Question

how many gram of h2so4 should be weight to prepare 250 ml of solution?​

Answer 1

Answer:

49 g of H2SO4 in 250 ml.

Reason -

A 1 normal (1 N) solution contains 1 equivalent weight of solute per liter of solution.

The equivalent weights of solute per liter of solution of H2SO4 is 2 since in 1 mole of sulfuric acid there are 2 moles of hydronium ions.

A molar solution contains 1 mole of solute per liter of solution.

An N/10 solution contains 0.1 / 2 equivalent weight of solute per liter solution. It is 0.05 equivalent weight.

The molar mass of H2SO4 is 98 grams.The equivalent mass of 1 N solution of H2SO4 is 98 * 0.5 which is 49 grams. The 0.1 N solution has 4.9 grams per liter of solution.

Therefore the amount of H2SO4 in 250 mL 0.1 N is 4.9 grams * 0.25. This amount is 1.225 grams.

Answer 2

Answer:

49 g $H_2SO_4$ should be weight to prepare 250 ml of solution

Explanation:

Step 1:

One equivalent of solute per liter of solution is present in a normal (1N) solution, Here 2 is the equivalent weight of solute per liter of $H_2SO_4$, because there are 2 moles of hydronium ion in 1 mole of sulfuric acid.

We know that 1 mole is present in a molar solution per unit solution

$\frac{N}{10}$ the solution contains $\frac{0.1}{2}$ equivalents of solute per liter of solution.  0.05 Equiv.

Step 2:

We know that the molar mass  $H_2SO_4$ is $98 g$

To calculate the equivalent mass of  $H_2SO_4$ normal solution

98 × 0.5 = 49 grams.  A 0.1N solution is 4.9 grams per liter of solution.

Therefore, the amount of $H_2SO_4$ 250 ml of 0.1N is 4.9 grams ×0.25.

This amount is 1.225 grams

hence, 49 g $H_2SO_4$ should be weight to prepare 250 ml of solution

Write chemical reaction for sodium react with carbon dioxide to form sodium carbonate

brainly.in/question/5682993

0.36g of each aluminum and oxygen produces alumina. Which of the following is a limiting reactant?

brainly.in/question/49783459

#SPJ2