# What volume of 95% sulphuric acid (density = 1.85 g/mL) and what mass of water must be taken to prepare 100 mL of 15% solution of sulphuric acid (density = 1.10 g/mL) ?

### Asked by abhinavsaini123 | 6th Jul, 2015, 09:16: AM

**To find: **
Volume of 95% sulphuric acid (density = 1.85 g/mL)
Mass of water to prepare 100 mL of 15% solution of sulphuric acid (density = 1.10 g/mL)
**Solution:**
Volume of the solution = 100 cm^{2}

Density of the solution = 1.10 g/cm^{3}

Therefore, Mass of 100 cm^{3} of solution = 100 x 1.10 g =110 g

The given solutions is 15%. Therefore, 100 g of solution contains 15 g of H_{2}SO_{4}

Then, mass H_{2}SO_{4} in 110 g (100 cm3 ) of solution =

Mass of water in 110 g (100cm3 ) of solution = (110 - 16.5) g = 93.5 g

To obtain 100 cm^{3} of 15 % solution acid, we require the given information.

Mass of water = 93.5 g

Mass of H_{2}SO_{4 }(100% pure) = 16.5 g

Since, the given sulphuric acid is 95% pure, hence,

Mass of H_{2}SO_{4} (95%) will be required =

**To find:**

**Solution:**

Volume of the solution = 100 cm^{2}

Density of the solution = 1.10 g/cm^{3}

Therefore, Mass of 100 cm^{3} of solution = 100 x 1.10 g =110 g

The given solutions is 15%. Therefore, 100 g of solution contains 15 g of H_{2}SO_{4}

Then, mass H_{2}SO_{4} in 110 g (100 cm3 ) of solution =

Mass of water in 110 g (100cm3 ) of solution = (110 - 16.5) g = 93.5 g

To obtain 100 cm^{3}of 15 % solution acid, we require the given information.

Mass of water = 93.5 g

Mass of H_{2}SO_{4 }(100% pure) = 16.5 g

Since, the given sulphuric acid is 95% pure, hence,

Mass of H_{2}SO_{4} (95%) will be required =

### Answered by Hanisha Vyas | 6th Jul, 2015, 12:46: PM

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