The pH of a solution is measured to be 5.4. Calculate the following:
a) [H3O^+]
b)pOH
c)[OH^-]
a) Well, let's see. The pH of a solution is simply a measure of how acidic or basic it is. In this case, a pH of 5.4 indicates that the solution is slightly acidic. Since pH is just the negative logarithm of the hydrogen ion concentration ([H3O+]), we can calculate it using some mathematical magic. So, to find [H3O+], we can do 10 raised to the power of -pH. Let me do the calculations here... *tap-tap-tap* and we get 3.98 x 10^-6 M. Voila!
b) Ah, pOH, my old friend. The pOH is simply the negative logarithm of the hydroxide ion concentration ([OH-]). But don't worry, it's a breeze to find once we know the pH. To calculate it, we can use this fun little formula: pOH = 14 - pH. So, plugging in the value of pH as 5.4, we subtract that from 14 and get... *drumroll* 8.6!
c) Now, to find the hydroxide ion concentration ([OH-]), we can use yet another magical formula. We take 10 raised to the power of -pOH, which in this case is 8.6. So hang on tight, let me do my calculations... *poof-poof* and we end up with [OH-] as 2.51 x 10^-9 M.
So, there you have it! [H3O+] is 3.98 x 10^-6 M, pOH is 8.6, and [OH-] is 2.51 x 10^-9 M. Hope that tickles your funny bone!
To calculate the following values, we need to use the equations:
pH + pOH = 14
[H3O^+] = 10^(-pH)
[OH^-] = 10^(-pOH)
a) [H3O^+]
The concentration of hydronium ions can be calculated using the equation [H3O^+] = 10^(-pH).
Substituting the given pH value of 5.4 into the equation:
[H3O^+] = 10^(-5.4)
[H3O^+] = 2.51 x 10^(-6) or 0.00000251 mol/L
b) pOH
The pOH value can be determined using the equation pH + pOH = 14.
Rearranging the equation:
pOH = 14 - pH
pOH = 14 - 5.4
pOH = 8.6
c) [OH^-]
The concentration of hydroxide ions can be calculated using the equation [OH^-] = 10^(-pOH).
Substituting the pOH value of 8.6 into the equation:
[OH^-] = 10^(-8.6)
[OH^-] = 2.51 x 10^(-9) or 0.00000000251 mol/L
Therefore:
a) [H3O^+] = 2.51 x 10^(-6) or 0.00000251 mol/L
b) pOH = 8.6
c) [OH^-] = 2.51 x 10^(-9) or 0.00000000251 mol/L
To answer these questions, we can use the principles of acid-base chemistry and the concept of pH. The pH scale is a logarithmic scale used to measure the acidity or alkalinity of a solution. The pH of a solution can be calculated using the formula:
pH = -log[H3O+]
where [H3O+] represents the concentration of hydronium ions in the solution.
a) [H3O+]:
To calculate the concentration of hydronium ions, we need to rearrange the formula:
[H3O+] = 10^(-pH)
Substituting the given pH value of 5.4 into the formula:
[H3O+] = 10^(-5.4)
[H3O+] ≈ 3.98 x 10^(-6) M
Therefore, the concentration of hydronium ions in the solution is approximately 3.98 x 10^(-6) M.
b) pOH:
The pOH of a solution can be calculated by using the formula:
pOH = 14 - pH
Substituting the given pH value of 5.4 into the formula:
pOH = 14 - 5.4
pOH ≈ 8.6
Therefore, the pOH of the solution is approximately 8.6.
c) [OH-]:
To calculate the concentration of hydroxide ions, we can use the relationship:
[H3O+] x [OH-] = 1.00 x 10^(-14) M^2
Rearranging the formula to solve for [OH-]:
[OH-] = 1.00 x 10^(-14) M^2 / [H3O+]
[OH-] = 1.00 x 10^(-14) M^2 / (3.98 x 10^(-6) M)
[OH-] ≈ 2.51 x 10^(-9) M
Therefore, the concentration of hydroxide ions in the solution is approximately 2.51 x 10^(-9) M.
pH = -log(H^+) will give you H^+.
pH + pOH = 14 will give you pOH.
pOH = -log(OH^-) will give you OH^-.