What is the pH, pOH, [H+] and [OH-] for a solution that contains 5.25 x 10^-3 moles of HCl dissolved in 3.25 L of water?
I was gone the day my teacher explained this and I'm completely lost on what to do.
An outline of steps needed to solve the problem would be helpful. Please do not provide the solution, as I would like to solve it for myself first.
M HCl = mols/L solution = ?
M H^+ = M HCl since HCl is a strong acid and ionizes 100%.
pH = -log (H^+)
pH + pOH = pKw = 14 allows you to calculate pOH after you know pH then
pOH = -log(OH^-) gives you OH^-
Alternatively, after you know (H^+), you can use (H^+)(OH^-) = Kw = 1E-14 to solve for OH^-
[H3O+] = 5.25 x 10-3M:
Sure! I can guide you through the steps to solve this problem. Here's an outline of what you need to do:
1. Write down the balanced chemical equation for the dissociation of HCl in water. This will help you determine the ratio of H+ ions to HCl moles.
2. Calculate the molarity of the HCl solution by dividing the moles of HCl by the volume of the solution in liters.
3. Use the molarity of HCl to calculate the concentration of H+ ions. Since HCl is a strong acid, it completely dissociates into H+ and Cl- ions in water.
4. Calculate the pOH of the solution. Remember that pOH is the negative logarithm of the hydroxide ion concentration. Since water is neutral, the concentration of OH- ions is equal to the concentration of H+ ions.
5. Finally, calculate the pH of the solution by subtracting the pOH from 14, as pH + pOH = 14.
Remember to use the correct formulas and units throughout the calculations. Let me know if you want me to go into more detail on any of the steps!
To solve this problem, you need to understand the basics of pH, pOH, and the relationship between hydrogen ion concentration ([H+]) and hydroxide ion concentration ([OH-]). Here is an outline of the steps you can follow to solve this problem:
1. Identify the given information:
- Moles of HCl: 5.25 x 10^-3 moles
- Volume of water: 3.25 L
2. Calculate the molarity of HCl:
- Molarity (M) = moles of solute / volume of solution in liters
- Divide the moles of HCl by the volume of water to obtain the molarity.
3. Determine the [H+] concentration:
- Since HCl is a strong acid, it ionizes fully in water, producing one mole of H+ for every mole of HCl.
- The [H+] concentration will be equal to the molarity of the HCl solution.
4. Calculate the pH:
- The pH is a measure of the acidity of a solution and is defined as the negative logarithm (base 10) of the [H+] concentration.
- Use the [H+] concentration calculated earlier and apply the pH formula: pH = -log[H+].
5. Calculate the pOH:
- The pOH is the negative logarithm (base 10) of the hydroxide ion concentration ([OH-]).
- Since water dissociates into equal amounts of H+ and OH-, the [H+] and [OH-] concentrations are equal.
- Therefore, the [OH-] concentration will also be the same as the [H+] concentration calculated earlier.
- Use the pOH formula: pOH = -log[OH-].
6. Calculate the [OH-] concentration:
- Since [H+] and [OH-] concentrations are equal, use the [H+] concentration calculated earlier as the [OH-] concentration.
Keep in mind that these steps assume that water does not contribute significantly to the ion concentration. Also, make sure to properly use logarithms and understand the logarithm properties when performing calculations.