a sample of Na2SO3.H2O weighing 0.62g is addedto 100ml.1NH2SO4 .THE resulting solution will be?
I assume 0.1NH2SO4 really is 0.1N H2SO4. What are you looking for in the answer? Normality? molarity? acidic? basic? H2SO3 + Na2SO4? what?
Acidic
To determine the resulting solution when a sample of Na2SO3.H2O is added to 100 mL of 1N H2SO4, we need to calculate the reaction that occurs between Na2SO3.H2O (sodium sulfite) and H2SO4 (sulfuric acid).
First, let's write the balanced chemical equation for the reaction:
Na2SO3.H2O + H2SO4 → Na2SO4 + H2O + SO2
Next, we need to calculate the number of moles of Na2SO3.H2O added to the solution. We can use the formula:
moles = mass / molar mass
The molar mass of Na2SO3.H2O can be calculated as follows:
Na (22.99 g/mol) * 2 + S (32.07 g/mol) + O (16 g/mol) * 3 + H (1.01 g/mol) * 2 = 126.04 g/mol
Using the given mass of 0.62 g:
moles of Na2SO3.H2O = 0.62 g / 126.04 g/mol
Now, let's calculate the molarity (M) of the 1N H2SO4 solution:
Molarity (M) = Normality (N) / Molar mass (g/mol) = 1N / 98.09 g/mol
We know that 1N H2SO4 solution contains 98.09 grams of H2SO4 per liter.
Since we are adding 100 mL (0.1 L) of the 1N H2SO4 solution:
moles of H2SO4 = 0.1 L * 1N / 98.09 g/mol
Now, we need to compare the number of moles of Na2SO3.H2O with the number of moles of H2SO4 to determine the limiting reactant. The reactant that has fewer moles is the limiting reactant, and it will determine the amount of products formed.
If the number of moles of Na2SO3.H2O is lower than the number of moles of H2SO4, all of the Na2SO3.H2O will react. Otherwise, only a fraction of the H2SO4 will react, and the remaining amount will be left unreacted.
Finally, we can calculate the resulting solution. If all of the Na2SO3.H2O reacts, the products formed will be Na2SO4 (sodium sulfate), H2O, and SO2 (sulfur dioxide). The resulting solution will contain these products along with the excess H2SO4.
If there is excess H2SO4 remaining, the resulting solution will contain Na2SO4 along with the excess H2SO4.
Please note that the above calculations give an idea of the resulting solution based on stoichiometry and the assumption of complete reaction. However, the actual reaction may depend on experimental conditions such as temperature and reaction kinetics. So, it's always best to experimentally verify the actual outcome.