Question

В 735 мг 20% раствора серной кислоты растворили 30 аммиака. Рассчитать массу образовавшейся соли.

Answer 1

Плотность аммиака 681,4 кг/м^3 = 0,0006814 кг/мл - > масса аммиака 0,002 кг
Масса кислоты 0,000735*0,2=0,000147
2NH3 + H2SO4 = (NH4)2SO4
....34....98....130
.0,002....0,000147 аммиак в избытке
....0,000147....x
x=0,00147*130/98=0,00195=1,95 г

Answer 2

Calculation of the Mass of the Formed Salt

To calculate the mass of the formed salt, we need to determine the amount of sulfuric acid and ammonia involved in the reaction.

Given: - Mass of the 20% sulfuric acid solution = 735 mg - Concentration of the sulfuric acid solution = 20% - Volume of ammonia solution = 30 mL

To calculate the mass of the formed salt, we need to consider the balanced chemical equation for the reaction between sulfuric acid (H2SO4) and ammonia (NH3):

H2SO4 + 2NH3 → (NH4)2SO4

From the balanced equation, we can see that one molecule of sulfuric acid reacts with two molecules of ammonia to form one molecule of ammonium sulfate.

To calculate the amount of sulfuric acid and ammonia, we can use the following formulas:

Amount of sulfuric acid = (concentration of sulfuric acid × volume of sulfuric acid solution) / 1000 Amount of ammonia = (concentration of ammonia × volume of ammonia solution) / 1000

Let's calculate the amounts of sulfuric acid and ammonia:

Amount of sulfuric acid = (20% × 735 mg) / 1000 = 0.147 g Amount of ammonia = (30 mL) / 1000 = 0.03 L

Now, we can calculate the amount of the formed salt (ammonium sulfate) using the stoichiometry of the balanced equation:

Amount of ammonium sulfate = (Amount of sulfuric acid) / 1 = 0.147 g

Therefore, the mass of the formed salt (ammonium sulfate) is 0.147 grams.

Please note that the above calculation assumes that the reaction goes to completion and that there are no other limiting factors or side reactions involved.