Question

Why is 1 molar aqueous solution more concentrated than a 1 molal solution?

Answer 1

1m molar concentrated:

• Molar concentration is a determination of a chemical species concentration in a solution, particularly a solute's concentration, in terms of the amount of substance per unit volume of solution.

Reason for 1m more concentrated:

• Because 1 molar solution contains 1 mole of solute in 1 litre of the solution, which includes both solute and solvent, it is more concentrated than 1 molar solution. Consequently, less than 1000 grams of water serve as the solvent mass.
• A solution is made up of a solute (a small amount of a chemical) and a solvent (the chemical that is present in bulk).
• They are unaffected by states such as solid, liquid, gas, and so on.
• Molality(m) and molarity(M) are the two ways to express the concentration of a solute.
• Molality is defined as the number of moles of a substance present in one kilogram of the substance. m=(given mass of the solute molar mass of solute)(1000 mass of solvent in gram) in mathematics, where m represents molality
• $\mathrm{m}=\left(\frac{\text{given mass of solute}}{\text{molar mass of solute}}\right)\times \left(\frac{1000}{\text{mass of solvent in gram}}\right)$
• Molarity(M) calculates the number of moles of solvent present in 1 liter (1000ml) of solution. Molarity is defined in mathematics
• $M=\left(\frac{\text{given mass of solute}}{\text{molar mass of solute}}\right)\times \left(\frac{1000}{\text{volume of solution in}\mathrm{ml}}\right)$
• Because molality is proportional to the mass of the solvent, it is noted that the mass of the solute, in this case, water, is less than 1000gm.
• As a result, a 1 molar aqueous solution must have 1 mole of solute in fewer than 1000 g of solvent.
• In a molal solution, 1 mole of solute must be present in 1000 grams of solvent.
• As a result, the concentration in a 1 molal aqueous solution will be higher than in a 1 molar aqueous solution.