Which salts will be more soluble in an acidic solution than in pure water?

Which salts will be more soluble in an acidic solution than in pure water?

The ability of a solid to dissolve is known as Solubility, and the dissolving agent can be water or another solution. How a solid dissolve is influenced by different components like temperature, pressure, and polarity. With that in mind, let’s find out which salts will be more soluble in an acidic solution than in pure water. 

Which salts will be more soluble in an acidic solution than in pure water?

For salts to be soluble in water, there must be a complete reaction between the salt and protons ions. Salts with conjugate bases will strongly and readily dissolve in acidic solutions than in water due to strong conjugate bases, which readily result in reaction with protons. For instance, the anion found in salt reacts with H+ion forming a weak acid that you can exchange from the solution by adding an acid.

Which salts will be more soluble in an Acidic solution than in pure water

Salts that are soluble in water have a higher pH compared to those that dissolve in other solubles. They have positively charged ions called cations while those with the negatively charged ions are known as anions. 

Which salts will be more soluble in an acidic solution than in Pure Water

When a strong acid and a weak base react, an acid salt is formed and the reaction is neutral. For example, in a reaction between hydraulic acid as the strong acid and ammonia as the weak base, it results in water and ammonium chloride making it an acidic salt.

  1. Sn(OH)2 + H+ reacts with OH- to form H2O making it more possible in an acidic solution than in pure water.
  2. Adding CuBr to H+ forms a weak acid HBr; thus, it is highly soluble in acidic solutions than pure water.
  3. Ag2SO4 + H+ form HSO4- with a K2 for H2SO4. In H2SO4. No K1 because it is a strong acid the first H explains its solubility in acidic solutions than pure water.
  4. For BaSO3 + H+ forms HSO3- with a k2 for k2SO3. The K1 in H2SO3 makes it a strong acid for the first H. So, BaSO3 will dissolve in acid rather than pure water.

Acidic solution Solubility

The carbonate rule is what makes the difference in salt metal carbonates. But, without it, anything with “acid” is soluble in water. And, the capacity of acids to produce ions allows hydronium ions to protonate the OH- ions of Zn(OH)2 and SO2.

How to determine Salts that are more soluble in acidic solutions than in pure water?

Insoluble salts with anions are more soluble with a weak acid-base such as hydroxide, acetate, carbonate, phosphate, and sulfide. Acidic solutions have stronger acids that increase solubility than in pure water. Here are the main reasons for solubility:

Which salts will be more soluble in an acidic solution than in pure water?

(a) Compounds are more soluble in acidic solutions because they break down in water giving the carbonate ion in the weak carbonic acid.

(b) Salts that are more soluble in acidic solutions dissociate in the water to produce sulfide ion, the weak acidic base of hydrogen sulfide.

(c) The stable compound of silver chloride breaks down to silver and chloride ions in water. 

(d) Any solid that breaks down into lead and iodide ions in water, the Iodide ion makes the neutral weak base in the strong acid proving that solubility does not increase in acidic solution.

Conclusion

The neutral reaction between a strong and weak acid brings forth an acidic salt. With the question, which salts will be more soluble in an acidic solution than in pure water? As demonstrated above, insoluble salts with anions or a weak acid-base increase solubility while in strong acids than in pure water. 

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