Question

If we have \[0.1{\text{ M}}\] of \[20{\text{ ml}}\] \[C{H_3}COOH\]and we add \[0.1{\text{ M}}\] of \[50{\text{ ml}}\] \[NaOH\].What will be the final pH of final solution?

Answer 1

Hint: Acids are those substances which give \[{{\text{H}}^ + }\]in its aqueous form. Bases are those substances which give \[{\text{O}}{{\text{H}}^ - }\]in its aqueous form. In historical times, an acid became any substance that had a bitter taste (e.g., vinegar or lemon juice), brought on steady shadeation adjustments in dyes derived from plants

Complete answer:
We can outline acids as materials that dissolve in water to provide H+ ions, while bases are described as materials that dissolve in water to provide OH− ions. In fact, that is the simplest one viable set of definitions. Here we want a quantity of acetic acid and base sodium hydroxide. If volumes aren't recognized we cannot discover pH of the ensuing answers. So the answer acts because the salt answer for locating pH we want to use salt hydrolysis method for locating pH.
Now the aggregate will act as salt sodium acetate of weak acid acetic acid and robust base sodium hydroxide.
 \[C{H_3}COOH + NaOH\xrightarrow{{}}C{H_3}COONa + {H_2}O\]
Concentration of acid \[ = 0.1{\text{M}}\]
 Concentration of base \[ = 0.1{\text{M}}\]
\[
  pH = pKa + \log \dfrac{{[A - ]}}{{[HA]}} \\
  pH = - \log (Ka) + \log \dfrac{{[A - ]}}{{[HA]}} \\
  pH = - \log (1.8 \times {10^{ - 5}}) + \log \dfrac{{[0.1]}}{{[0.1]}} \\
  pH = 4.74 \\
 \]
In chemistry, pH is a scale used to specify the acidity or basicity of an aqueous answer. Acidic answers (answers with better concentrations of H+ ions) are measured to have decreased pH values than simple or alkaline answers.

Note:
The pH scale is logarithmic and inversely shows the awareness of hydrogen ions within the answer. This is due to the fact the method used to calculate pH approximates the bad of the bottom 10 logarithm of the molar awareness of hydrogen ions inside the answer. More precisely, pH is the bad of the bottom 10 logarithms of the hobby of the H+ ion.