Chemistry College

What is the mass of pure sulfuric acid (H2SO4) required to make 20% and 150g of solution of H2SO4​

Answers

Answer 1

30 g of pure sulfuric acid (H2SO4) is required to make 150 g of 20% solution of H2SO4.

To find the mass of pure sulfuric acid (H2SO4) required to make a 20% and 150g of solution of H2SO4, you first need to understand the concept of concentration.The concentration of a solution is the amount of solute dissolved in a given volume or mass of solvent. It is expressed as a percentage or as the number of moles per liter of solution.20% solution means that 20 grams of solute is present in 100 grams of solution or 20 grams of solute is dissolved in 80 grams of solvent (water in this case).So, for 150 g of solution, the mass of solute (H2SO4) can be calculated as follows:20% solution means 20 g H2SO4 in 100 g solution.So, in 1 g solution, the mass of H2SO4 is:20 g / 100 g = 0.2 g/g solution.So, in 150 g of solution, the mass of H2SO4 is:0.2 g/g solution x 150 g = 30 g.So, 30 g of H2SO4 is required to make 20% and 150g of solution of H2SO4.To find the mass of pure sulfuric acid (H2SO4) required to make the solution, you need to consider the molar mass of H2SO4. The molar mass of H2SO4 is:2(1.01 g/mol) + 32.07 g/mol + 4(16.00 g/mol) = 98.08 g/mol.So, to find the mass of pure sulfuric acid (H2SO4) required to make the solution, you need to use the formula:mass = moles x molar mass.To find the moles of H2SO4, you need to use the formula:moles = concentration x volume / molar mass.For the 20% solution, the concentration is 20 g/100 g solution or 0.2 g/g solution.The volume of the solution is not given, so we cannot calculate the number of moles of H2SO4 required.For the 150 g solution, the mass of H2SO4 required is 30 g.

So, the number of moles of H2SO4 required is:moles = mass / molar mass = 30 g / 98.08 g/mol = 0.305 mol.So, the mass of pure sulfuric acid (H2SO4) required to make the solution is : mass = moles x molar mass = 0.305 mol x 98.08 g/mol = 29.93 g.

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Related Questions

1. Thinley filled a ballon with 14L of hydrogen gas, the the reduced the pressure to 4 atmosphere and found out that the ballon expanded to occupy double the initial volume. What was the initial pressure exerted on the ballon?​

Answers

The initial pressure exerted on the balloon was 8 atmospheres.

To find the initial pressure exerted on the balloon, we can use Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when temperature is constant. The formula for Boyle's Law is P1V1 = P2V2, where P1 and V1 represent the initial pressure and volume, and P2 and V2 represent the final pressure and volume.

In this case, we are given that the initial volume (V1) is 14 L and the final volume (V2) is double the initial volume (2 x V1). We are also given that the final pressure (P2) is 4 atmospheres. We need to find the initial pressure (P1).

Using the formula P1V1 = P2V2 and plugging in the given values, we have:

P1 * 14 = 4 * (2 * 14)

P1 * 14 = 4 * 28

P1 * 14 = 112

To isolate P1, we divide both sides of the equation by 14:

P1 = 112 / 14

P1 = 8

It's important to note that the unit of pressure in this case is atmospheres, as stated in the question. If the pressure unit had been different, appropriate unit conversions would have been necessary.

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