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This is mostly the case of sulfuric acid. Commercially available sulfuric acid is dense (~1.8 g/ml) and when water is added, it may not mix. In this case a layer of hot weak acid solution is formed, which boils and sprays around. When acid is poured into water, it flows down the flask and mixes much better, so no boiling occurs.

The reason for it is high energy release in reaction of hydration of sulfuric acid ions. Do not believe that heat comes from dissociation, dissociation of acids, bases and salts always consume energy. The energy is released from subsequent hydration, and the release may be high, especially if $H^+$ or $OH^-$ ions are hydrated.

This is mostly the case for sulfuric acid. Commercially available sulfuric acid is dense (~1.8 g/ml) and when water is added, it may not mix. In this case a layer of hot weak acid solution is formed, which boils and sprays around. When acid is poured into water, it flows down the flask and mixes much better, so no boiling occurs.

The reason this occurs is due to the large amount of energy released in the hydration reaction of sulfuric acid ions. Do not believe that heat comes from dissociation, as the dissociation of acids, bases, and salts always consumes energy. The energy is released from subsequent hydration, and the release may be high, especially if $\ce{H+}$ or $\ce{OH-}$ ions are hydrated.

This is mostly the case of sulfuric acid. Commercially available sulphuric acid is dense (~1.8 g/ml) and when water is added, it may not mix. In this case a layer of hot weak acid solution is formed, it boils and sprays around. When acid is poured into water, is flows down the flask and mixes much better, so no boiling occurs.

The reason for it is high energy release in reaction of hydration of sulfuric acid ions. Do not believe that heat comes from dissociation, dissociation of acids, bases and salts always consume energy. The energy is released from subsequent hydration, and the release may be hight, especially if $H^+$ or $OH^-$ ions are hydrated.

This is mostly the case of sulfuric acid. Commercially available sulfuric acid is dense (~1.8 g/ml) and when water is added, it may not mix. In this case a layer of hot weak acid solution is formed, which boils and sprays around. When acid is poured into water, it flows down the flask and mixes much better, so no boiling occurs.

The reason for it is high energy release in reaction of hydration of sulfuric acid ions. Do not believe that heat comes from dissociation, dissociation of acids, bases and salts always consume energy. The energy is released from subsequent hydration, and the release may be high, especially if $H^+$ or $OH^-$ ions are hydrated.

This is mostly the case of sulfuric acid. Commercially available sulphuric acid is dense (~1.8 g/ml) and when water is added, it may not mix. In this case a layer of hot weak acid solution is formed, it boils and sprays around. When acid is poured into water, is flows down the flask and mixes much better, so no boiling occurs.

The reason for it is hight energy release in reaction of hydration of sulfuric acid ions. Do not believe that heat comes from dissociation, dissociation of acids, bases and salts always consume energy. The energy is released from subsequent hydration, and the release may be hight, especially if $H^+$ or $OH^-$ ions are hydrated.

This is mostly the case of sulfuric acid. Commercially available sulphuric acid is dense (~1.8 g/ml) and when water is added, it may not mix. In this case a layer of hot weak acid solution is formed, it boils and sprays around. When acid is poured into water, is flows down the flask and mixes much better, so no boiling occurs.

The reason for it is high energy release in reaction of hydration of sulfuric acid ions. Do not believe that heat comes from dissociation, dissociation of acids, bases and salts always consume energy. The energy is released from subsequent hydration, and the release may be hight, especially if $H^+$ or $OH^-$ ions are hydrated.