If 535 Ml of gaseous HCL, at 26.5 degrees Celsius and 747mm Hg, is dissolved in enough water to prepare 625 ml of solution, what is the PH of the solution?
What is Ml ? megaliters?
You need to find the moles of HCl from the ideal gas equation. PV=nRT
Then, assume the HCl entirely dissociates, so the Molaritiy= molesH/.625
Then apply your pH definition.
1.5
To find the pH of the solution, we need to know the concentration of HCl in the solution. From the given information, we have 535 mL of gaseous HCl that is dissolved in enough water to prepare 625 ml of solution. However, we don't know the initial concentration or the final volume of the solution.
To find the concentration of HCl in the solution, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure in atm
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 atm L/mol K)
T = temperature in Kelvin
First, let's convert the given temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 26.5 + 273.15 = 299.65 K
Next, let's convert the given pressure from mmHg to atm:
P(atm) = P(mmHg) / 760
P(atm) = 747 mmHg / 760 = 0.981579 atm
Now that we have the temperature and pressure, we can calculate the number of moles of HCl using the ideal gas law equation:
PV = nRT
n = (PV) / (RT)
n = (0.981579 atm) * (0.535 L) / [(0.0821 atm L/mol K) * 299.65 K]
n ≈ 0.0228 moles
Now, we know we have 0.0228 moles of HCl in 625 mL of solution. To find the concentration of HCl, we divide the moles by the volume of the solution:
Concentration (M) = Moles / Volume (L)
Concentration (M) = 0.0228 moles / 0.625 L
Concentration (M) ≈ 0.0365 M
Finally, we can calculate the pH of the solution using the formula:
pH = -log10 [H+]
Since HCl is a strong acid, it completely ionizes in water. Therefore, the concentration of H+ ions is equal to the concentration of HCl.
So, the pH of the solution is:
pH = -log10 (0.0365)
pH ≈ 1.437
Therefore, the pH of the solution is approximately 1.437.