The pH of 1 m solution of a weak monobasic acid (HA) is 2. Then, what is its VAN'T HOFF FACTOR?

Question

The pH of 1 m solution of a weak monobasic acid (HA) is 2. Then, what is its VAN'T HOFF FACTOR? (A) 1.01 (B) 2.3 (C) 3.5 (D) 7

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/2d986d80f7666c95cae5b4f43fac131f-.png" /> pH =2 ∴ ( H +)=10-2 m ∴ C α=10-2 ⇒ 1 × α=10-2 α=0.01 α=(i-1/n-1) ⇒ 0.01=(i-1/2-1) i=1.01

Q. The pH of $1 m$ solution of a weak monobasic acid (HA) is 2. Then, what is its VAN'T HOFF FACTOR?

1.01

2.3

3.5

7

$p H = 2$

$∴ (H^{+}) = 1 0^{- 2} m$

$∴ C α = 1 0^{- 2}$

$\Rightarrow 1 \times α = 1 0^{- 2}$

$α = 0.01$

$α = \frac{i - 1}{n - 1}$

$\Rightarrow 0.01 = \frac{i - 1}{2 - 1}$

$i = 1.01$

Q. The pH of 1m solution of a weak monobasic acid (HA) is 2. Then, what is its VAN'T HOFF FACTOR?

1.01

2.3

3.5

7

pH=2 ∴(H+)=10−2m ∴Cα=10−2 ⇒1×α=10−2 α=0.01 α=n−1i−1​ ⇒0.01=2−1i−1​ i=1.01

Q. The pH of $1 m$ solution of a weak monobasic acid (HA) is 2. Then, what is its VAN'T HOFF FACTOR?

$p H = 2$

$∴ (H^{+}) = 1 0^{- 2} m$

$∴ C α = 1 0^{- 2}$

$\Rightarrow 1 \times α = 1 0^{- 2}$

$α = 0.01$

$α = \frac{i - 1}{n - 1}$

$\Rightarrow 0.01 = \frac{i - 1}{2 - 1}$

$i = 1.01$