What is the pH of sodium hydroxide (NaOH) 0.5N
conc of OH=.5 moles/liter
p(h)=14-p(OH)=14-log(.5)=13.7
To determine the pH of a solution of sodium hydroxide (NaOH) 0.5N, you need to consider the basic nature of the compound. Sodium hydroxide is a strong base that dissociates completely in water to produce sodium ions (Na+) and hydroxide ions (OH-).
To find the pH, you can use the fact that the pH of a basic solution is equal to the negative logarithm (base 10) of the concentration of the hydrogen ion (H+). In this case, since sodium hydroxide is a strong base, you have an excess of hydroxide ions (OH-) instead of hydrogen ions (H+). Therefore, you need to calculate the pOH first and then convert it to pH.
The pOH is calculated as the negative logarithm (base 10) of the hydroxide ion concentration (OH-). In this case, the hydroxide ion concentration can be determined by multiplying the concentration of sodium hydroxide by the number of hydroxide ions produced during dissociation. As NaOH is a strong base, it completely dissociates into one sodium ion (Na+) and one hydroxide ion (OH-) per molecule.
So, to calculate the hydroxide ion concentration, you can use the formula:
OH- concentration (in moles per liter) = NaOH concentration (in moles per liter) × number of hydroxide ions produced during dissociation
In this case, the concentration of NaOH is given as 0.5N, which means 0.5 moles per liter. Since NaOH produces one hydroxide ion (OH-) per molecule, the hydroxide ion concentration is also 0.5N.
Now that you have the hydroxide ion concentration (0.5N), you can calculate the pOH using the formula:
pOH = -log10(OH- concentration)
pOH = -log10(0.5)
Using a logarithm calculator or manually calculating it, pOH is approximately 0.301.
To convert pOH to pH, you can use the formula:
pH = 14 - pOH
pH = 14 - 0.301
Using a calculator, the pH of sodium hydroxide 0.5N is approximately 13.699.
Therefore, the pH of a sodium hydroxide (NaOH) 0.5N solution is approximately 13.699.