Question

Using this balanced equation: 2 NaOH + H2SO4 —> H2O + Na2SO4

How many grams of sodium sulfate will be formed if you start with 150 grams of
sodium hydroxide and you have an excess of sulfuric acid?

Please help!

Answer 1

266. 25 g

Step-by-step explanation:

Data given:

Sodium hydroxide (NaOH) = 150 g

Sodium sulfate Na₂SO₄= ?

Reaction Given:

2 NaOH + H₂SO₄—> H₂O + Na₂SO₄

Solution:

First we have to look at the reaction

2 NaOH + H₂SO₄—> H₂O + Na₂SO₄

2 mol 1 mol

So,

2 mole sodium hydroxide gives 1 mole Na₂SO₄

Now,

Convert moles to mass

for this purpose we have to know molar mass of sodium hydroxide (NaOH) and sodium sulfate (Na₂SO₄)

Molar mass of NaOH = 23 + 16 +1

Molar mass of NaOH = 40 g

Molar mass of Na₂SO₄ = 2(23) + 32+ 4(16)

Molar mass of Na₂SO₄ = 46 + 32+ 64

Molar mass of Na₂SO₄ = 142

Mole Mass Conversion:

2 NaOH + H₂SO₄ —> H₂O + Na₂SO₄

2 mol (40g/mol) 1 mol (142 g/mol)

So

2 NaOH + H₂SO₄—> H₂O + Na₂SO₄

80 g 142 g

Apply unity formula

80 g of NaOH ≅ 142 g of Na₂SO₄

150 g of NaOH ≅ X g of Na₂SO₄

by Cross multiplication

X g of Na₂SO₄ = 142g x 150g / 80 g

X g of Na₂SO₄ = 266. 25 g

So 150 g of sodium hydroxide will give 266.25 g Na₂SO₄