Question

how to prepare 1M of sulphuric acid​

Answer 1

To prepare 1M of sulphuric acid​ we have add 54.3 ml of Sulphuric Acid.

Explanation:

• The Molecular weight of  $H2SO4$ is  98 g/mol.
• Next we add 98g of conc. acid and makeup to 1 liter of water.
• As Acid is a liquid,density should be taken into account
• Density =Mass/volume
• Density given on the bottle of Sulphuric acid is 1.84 g/ml
• Volume =$\frac{98}{1.84}$ where mass =98 gm and density is 1.84 g/mol
• Volume =53.2 ml
• Purity of acid is $98%$ %
• 53.2 ml of the given acid which is $100$ % pure is to be converted to $98$%
• so $100$ % × $\frac{53.2}{98}$=$54.3$ % of concentrated acid.
• Now add $54.3$ ml to $0.9$ L distilled water
• Keep continuous stirring and after that make the solution to 1 liter with distilled water.
• Thus in this way 1M of sulphuirc acid can be prepared.

Answer 2

Step-by-Step Explanation:

To make 1M sulphuric acid from concentrated sulphuric acid, follow these steps:

1. First, examine the molecular weight of $H_{2}SO_{4}$ $= 98 g/mol$, therefore, you must mix 98g of concentrated acid with 1 liter of water.
2. You need to take density into account as acid is a liquid: where $Density = \frac{Mass}{Volume}$ which is given on the bottle to be (about) $1.84 g/mL$, so then you have: $Volume = \frac{98g}{1.84(g/mL)} = 53.2 mL$
3. Now you must consider the acid purity, which is normally 98%, and then do the following: If the 53.2 mL acid were 100 percent pure, convert it to 98 percent purity, So $\frac{53.2 }{ 98}$ x $100$% $= 54.3 mL$
4. Finally, while continually stirring (developing heat), add this 54.3 mL to roughly 0.9 L dist. water, and then fill it up to 1.00 L with dist. water.

#SPJ3