Question

One litre solution of which of the following contains more H+ ions: Blood, pH= 7.4 or Vinegar, pH= 2.5. Please full explanation.​

Answer 1

$\pink{ \boxed{\boxed{\begin{array}{cc} \maltese  \bf \: \: given \\ \\ \to \rm \:volume \: \: v = 1 \: ltr \\ \\ \to \rm \:P^H \: of \: blood \: = 7.4 \\ \\ \to \rm \:P^H \: of \: vinegar \: \: = 2.5 \end{array}}}}$

$\pink{ \boxed{\boxed{\begin{array}{cc} \maltese  \bf \underline{ \bf \: blood} \\ \\ \rm \: P^H = - log [H ^ + ] \\ \\ = > \rm \: log[H ^ + ] = - P^H = - 7.4 \\ \\ = > \rm \: [H ^ + ] =antilog( - 7.4) \\ \\ = > \rm \: [H ^ + ] = 3.98 \times {10}^{ - 8} \: molar \\ \\ \\ \rm \: number \: of \: mole \: in \: blood = n _ {\small{{blood}}} \\ \\ \rm \: n _ {\small{{blood}}} = concentration \: \times \: volume \\ \\ \rm = [H ^ + ] \times v \\ \\ \rm = 3.98 \times {10}^{ - 8} \times 1 \\ \\ = 3.98 \times {10}^{ - 8} \end{array}}}}$

${ \boxed{\boxed{\begin{array}{cc} \maltese  \bf \underline{ \bf \: vinegar} \\ \\ \rm \: P^H = - log [H ^ + ] \\ \\ = > \rm \: log[H ^ + ] = - P^H = -2.5\\ \\ = > \rm \: [H ^ + ] =antilog( - 2.5) \\ \\ = > \rm \: [H ^ + ] = 3.16 \times {10}^{ - 3} \: molar \\ \\ \\ \rm \: number \: of \: mole \: in \: blood = n _ {\small{{vinegar}}} \\ \\ \rm \: n _ {\small{{vinegar}}} = concentration \: \times \: volume \\ \\ \rm = [H ^ + ] \times v \\ \\ \rm = 3.16\times {10}^{ - 3} \times 1 \\ \\ = 3.16 \times {10}^{ -3} \end{array}}}}$

$\rm \: n _ {\small{{vinegar}}}> n _ {\small{{blood}}}$

So in the vinegar number of mole of H+ is much than the blood.

Note :

• $[H ^ + ]\:indicates \:\:concentration$

• n= CV

here

n = number of mole

C = concentration

V = volume in litre

Answer 2

• 1 is the ph value of gastric juice.

• 7 is the ph value of brine solution.

• 10 is the ph value of milk of magnesia.

• 13 is the ph value of aqueous sodium hydroxide.