A mixture formed by adding 55.0 mL of a 1.5x10^-2 M HCl to 140 mL of 1.0x10^-2 M HI.
How do you calculate the pH for this problem?
Both HCl and HI are strong acids; therefore add them.
mols HCl = M x L = ?
mols HI = M x L = ?
mols (H^+) = ? + ?
Then M = moles/total volume in liters.
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To calculate the pH of a solution, we need to determine the concentration of hydrogen ions (H+) in the solution.
Step 1: Calculate the moles of HCl.
Moles = volume (in liters) × molarity
Given that the volume of HCl added is 55.0 mL (converted to liters, it is 0.055 L), and the molarity of HCl is 1.5 × 10^-2 M, we can calculate the moles of HCl:
Moles of HCl = 0.055 L × 1.5 × 10^-2 M
Step 2: Calculate the moles of HI.
Moles = volume (in liters) × molarity
Given that the volume of HI is 140 mL (converted to liters, it is 0.140 L), and the molarity of HI is 1.0 × 10^-2 M, we can calculate the moles of HI:
Moles of HI = 0.140 L × 1.0 × 10^-2 M
Step 3: Determine the total moles of H+.
To find the total moles of H+, we need to consider that HCl (aqueous) completely dissociates to produce one mole of H+ per mole of HCl, while HI (aqueous) also completely dissociates to produce one mole of H+ per mole of HI.
Total moles of H+ = moles of HCl + moles of HI
Step 4: Calculate the total volume of the solution.
Given that the volume of the HCl solution is 55.0 mL and the volume of the HI solution is 140 mL, the total volume of the solution is:
Total volume = 55.0 mL + 140 mL = 195 mL (converted to liters, it is 0.195 L)
Step 5: Calculate the concentration of H+.
Concentration = moles / volume
Concentration of H+ = total moles of H+ / total volume
Step 6: Calculate the pH.
The pH of a solution can be determined using the equation:
pH = -log[H+]
Substitute the concentration of H+ into the equation to find the pH.
Note: When performing these calculations, make sure to use proper scientific notation and keep track of significant figures to maintain accuracy in the final answer.