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Furkat [3]
3 years ago
9

Find the volume of 0.160 M sulfuric acid necessary to react completely with 75.0 g sodium hydroxide.

Chemistry
1 answer:
ladessa [460]3 years ago
3 0

The volume of 0.160 M sulfuric acid necessary to react completely with 75.0 g sodium hydroxide is 0.15L

The reaction of sulphuric acid and sodium hydroxide is expressed as:

2NaOH + H_2SO_4 ==> Na_2SO_4 + 2H_2O

Determine the moles of NaOH present

Molar mass of NaOH = 23 + 16 + 1 = 40g/mole

Given that mass of NaOH is 75.0g

Mole of NaOH = 75/40  = 1.875moles

Determine the number of moles H_2SO_4 needed to react with 1.875 moles NaOH

Moles of H_2SO_4 = \frac{1.875}{2} = 0.9375moles of H_2SO_4

Recall that volume = Molar mass * number of moles

Volume of H_2SO_4 =  0.160 * 0.9375

Volume of  H_2SO_4 = 0.15L

Hence the volume of 0.160 M sulfuric acid necessary to react completely with 75.0 g sodium hydroxide is 0.15L

Learn more here: brainly.com/question/837939

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