First slide

PH of strong acids and strong bases

Question

The pH of a sample of H₂SO₄ is 1.3979. The percentage of the solution is 73.5% (w/w), the density of the solution is

Moderate

A

2.66 x 10^-3 g/cc
B

5.32 x 10^-3g/cc
C

1.33 x 10^-3 g/cc
D

0.01g/cc

Solution

P^H = 1.3979
log[H⁺] =-1-0.3979
[H⁺] = anti log $\overset{}{\bar{2} . 602}$ ;
[H⁺] = 4 x10^-2
[H₂SO₄] = 2 x10^-2 = $M_{H_{2} {SO}_{4}}$
Also, Every 100 g of solution, contains 73.5 g of H₂SO₄
Every $\frac{100}{d} ml$ of solution, contains 73.5 g of H₂SO₄
$M = \frac{\frac{73.5}{98}}{\frac{100}{d} \times 10^{- 3}}$
$\Rightarrow 2 \times 10^{- 2} = \frac{73.5 \times d}{98 \times 10^{- 1}}$
$\Rightarrow d = \frac{2 \times 98 \times 10^{- 3}}{73.5} = 2.66 \times 10^{3} {gml}^{- 1}$

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