To calculate the pH of a solution, we first need to find the concentration of hydronium ions in the solution. Since KOH is a strong base, it dissociates completely in water to produce hydroxide ions (OH-) and potassium ions (K+).
The concentration of hydronium ions in a solution of KOH can be calculated using the concentration of hydroxide ions and the equilibrium constant for water, which is equal to 1.00 x 10^-14 at 25 degrees Celsius.
The concentration of hydroxide ions in a 0.160 M solution of KOH is equal to the concentration of KOH, which is 0.160 M. The concentration of hydronium ions in the solution can be calculated using the equation below:
[H3O+] = (1.00 x 10^-14) / [OH-]
Substituting the concentration of hydroxide ions into the equation above, we get:
[H3O+] = (1.00 x 10^-14) / (0.160 M) = 6.25 x 10^-13 M
To calculate the pH of the solution, we need to take the negative logarithm of the concentration of hydronium ions. This can be done using the equation below:
pH = -log([H3O+])
Substituting the concentration of hydronium ions into the equation above, we get:
pH = -log(6.25 x 10^-13) = 12.20
The pH of a 0.160 M solution of KOH is 12.20.
To calculate the pOH of a solution, we first need to find the concentration of hydroxide ions in the solution. Since we already calculated this value above, we can simply use the concentration of hydroxide ions we found earlier: 0.160 M.
To calculate the pOH of the solution, we need to take the negative logarithm of the concentration of hydroxide ions. This can be done using the equation below:
pOH = -log([OH-])
Substituting the concentration of hydroxide ions into the equation above, we get:
pOH = -log(0.160 M) = 1.80
The pOH of a 0.160 M solution of KOH is 1.80.
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. This is the definition of density. If you rearrange this equation by multiplying each side of the equation by the volume, you get: (Density)(Volume)=Mass. Divide each side by the density to get: Volume=Mass/Density. Now just plug everything in: