Question

the PH value of 0.005M solution of HCL​

Answer 1

Hope this helps you and you have understood the concept.

Answer 2

$\bigstar$ Answer $\bigstar$

$\checkmark$ Given:

0.005 M Solution of $\rm HCl$

$\checkmark$ To Find:

pH value of 0.005 M Solution of $\rm HCl$

$\checkmark$ Solution:

​We know that,

$\rm HCl$ is a strong monoprotic acid

$\rm HCl$ dissociates completely into ions

The ionization equation for $\rm HCl$ is

$\red{\boxed{\rm HCl \longrightarrow H^{+} + Cl^{-}}}$

From the above equation we can understand that,

Each molecule of $\rm HCl$ will produce 1 hydrogen ion

Hence,

Concentration of H⁺ will be equal to the Concentration of HCl

Therefore,

[ H⁺ ] = [ HCl ]

Given that,

0.005 M Solution of $\rm HCl$

Therefore,

[ H⁺ ] = [ HCl ] = 0.005 M

[ H⁺ ] = 0.005 M

We know that,

pH is defined as the negative logarithm of the hydrogen ion in solution

Mathematically,

$\pink{\boxed{\boxed{\rm pH=-log[H^{+}]}}}$

We found out that,

[ H⁺ ] = 0.005

Therefore,

$\blue{\implies \rm pH=-log[0.005]}$

$\green{\implies \rm pH=-(-2.301)}$

NOTE:

→ log 0.005 = -2.301

Therefore,

$\orange{\implies \rm pH=2.301}$

Approximately,

$\star$ pH = 2.3

Hence,

The pH value of 0.005 M Solution of $\rm HCl$ is 2.3