Question

рассчитайте объем раствора серной кислоты с концентрацией H2so4 0,1 моль/дм3, который потребуется для осаждения ионов бария из 20 г раствора хлорида бария с массовой долей BaCl2 3%. Срочно! Даю 100!

Answer 1

Ответ: 0,29 л

Дано:

с(H2SO4) = 0,1 моль/дм³

m(p-pa BaCl2) = 20 г

ω(BaCl2) = 3% или 0,03

Найти:

m(p-pa H2SO4)-?

Объяснение:

m(BaCl2) = m(p-pa BaCl2)*ω(BaCl2) = 20 г*0,03 = 0,6 г

M(BaCl2) = 208 г/моль

n(BaCl2) = m(BaCl2)/M(BaCl2) = 0,6 г/208 г/моль = 0,029 моль

Составляем УХР:

BaCl2 + H2SO4 = BaSO4↓ + 2HCl

Из УХР видно, что n(H2SO4) = n(BaCl2); n(H2SO4) = 0,029 моль

m(p-pa H2SO4) = n(H2SO4)/с(H2SO4)

m(p-pa H2SO4) = 0,029 моль/0,1 моль/дм³ = 0,29 дм³

Ответ: 0,29 дм³

Answer 2

Calculating the Volume of Sulfuric Acid Solution Required

To calculate the volume of sulfuric acid solution with a concentration of H2SO4 0.1 mol/dm3 needed to precipitate barium ions from a 20g solution of barium chloride with a mass fraction of BaCl2 3%, we can use the following steps:

1. Determine the Moles of Barium Ions in the Barium Chloride Solution: - The mass of barium chloride (BaCl2) in the solution is 20g, and the mass fraction of BaCl2 is 3%. We can calculate the moles of BaCl2 using its molar mass.

2. Write the Chemical Equation for the Precipitation Reaction: - The precipitation reaction between barium chloride and sulfuric acid can be represented by the following chemical equation: ``` BaCl2 + H2SO4 -> BaSO4 + 2HCl ```

3. Use Stoichiometry to Relate the Moles of Barium Ions to Sulfuric Acid: - From the balanced chemical equation, we can determine the stoichiometric ratio between BaCl2 and H2SO4 to calculate the moles of H2SO4 required.

4. Calculate the Volume of Sulfuric Acid Solution: - Once we have the moles of H2SO4 required, we can use the concentration of the sulfuric acid solution to calculate the volume needed.

Calculation Steps

1. Determine the Moles of Barium Ions in the Barium Chloride Solution: - The molar mass of BaCl2 is 137.327 g/mol (Ba: 137.327 g/mol, Cl: 35.453 g/mol). - The mass of BaCl2 in the solution is 20g, and the mass fraction of BaCl2 is 3%. We can calculate the moles of BaCl2 using its molar mass. - Moles of BaCl2 = (mass of BaCl2 / molar mass of BaCl2) = (20g / 137.327 g/mol) = 0.1457 mol.

2. Use Stoichiometry to Relate the Moles of Barium Ions to Sulfuric Acid: - From the balanced chemical equation, we know that 1 mole of BaCl2 reacts with 1 mole of H2SO4. - Therefore, the moles of H2SO4 required are also 0.1457 mol.

3. Calculate the Volume of Sulfuric Acid Solution: - The concentration of the sulfuric acid solution is 0.1 mol/dm3. - Volume of sulfuric acid solution = (moles of H2SO4 / concentration of H2SO4) = (0.1457 mol / 0.1 mol/dm3) = 1.457 dm3.

The volume of sulfuric acid solution with a concentration of H2SO4 0.1 mol/dm3 required for the precipitation of barium ions from the 20g solution of barium chloride with a mass fraction of BaCl2 3% is approximately 1.457 dm3.