Question

When 100cc of 1m H2So4 is mixed with 20cc of 5m NaoH the resulting solution is.?

Answer 1

Explanation:

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Answer 2

Answer:

Resulting solution is Na₂SO₄ of molarity 0.006M.

Explanation:

The balanced chemical reaction is;

    $H_{2} SO_{4} +2 NaOH$  →  $Na_{2}SO_{4}+2H_{2}O$

We know that 1cc = 1ml

Moles of $H_{2}SO_{4}$ in 100ml of 1M H₂SO₄ solution=$(\frac{1mol}{1000ml})*100ml=0.1mol$

Moles of NaOH in 20ml of 5M NaOH solution=$(\frac{5mol}{1000ml})*20ml=0.1mol$

But we know from balanced equation, 2mol of NaOH reacts with 1mol of H₂SO₄.

∴ for given 0.5 moles  of H₂SO₄ remain unreacted.

Final volume of solution $= 100+20 = 120ml$

Molarity of resulting solution of $Na_{2}SO_{4}=(\frac{0.05mol}{1000ml}) *(120)=0.006M$