Molar mass of sulfuric acid

The molar mass of sulfuric acid (H2SO4) can be calculated by adding the atomic masses of all the atoms in its chemical formula:

• The molar mass of hydrogen (H) is approximately 1.008 grams per mole.
• The molar mass of sulfur (S) is approximately 32.07 grams per mole.
• The molar mass of oxygen (O) is approximately 16.00 grams per mole.

The chemical formula of sulfuric acid (H2SO4) consists of 2 hydrogen atoms, 1 sulfur atom, and 4 oxygen atoms:

• Molar mass of H2SO4 = (2 × molar mass of H) + (1 × molar mass of S) + (4 × molar mass of O)
• Molar mass of H2SO4 = (2 × 1.008 g/mol) + (1 × 32.07 g/mol) + (4 × 16.00 g/mol)

Now, calculate the molar mass:

• Molar mass of H2SO4 = (2.016 g/mol) + (32.07 g/mol) + (64.00 g/mol)
• Molar mass of H2SO4 = 98.086 g/mol

So, the molar mass of sulfuric acid (H2SO4) is approximately 98.086 grams per mole.

Sulfuric acid PH

Sulfuric acid (H2SO4) is a strong mineral acid, and at full concentration its pH value is extremely low, typically around -1. This means that it is highly acidic. The pH scale ranges from 0 (most acidic) to 14 (most alkaline), with 7 being neutral. The low pH of sulfuric acid is a result of the high concentration of hydrogen ions (H+ ions) when dissolved in water.

However, the pH of sulfuric acid can change depending on its concentration. When it is diluted with water, the pH will increase, but will still remain acidic. Dilute sulfuric acid is commonly used in various industrial and laboratory applications, and its pH can be calculated based on concentration. For example, a 1 molar (1M) solution of sulfuric acid completely dissociated in water will have a pH of approximately 0.3.

Always use caution when handling sulfuric acid, especially in concentrated form, as it is highly corrosive and can cause severe chemical burns and other hazards. Proper safety precautions should be taken when working with this substance.

Sulfuric acid boiling point

The boiling point of sulfuric acid (H2SO4) is approximately 337 °C (639 °F) at standard atmospheric pressure. However, it is important to note that sulfuric acid can decompose at high temperatures, especially when heated at atmospheric pressure, so care must be taken when heating it.

When sulfuric acid is heated, it can undergo various reactions and lose water molecules, resulting in the formation of sulfur trioxide (SO3) and water vapor. The boiling point mentioned here matches the boiling point of concentrated sulfuric acid at standard atmospheric pressure. The boiling point of dilute solution of sulfuric acid will be lower due to the presence of water.

Again, it is important to handle sulfuric acid with care and follow proper safety procedures when heating or working with it, as it is a highly corrosive and dangerous substance.