Im fed up with this assignment please help
The oxide formed when selenium burns in air dissolves in water to give a solution of selenious acid, H2SeO3. The solution conducts electricity, and turns blue litmus paper red.
State the evidence that supports classifying H2SeO3 as an acid, and identify the positively charged ion present in an aqueous solution of the acid.
Blue litmus turns red is an acid indiator.
H ions are the acid part of the molecule.
If you are fed up on this easy stuff (easy= memorization), you ought to drop the course now, and avoid grief when you have to start thinking and analyzing.
I'm here to help! It seems like you already know part of the answer.
To determine the evidence that supports classifying H2SeO3 as an acid, we can look at two properties: the ability to conduct electricity and the reaction with litmus paper.
1. The solution conducting electricity: When an acid dissolves in water, it ionizes and produces free hydrogen ions (H+). These ions can move and carry electric charge, allowing the solution to conduct electricity. So, the fact that the solution of H2SeO3 conducts electricity indicates that it contains free hydrogen ions, which is characteristic of acids.
2. Turning blue litmus paper red: Litmus paper is a common acid-base indicator. Blue litmus paper turns red in the presence of an acid. In the case of H2SeO3, the solution turns blue litmus paper red, indicating the presence of acidic properties.
So, the evidence that supports classifying H2SeO3 as an acid is its ability to conduct electricity and its ability to turn blue litmus paper red.
Regarding the positively charged ion present in an aqueous solution of the acid, you correctly identified it as the hydrogen ion (H+). In a solution of H2SeO3, the positively charged hydrogen ions dissociate from the acid molecule, while the negatively charged ions (SeO3^2-) remain in the solution. Therefore, the positively charged ion in the aqueous solution of H2SeO3 is the hydrogen ion (H+).