Calculate the hydrogen ion concentration, pH, POH, OH‐ in 0.02 H2SO4?
H2SO4 is a strong acid for the first H^+.
k2 = about 0.12 but you should look that up to make sure. I may not have remembered it correctly.
.............H2SO4 ==> H^+ + HSO4^-
I..............0.02............ 0..........0
C............-0.02...........+0.02...+0.02
E..............0..................0.02.....0.02
.............HSO4^- ==> H^+ + SO4^2-
I..................0.02........0.02......0
C..................-x...........+x.........x
E............0.02-x.........0.02+x......x
k1 = about 0.012 = (H^+)(SO4^-2)/(HSO4^-)
Plug in the E line into the k1 expression and solve for x to give you the concentrations of each specie. The you can do pH, pOH, H^+ and OH^-
To calculate the hydrogen ion concentration, pH, pOH, and OH- in 0.02 H2SO4, we need to consider the dissociation of H2SO4.
Step 1: Write the balanced equation for the dissociation of H2SO4:
H2SO4 -> 2H+ + SO4^2-
Step 2: Identify the number of moles of H2SO4:
In this case, the concentration is given as 0.02 H2SO4, which means there are 0.02 moles of H2SO4 in 1 liter of solution.
Step 3: Calculate the hydrogen ion concentration (H+):
Since the H2SO4 dissociates into 2H+, the hydrogen ion concentration is equal to twice the concentration of H2SO4.
Hydrogen ion concentration = 2 * 0.02 = 0.04 M
Step 4: Calculate the pH:
The pH is calculated using the equation:
pH = -log[H+]
pH = -log(0.04)
pH ≈ 1.4
Step 5: Calculate the pOH:
The pOH is calculated using the equation:
pOH = -log[OH-]
Since H2SO4 is a strong acid, it completely dissociates, and the concentration of OH- ions is negligible.
pOH ≈ 0
Step 6: Calculate OH- concentration:
The OH- concentration can be calculated by using the equation:
OH- = 10^(-pOH)
OH- = 10^(-0)
OH- = 1
To summarize:
Hydrogen ion concentration = 0.04 M
pH ≈ 1.4
pOH ≈ 0
OH- = 1
To calculate the hydrogen ion concentration, pH, pOH, and OH- concentration in 0.02 H2SO4, we need to understand the properties of the sulfuric acid (H2SO4) and its dissociation.
Sulfuric acid is a strong acid that dissociates completely in water. Its chemical equation for dissociation is:
H2SO4 -> 2H+ + SO4^2-
To calculate the hydrogen ion concentration ([H+]), we can use the fact that 0.02 mole of H2SO4 dissociates into 0.04 moles of H+. Since the concentration is given in moles per liter (M), we can simply divide the moles of H+ by the volume in liters to obtain the concentration:
[H+] = moles of H+ / volume (in liters)
In this case, the volume is not given, so we will assume it to be 1 liter for simplicity. Therefore, the hydrogen ion concentration can be calculated as follows:
[H+] = 0.04 moles / 1 liter
[H+] = 0.04 M
The pH is a measure of the hydrogen ion concentration and is defined as the negative logarithm (base 10) of the hydrogen ion concentration:
pH = -log10[H+]
To calculate the pH, we can substitute the value of [H+] into the equation:
pH = -log10(0.04)
pH ≈ 1.40
The pOH is the negative logarithm (base 10) of the hydroxide ion concentration ([OH-]). Since the sulfuric acid is a strong acid, we can assume that the concentration of OH- is negligible compared to the concentration of H+ ions. Therefore, we can ignore the contribution of OH- concentration.
Finally, to calculate the OH- concentration, we can use the fact that water undergoes autoionization to produce equal amounts of H+ and OH- ions. At 25°C, the concentration of H+ and OH- ions in pure water is 1x10^-7 M. However, in the presence of a strong acid like sulfuric acid, the concentration of H+ ions is significantly higher than 1x10^-7 M, while the concentration of OH- ions decreases.
Therefore, in 0.02 H2SO4, we can assume that the OH- concentration is negligible compared to the H+ concentration.
To summarize:
- Hydrogen ion concentration ([H+]) = 0.04 M
- pH ≈ 1.40
- pOH is not calculated in this case since we assume negligible OH- concentration.
- The OH- concentration is negligible.