For example, pepsin, the enzyme that digests proteins in the stomach, works best in acidic conditions.

pH in Water & Environmental Chemistry 🌍💧

💥 The pH of natural water bodies (like rivers, lakes, and oceans) affects aquatic life.

💥 Acid Rain 🌧️: Caused by the dissolution of sulfur dioxide (SO₂) and nitrogen oxides (NOₓ) in water, forming acidic solutions (pH < 5.6), which can harm ecosystems.

💥 Ocean Acidification 🌊: Increased CO₂ levels lower the pH of oceans, affecting marine life, particularly corals and shellfish.

💥 MCQ Quiz on pH for MDCAT & ECAT 🧠

1. Which of the following is the pH of lemon juice?

🟦 A. 2.3

🟩 B. 4.5

🟪 C. 7.0

🟨 D. 9.0

2. The pH of human blood is normally:

🟦 A. 6.8

🟩 B. 7.0

🟪 C. 7.35 - 7.45

🟨 D. 8.0

3. A solution with a pH of 12 is:

🟦 A. Neutral 💧

🟩 B. Acidic 🍋

🟪 C. Alkaline 🌱

🟨 D. Weakly acidic 🍓

4. What is the pH of sodium hydroxide (NaOH) solution?

🟦 A. 1.0

🟩 B. 7.0

🟪 C. 10.5

🟨 D. 14.0

5. Which of the following is considered a weak acid?

🟦 A. Hydrochloric acid (HCl)

🟩 B. Sulfuric acid (H₂SO₄)

🟪 C. Acetic acid (CH₃COOH)

🟨 D. Nitric acid (HNO₃)

6. Which of these is a strong base?

🟦 A. Ammonia (NH₃)

🟩 B. Sodium hydroxide (NaOH)

🟪 C. Calcium hydroxide (Ca(OH)₂)

🟨 D. Potassium carbonate (K₂CO₃)

7. What is the pH of a 1 M solution of hydrochloric acid (HCl)?

🟦 A. 0

🟩 B. 1

🟪 C. 2

🟨 D. 7

8. The pH of a solution is a measure of the concentration of which ion?

🟦 A. Hydroxide ion (OH⁻)

🟩 B. Hydrogen ion (H⁺)

🟪 C. Sodium ion (Na⁺)

🟨 D. Chloride ion (Cl⁻)

9. Which of the following has the lowest pH?

🟦 A. Tomato juice 🍅

🟩 B. Vinegar 🍶

🟪 C. Ammonia (NH₃) 🧴

🟨 D. Sea water 🌊

10. Which of the following methods is used to remove temporary hardness in water?

🟦 A. Ion-exchange method

🟩 B. Boiling

🟪 C. Reverse osmosis

🟨 D. Distillation

11. A solution of sodium chloride (NaCl) in water has a pH of:

🟦 A. 2

🟩 B. 5

🟪 C. 7

🟨 D. 12

12. Which substance has the highest pH value?

🟦 A. Hydrochloric acid (HCl)

🟩 B. Ammonium hydroxide (NH₄OH)

🟪 C. Sodium hydroxide (NaOH)

🟨 D. Nitric acid (HNO₃)

13. What is the pH of a neutral solution at 25°C?

🟦 A. 0

🟩 B. 7

🟪 C. 14

🟨 D. 10

14. A substance that increases the concentration of H⁺ ions in solution is known as a:

🟦 A. Base 🌱

🟩 B. Acid 🍋

🟪 C. Salt 🧂

🟨 D. Buffer 🛡️

15. Which of the following is a buffer solution?

🟦 A. A solution of sodium chloride (NaCl)

🟩 B. A solution of sodium acetate (CH₃COONa) and acetic acid (CH₃COOH)

🟪 C. A solution of hydrochloric acid (HCl)

🟨 D. A solution of ammonia (NH₃)

16. A pH of 10 indicates that a solution is:

🟦 A. Acidic 🍋

🟩 B. Neutral 💧

🟪 C. Alkaline 🌱

🟨 D. Very acidic 🍓

17. A solution of pH 4 is:

🟦 A. Strongly acidic 🍋

🟩 B. Slightly acidic 🍏

🟪 C. Neutral 💧

🟨 D. Slightly alkaline 🌱

18. The pH scale is used to measure:

🟦 A. The temperature of a solution

🟩 B. The pressure of a solution

🟪 C. The acidity or alkalinity of a solution

🟨 D. The volume of a solution

19. Which of the following is true about acidic solutions?

🟦 A. pH > 7

🟩 B. pH = 7

🟪 C. pH < 7

🟨 D. pH = 14

20. Which of the following has a pH greater than 7?

🟦 A. Vinegar 🍶

🟩 B. Lemon Juice 🍋

🟪 C. Ammonia (NH₃) 🧴

🟨 D. Hydrochloric acid (HCl)

21. What is the pH of pure water?

🟦 A. 0

🟩 B. 7

🟪 C. 14

🟨 D. 3

22. A solution with a pH of 3 is:

🟦 A. Acidic 🍋

🟩 B. Basic 🧴

🟪 C. Neutral 💧

🟨 D. Alkaline 🌱

23. If the concentration of hydrogen ions [H⁺] is 1 × 10⁻⁶ M, what is the pH of the solution?

🟦 A. 4

🟩 B. 6

🟪 C. 8

🟨 D. 10

24. Which of the following has a pH greater than 7?

🟦 A. Vinegar 🍶

🟩 B. Lemon Juice 🍋

🟪 C. Ammonia (NH₃) 🧴

🟨 D. Orange Juice 🍊

25. What is the relationship between pH and pOH?

🟦 A. pH + pOH = 7

🟩 B. pH + pOH = 14

🟪 C. pH × pOH = 7

🟨 D. pH = pOH

Answer Key 📝

1. Answer: A

Explanation: The pH of lemon juice is typically 2.3, which is acidic 🍋.

2. Answer: C

Explanation: The normal pH of human blood is around 7.35 - 7.45, which is slightly alkaline.

3. Answer: C

Explanation: A solution with a pH of 12 is alkaline 🌱, meaning it is basic.

4. Answer: D

Explanation: The pH of a NaOH solution (a strong base) is 14 (very alkaline).

5. Answer: C

Explanation: Acetic acid (CH₃COOH) is a weak acid commonly found in vinegar.

6. Answer: B

Explanation: Sodium hydroxide (NaOH) is a strong base 🧴 with a high pH.

7. Answer: B

Explanation: A 1M HCl solution has a pH of 1, indicating it's highly acidic.

8. Answer: B

Explanation: The pH scale is a measure of the concentration of hydrogen ions (H⁺).

9. Answer: B

Explanation: Vinegar 🍶 has a pH of 2.8 - 3.0, which is acidic.

10. Answer: B

Explanation: Boiling removes temporary hardness in water by precipitating calcium bicarbonate.

11. Answer: C

Explanation: Sodium chloride (NaCl) in water is neutral with a pH of 7.

12. Answer: C

Explanation: Sodium hydroxide (NaOH) is a strong base 🧴, which has a pH greater than 7.

13. Answer: B

Explanation: Pure water at 25°C has a pH of 7, which is neutral.

14. Answer: B

Explanation: An acid 🍋 increases the concentration of H⁺ ions.

15. Answer: B

Explanation: A buffer solution maintains pH and resists changes, like sodium acetate and acetic acid.

16. Answer: C

Explanation: A pH of 10 indicates an alkaline 🌱 solution.

17. Answer: A

Explanation: A solution with pH 4 is strongly acidic 🍋.

18. Answer: C

Explanation: The pH scale measures the acidity or alkalinity of a solution.

19. Answer: C

Explanation: Acidic solutions have pH < 7.

20. Answer: C

Explanation: Ammonia (NH₃) is alkaline, with a pH greater than 7.

21. Answer: B

Explanation: Pure water has a neutral pH of 7. It is neither acidic nor basic.

22. Answer: A

Explanation: A solution with a pH of 3 is acidic, similar to lemon juice 🍋.

23. Answer: B

Explanation: Using the formula pH=−log⁡[H⁺]

For [H⁺] = 1×10⁻⁶

, we get pH=6

24. Answer: C

Explanation: Ammonia (NH₃) 🧴 is basic, and it has a pH greater than 7.

25. Answer: B

Explanation: The sum of pH and pOH is always 14 at 25°C.

pH + pOH = 14

🌟 Quick Guide to pH for MDCAT & ECAT 📚

What is pH? 🤔

pH measures the acidity or alkalinity of a solution:

pH < 7 = Acidic 🍋

pH = 7 = Neutral 💧 (e.g., Pure water)

pH > 7 = Alkaline 🌱

How is pH Measured? 📊

pH Paper (Litmus Paper) 📜: Red = acidic 🍓, Blue = alkaline 🌊

pH Meter ⚡: Digital device for accurate pH measurement.

pH Scale Range 🔴🟢🔵

Acidic: pH 0 - 6 (e.g., Lemon Juice 🍋: pH 2.3)

Neutral: pH = 7 (e.g., Water 💧)

Alkaline: pH 8 - 14 (e.g., Baking Soda 🥣: pH 8.3)

Why is pH Important? 💡

Chemical Reactions 🔬: pH affects the rate and outcome of reactions.

Biology 🧬: Enzyme activity and bodily functions depend on pH.

Environmental Science 🌍: Water pH affects aquatic life (e.g., acid rain 🌧️).

How to Calculate pH? 🧮

Formula:

pH=−log⁡[H⁺]

For example, [H⁺] = 1 × 10⁻⁴ M → pH = 4.

Common pH Values 🍏🍋🌱

Water 💧: pH = 7 (Neutral)

Lemon Juice 🍋: pH = 2.3 (Strongly acidic)

Vinegar 🍶: pH = 3 (Acidic)

Milk 🥛: pH = 6.5 - 7 (Neutral to slightly acidic)

Ammonia (NH₃) 🧴: pH = 11 - 12 (Alkaline)

Baking Soda 🥣: pH = 8.3 (Alkaline)

pH in Biology 🧬

Blood 🩸: pH = 7.35 - 7.45 (slightly alkaline)

Stomach 🥄: pH = 1.5 - 3.5 (acidic for digestion)

Conclusion 🎯

Understanding pH is essential for MDCAT and ECAT! It affects chemical reactions, biological processes, and even environmental health 🌍. Master pH to boost your exam prep and knowledge of the world around you!

Oxides Uncovered: Types, Properties & Uses – Your Ultimate MDCAT & Chemistry Guide by Inam Jazbi

https://learnchemistrybyinamjazbi.blogspot.com/2025/11/class-12-chemistry-notes-with-mechanism.html

https://learnchemistrybyinamjazbi.blogspot.com/2025/10/numericals-on-gaseous-state.html

https://learnchemistrybyinamjazbi.blogspot.com/2025/07/derivation-of-radius-energy-change-in.html

https://learnchemistrybyinamjazbi.blogspot.com/2025/05/xi-chemistry-new-book-concise-notes-2025.html

https://learnchemistrybyinamjazbi.blogspot.com/2025/03/xi-chemistry-numerical-book-according.html

https://learnchemistrybyinamjazbi.blogspot.com/2025/01/model-test-questions-xi-chemistry-on.html

https://learnchemistrybyinamjazbi.blogspot.com/2024/08/model-test-questions-xi-chemistry-on.html

https://learnchemistrybyinamjazbi.blogspot.com/2024/07/uncertainty-in-measurement.html

https://learnchemistrybyinamjazbi.blogspot.com/2024/05/solution-of-important-numericals-of-xi.html

https://learnchemistrybyinamjazbi.blogspot.com/2024/02/xi-mcqs-on-oxidation-numbers-and.html

Strength of Acids and Bases | Strong vs Weak Acids and Bases, Ionization, Ka, Kb Explained | Chemistry Notes for XI & MDCAT with Tricks and Tables