Question

Какую массу 5% раствора гидроксида бария нужно прилить к 100г 9,8% раствора серной кислоты, чтобы получить чистую воду? Сколько г. воды будет в колбе по окончанию реакции? ПОМОГИТЕ ПОЖАЛУЙСТА!!!!

Answer 1

n(H2SO4) = 100g * 0,098 / 98g/mol = 0.1 mol

H2SO4 + Ba(OH)2 = BaSO4 + 2H2O

==> n(H2SO4) = n(Ba(OH)2)

==> n(Ba(OH)2) = 0,1mol

m(solution) = 0,1 mol * (137 + 32 + 2)g / 0,05 = 342g

m(H2O)1 = 100 - 100*0,098 = 90,2 g

m(H2O)2 = 342 - 342*0,05 = 324,9 g

m(H2O)3 = 0,1 mol * 2 * 18 = 3,6 g

===> sum m(H2O) = 90,2 g + 324,9g + 3,6g = 418,7 g

Answer 2

Calculation of the Mass of Barium Hydroxide Solution Needed

To calculate the mass of the 5% barium hydroxide solution needed to react with 100g of 9.8% sulfuric acid solution, we need to determine the stoichiometry of the reaction and use it to find the required amount of barium hydroxide.

The balanced chemical equation for the reaction between barium hydroxide (Ba(OH)2) and sulfuric acid (H2SO4) is:

Ba(OH)2 + H2SO4 → BaSO4 + 2H2O

From the equation, we can see that one mole of barium hydroxide reacts with one mole of sulfuric acid to produce one mole of barium sulfate and two moles of water.

To find the amount of barium hydroxide needed, we can use the concept of stoichiometry and the given concentrations of the solutions.

Let's assume that x grams of the 5% barium hydroxide solution is required.

The concentration of a solution is defined as the amount of solute (in this case, barium hydroxide) divided by the volume of the solution.

For the 5% barium hydroxide solution, the concentration can be expressed as:

5% = (mass of barium hydroxide / volume of solution) * 100

Since we are given the mass of the solution (x grams) and the concentration (5%), we can rearrange the equation to solve for the mass of barium hydroxide:

(mass of barium hydroxide) = (5/100) * x

Now, let's calculate the mass of barium hydroxide needed:

(mass of barium hydroxide) = (5/100) * x = 0.05x grams

Calculation of the Amount of Water Produced

To calculate the amount of water produced in the reaction, we need to determine the stoichiometry of the reaction and use it to find the number of moles of water produced.

From the balanced chemical equation:

Ba(OH)2 + H2SO4 → BaSO4 + 2H2O

We can see that for every mole of barium hydroxide, two moles of water are produced.

To find the number of moles of water produced, we need to know the number of moles of barium hydroxide used. We can calculate this using the molar mass of barium hydroxide.

The molar mass of barium hydroxide (Ba(OH)2) can be calculated as:

Molar mass of Ba(OH)2 = (molar mass of Ba) + 2 * (molar mass of O) + 2 * (molar mass of H)

Using the atomic masses from the periodic table, we find:

Molar mass of Ba(OH)2 = 137.33 g/mol + 2 * 16.00 g/mol + 2 * 1.01 g/mol = 171.34 g/mol

Now, let's calculate the number of moles of barium hydroxide used:

Number of moles of Ba(OH)2 = (mass of barium hydroxide) / (molar mass of Ba(OH)2)

Substituting the mass of barium hydroxide calculated earlier:

Number of moles of Ba(OH)2 = 0.05x g / 171.34 g/mol

Since one mole of barium hydroxide produces two moles of water, the number of moles of water produced is:

Number of moles of water = 2 * (number of moles of Ba(OH)2)

Now, let's calculate the amount of water produced:

Amount of water produced = (number of moles of water) * (molar mass of water)

The molar mass of water (H2O) is:

Molar mass of H2O = 2 * (molar mass of H) + (molar mass of O) = 2 * 1.01 g/mol + 16.00 g/mol = 18.02 g/mol

Substituting the values:

Amount of water produced = 2 * (0.05x g / 171.34 g/mol) * 18.02 g/mol

Calculation of the Amount of Water in the Flask After the Reaction

To calculate the amount of water in the flask after the reaction, we need to consider the initial amount of water (100g) and subtract the amount of water produced in the reaction.

Let's calculate the amount of water in the flask after the reaction:

Amount of water in the flask = (initial amount of water) - (amount of water produced)

Substituting the values:

Amount of water in the flask = 100g - (2 * (0.05x g / 171.34 g/mol) * 18.02 g/mol) Please note that the value of x, which represents the mass of the 5% barium hydroxide solution needed, has not been provided in the question. To obtain the final numerical values, the value of x needs to be determined or provided.

I hope this helps! Let me know if you have any further questions.