Which one of the solution have high boiling point 1m H3PO4 or 1m CaCl2 ?

Since the van't Hoff factor is higher for CaCl2 it will have the higher b.p. for the same molality.

Well, let's put on our clown noses and dive into some chemistry fun! If we're talking about high boiling points, we're basically determining which solution likes to stick around in its liquid form at higher temperatures. So, between our contenders, 1m H3PO4 (phosphoric acid) and 1m CaCl2 (calcium chloride), who's the heat-loving champion?

In this wacky scenario, it's actually 1m CaCl2 that takes the crown for having a higher boiling point! Calcium chloride is notorious for being quite the attention seeker when it comes to temperature. It just can't resist hanging out as a liquid at higher temperatures, making it more stubborn to boil away.

So, there you have it! The clown-approved answer is 1m CaCl2 because it simply refuses to evaporate easily. Keep in mind that this answer might change if we add more clownish ingredients or alter the conditions. Chemistry can sometimes be as unpredictable as a circus, after all!

To determine which solution has a higher boiling point, we need to compare the properties of the two solutes: H3PO4 (phosphoric acid) and CaCl2 (calcium chloride).

H3PO4 is a weak acid, and it does not dissociate completely in water. It forms H+ ions and PO4 -3 ions. On the other hand, CaCl2 is a strong electrolyte, and it dissociates completely in water to form Ca+2 ions and 2Cl- ions.

Since CaCl2 is a strong electrolyte, it will have more ions in solution compared to H3PO4. This increase in the number of particles in solution is known as the van't Hoff factor and affects the colligative properties of a solution.

Therefore, 1M CaCl2 will have a higher boiling point than 1M H3PO4 solution because it will have a higher van't Hoff factor due to more ionization in solution.

In conclusion, 1M CaCl2 has a higher boiling point compared to 1M H3PO4.

To determine which solution has a higher boiling point, we need to compare the properties of the solutes - H3PO4 (phosphoric acid) and CaCl2 (calcium chloride).

Phosphoric acid (H3PO4) is a weak acid that exists as a liquid at room temperature. However, when it dissolves in water, it dissociates into three H+ ions and one PO4^-3 ion. This means that in a 1m H3PO4 solution, you have one mole of H3PO4 per liter of solution.

Calcium chloride (CaCl2) is an ionic compound that also dissolves in water to form ions. In a 1m CaCl2 solution, you have one mole of CaCl2 per liter of solution. When CaCl2 dissolves in water, it dissociates into one Ca^2+ ion and two Cl^- ions.

Now, let's compare the boiling points. The boiling point of a solution depends on the concentration of the solute particles and their properties. In this case, both H3PO4 and CaCl2 solutions have the same molarity (1m), so the concentration of solute particles is equal.

However, when comparing the properties of the solute particles, we can see that CaCl2 produces more ions in solution than H3PO4. In a 1m CaCl2 solution, you have three ions (one Ca^2+ and two Cl^-) per CaCl2 molecule. On the other hand, in a 1m H3PO4 solution, you have four ions (three H+ and one PO4^-3) per H3PO4 molecule.

The presence of more ions in solution increases the boiling point because it increases the strength of intermolecular forces. Therefore, the 1m CaCl2 solution is expected to have a higher boiling point compared to the 1m H3PO4 solution.

In summary, the 1m CaCl2 solution has a higher boiling point compared to the 1m H3PO4 solution because CaCl2 produces more ions in solution.