Aqueous potassium sulfate can be prepared by titrating dilute sulfuric acid against aqueous potassium carbonate. What conclusion can e drawn from here? And explain why is it so.
H2SO4 + K2CO3 ==> K2SO4 + H2CO3
(and H2CO3 breaks down to form H2O and CO2).
If K2SO4 is to form from this reaction, the other product must be (a) a solid(insoluble) (b) a gas (c)slightly ionized substance. It isn't a solid therefore it must be b or c. If be forms it is transient and we see a gas being evolved; therefore, c is the reason the reaction proceeds.
Which conclusion can be drawn when aqueous potassium sulphate can be prepared by titrating dilute sulphuric acid against aqueous potassium carbonate
From the given information, the conclusion that can be drawn is that the reaction between dilute sulfuric acid and aqueous potassium carbonate forms aqueous potassium sulfate.
This can be explained by the following chemical equation:
H2SO4 (dilute) + K2CO3 (aqueous) → K2SO4 (aqueous) + H2O + CO2
In the reaction, dilute sulfuric acid (H2SO4) reacts with aqueous potassium carbonate (K2CO3). This reaction results in the formation of aqueous potassium sulfate (K2SO4), water (H2O), and carbon dioxide (CO2) as byproducts.
The formation of aqueous potassium sulfate can be confirmed by performing a titration, which is a process of determining the concentration of a substance in a solution by reacting it with a known volume and concentration of another substance.
By adding the dilute sulfuric acid gradually to the aqueous potassium carbonate, and measuring the volume of acid required to completely react, the stoichiometry of the reaction can be determined, leading to the conclusion that the reaction produces aqueous potassium sulfate.
The conclusion that can be drawn from the statement is that potassium carbonate is a weak base, and sulfuric acid is a strong acid.
When titrating dilute sulfuric acid against aqueous potassium carbonate, the acid-base reaction that occurs is as follows:
H2SO4 + K2CO3 -> K2SO4 + H2O + CO2
In this reaction, sulfuric acid (H2SO4) donates protons (H+) to carbonate ions (CO3^2-) derived from potassium carbonate (K2CO3). This reaction produces potassium sulfate (K2SO4), water (H2O), and carbon dioxide (CO2) as products.
The fact that potassium sulfate is formed as a product indicates that complete neutralization has occurred. This is because potassium sulfate (K2SO4) is a salt, and salts are formed when an acid and a base fully react with each other.
Furthermore, the use of dilute sulfuric acid and the presence of the carbonate ion suggest that potassium carbonate is a weak base. This is because strong acids react completely with weak bases to form salts, and sulfuric acid (H2SO4) is classified as a strong acid.
To summarize, the conclusion that can be drawn from the statement is that aqueous potassium sulfate can be prepared by titrating dilute sulfuric acid against aqueous potassium carbonate because potassium carbonate is a weak base and sulfuric acid is a strong acid, resulting in complete neutralization and the formation of potassium sulfate.