Question

Calculate the PH of a solution:-

a) containg 2gram of sodium hidroxide in one liter.
b) made by mixing 50ml of 0.01 M Ba (Oh)2 solution with 50 ml water​

Answer 1

Answer:- pH value of the resulting solution is 12.

Solution:- using the dilution equation we will calculate the molarity of the diluted solution.

M_1V_1=M_2V_2

Given:-

M_1 = 0.01 M

V_1 = 50 mL

V_2 = 50 + 50 = 100 mL

M_2 = ?

Let's plug in the values and solve it for the molarity of diluted solution.

0.01M(50mL)=M_2(100mL)

M_2=\frac{0.01M(50mL)}{100mL}

M_2=0.005M

Ba(OH)_2(aq)\rightarrow Ba^+^2(aq)+2OH^-(aq)

From above equation, 1 mol of barium hydroxide gives 2 moles of hydroxide ions. So, the concentration of hydroxide ions would also be 2 times the concentration of diluted solution of barium hydroxide.

[OH^-]=2(0.005M) = 0.01M

pOH=-log[OH^-]

pOH=-log0.01

pOH = 2

pH = 14 - pOH

pH = 14 - 2

pH = 12

So, the pH value of the resulting solution is 12.

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