 admin # A chemical supply company sells a concentrated solution of aqueous h2so4 (molar mass 98 g mol−1 ) that is 50. percent h2so4 by mass. at 25°c, the density of the solution is 1.4 g ml−1 . what is the molarity of the h2so4 solution at 25°c?

2 months ago

## Solution 1 Guest #16
2 months ago
Answer is: the molarity of the sulfuric acid is 7.14 M.
ω(H₂SO₄) = 50% ÷ 100% = 0.5.
d(H
₂SO₄) = 1.4 g/mL.
V(H₂SO₄) = 100 mL ÷ 1000 mL/L = 0.1 L..
mr(H₂SO₄) = d(H₂SO₄) · V(H₂SO₄).
mr(H₂SO₄) = 1.4 g/mL · 100 mL.
mr(H₂SO₄) = 140 g.
m(H₂SO₄) = ω(H₂SO₄) · mr(H₂SO₄).
m(H₂SO₄) = 0.5 · 140 g.
m(H₂SO₄) = 70 g.
n(H₂SO₄) = m(H₂SO₄) ÷ M(H₂SO₄).
n(H₂SO₄) = 70 g ÷ 98 g/mol.
n(H₂SO₄) = 0.714 mol.
c(H₂SO₄) = n(H₂SO₄) ÷ V(H₂SO₄).
c(H₂SO₄) = 0.714 mol ÷ 0.1 L.
C(H₂SO₄) = 7.14 M.

## 📚 Related Questions

Question
Calculate the number of moles of naoh present in 11.2 ml of 2.50 m naoh solution
Solution 1
Let's review what is given in this problem.

The volume of the solution is 11.2 milliliters, which is 0.0112 liters (multiply 11.2 mL with 1 L / 1000 mL to get 0.0112).

The molar concentration is 2.5 M. This means that there are 2.5 moles of NaOH per liter in the solution.

Multiply the volume and the molar concentration to get the moles of NaOH in the solution. The "Liter" will cancel out, leaving only moles.
After using a calculator (or computing by hand), you should get the following value: Since the given values were given with 3 significant figures, let's change this answer so there are 3 significant figures.

Thus, your final answer is 2647929
842281
748681
586256
406852
368373
348603
324927
199835
130075
112100
106146
77164
23213
22589
19607
17108
13966
10987
3389