a solution of hcl of concentration 1.5 mole/liter is mixed with another solution of hbr of the same concentration.

calculate:
1)ph of hcl solution alone
2)ph of the final mixture

To calculate the pH of the HCl solution alone, we can use the equation for pH:

pH = -log[H+]

where [H+] represents the concentration of hydrogen ions in the solution.

1) pH of HCl solution alone:
In this case, the concentration of HCl is given as 1.5 mole/liter. Since HCl is a strong acid and fully dissociates in water, the concentration of H+ ions will be equal to the concentration of HCl. Therefore, the pH can be calculated as:

pH = -log[H+]
= -log(1.5)
≈ -log(1.5 × 10^0) (since the concentration is given in moles per liter)
≈ -log(1.5 × 10^0)
≈ -log(1.5)
≈ -0.18
≈ 0.18

So, the pH of the HCl solution alone is approximately 0.18.

2) pH of the final mixture:
To calculate the pH of the final mixture, we need to consider the fact that HBr, like HCl, is a strong acid and fully dissociates in water. When the solutions of HCl and HBr of the same concentration are mixed, the final concentration of hydrogen ions ([H+]) will be the sum of the individual concentrations.

Since both solutions have the same concentration of 1.5 mole/liter, the final concentration of hydrogen ions ([H+]) will be:

[H+] = [HCl] + [HBr] (since HCl and HBr are mixed)

Using the same concentration of 1.5 mole/liter, we get:

[H+] = 1.5 mole/liter + 1.5 mole/liter
= 3 mole/liter

Now, we can calculate the pH of the final mixture using the equation:

pH = -log[H+]
= -log(3)
≈ -log(3 × 10^0) (since the concentration is given in moles per liter)
≈ -log(3 × 10^0)
≈ -log(3)
≈ -0.48
≈ 0.48

So, the pH of the final mixture is approximately 0.48.