Question

Calculate the pH of 0.002M HCl solution.​

Answer 1

Answer:

1.7

Explanation:

Since HCl is a strong acid it completely dissociates. Therefore all the H+ protonates water molecules to give H3O+. Its concentration here is high enough to ignore H3O+ contribution from water so the pH is just -log(0.02) = 1.7. pH + pOH = 14 so the pOH is 12.3.

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Answer 2

Answer:

The pH of 0.002M HCl solution is 2.7.

Explanation:

The pH of a compound is given as,

$pH=-log[H^+]$     (1)

Where,

pH=pH of the solution

[H⁺]=hydrogen ion concentration

From the question we have,

[H⁺]=0.002M=2×10⁻³M

By substituting the value of [H⁺] in equation (1) we get,

$pH=-log[2\times 10^-^3]$

$pH=3-log2$

$pH=3-0.3$

$pH=2.7$

Hence, the pH of the solution is 2.7.

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