Final answer:
The pH of solution B is unknown because the volumes and concentrations are not provided; however, we know that it is more acidic than solution A (pH 10) and the resulting solution C (pH 6), meaning that the pH of B is less than 6.
Step-by-step explanation:
To determine the pH of solution B, we need to understand the concept of the pH scale and how mixing solutions affect their pH values. Given that solution A has a pH of 10, and the resulting solution C has a pH of 6 after A is mixed with B, we can deduce that B must be more acidic than A.
The equation for pH is:
pH = -log [H3O+]
Let's convert the given pH values for solutions A and C to the concentration of hydronium ions.
For A (pH 10): [H3O+] = 10^-10 M
For C (pH 6): [H3O+] = 10^-6 M
Because the pH of the resulting solution C is more acidic than A, the solution B must have contributed to an increase in hydronium ion concentration. The exact pH of B depends on the volumes and the concentrations of A and B, which are not provided. However, we know that the solution B is stronger in acidity than what we have after mixing (pH 6), thus the pH of B is less than 6.