Calculate the pH and of aqueous solutions having the fol lowing ion concentrations
a. [H^ + ]=1.0*10^ -14 M
b. [OH^ - ]=5.6*10^ -8
C. [H^ + ]=2.7*10^ -3 M
d. [OH^ - ]=0.061M
pH = -log(H^+) for a and c.
pOH = -log(OH^-), then substitute into next eqn to solve for pH.
pH + pOH = pKw = 14 for b and d.
pH = - log[H+] ... pOH = - log[OH-] ... pH + pOH = 14
use a calculator to find the logs of the given concentrations
To calculate the pH and pOH of aqueous solutions with the given ion concentrations, you need to use the following formulas:
pH = -log[H+]
pOH = -log[OH-]
For each case, we will plug in the given ion concentration into the respective formula.
a. [H+] = 1.0*10^-14 M
Using the formula, pH = -log(1.0*10^-14), calculate:
pH = -(-14) = 14
b. [OH-] = 5.6*10^-8 M
Using the formula, pOH = -log(5.6*10^-8), calculate:
pOH = -(-7.25) = 7.25
c. [H+] = 2.7*10^-3 M
Using the formula, pH = -log(2.7*10^-3), calculate:
pH ≈ 2.57
d. [OH-] = 0.061 M
Using the formula, pOH = -log(0.061), calculate:
pOH ≈ -(-1.214) = 1.214
Remember, pH and pOH are logarithmic scales that measure the concentration of hydrogen ions (H+) and hydroxide ions (OH-) in a solution, respectively. The pH scale ranges from 0 to 14, with a pH of 7 considered neutral, pH less than 7 considered acidic, and pH greater than 7 considered basic. Similarly, the pOH scale ranges from 0 to 14, with a pOH of 7 considered neutral, pOH less than 7 considered basic, and pOH greater than 7 considered acidic.