2. 200 ml of 0.1 M Na2CO3 + 100 ml of 0,365% HCl
3. 50ml of 0.1M Na3PO4 + 100ml of 0.05 M H2SO4
4. 80 ml of 0.01M HNO2 + 20ml of 0.05 M
HNO3
5. 20 ml of 0.05 M H2C2O4 + 200 ml of 0.01 M KOH
6. 100 ml of 0.05 M H2S + 100 ml of 0.1 M NaOH
How to find pH of solutions
To calculate pH of 80ml 0.01M HNO2 + 20ml of 0.05M HNO3:
Each acid will dissociate to give H+ ions.
pH is defined as the negative logarithm of H+ion concentration present in the solution.
All acids have pH < 7
water or any neutral solution has pH =7
All bases have pH>7
As we got a mixture of two different acids here, we will get only H+ ions concentration in the solution and pH <7
Lets calculate the number of moles of H+ ions from each acids
generally the formula to calculate molarity is
so number of moles = molarity x volume of the solution in litre
From HNO2, number of moles of H+ ions = (0.01x80)/1000 = 0.8 x 10 ^ -3
From HNO3, number of moles of H+ ions = (0.05x20) / 1000 = 1.0 x 10^ -3
Total number of moles of H+ ions = 1.8 x 10^-3
Total volume of the solution = 80 + 20 = 100 ml
Hence, the net H+ ion concentration = (1.8 x10^-3) x1000 /100 = 1.8 x 10^-2
Therefore , pH = - [H+]
= - [ 1.8x10^-2] = 1.745 ...... answer
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