what is the pH of a NaOH solution whose concentraiton is 4.5 * 10^-5 M.
HOW WOULD I DO THIS PROBLEM??
NaOH ==>Na^+ + OH^-
The trick is to know that NaOH is a strong base; i.e., it is ionized in water solution 100%. Therefore, (NaOH) = (OH^-)
So (OH^-) = 4.5 x 10^-5 M
Change that to pOH, and subtract from 14.
pH about 9.6 or so.
To find the pH of a NaOH solution with a concentration of 4.5 * 10^-5 M, you need to follow these steps:
Step 1: Recall that NaOH is a strong base that dissociates completely in water.
Step 2: Write the balanced chemical equation for the dissociation of NaOH in water:
NaOH → Na+ + OH-
Step 3: Determine the concentration of hydroxide ions (OH-) in the solution. In this case, since NaOH dissociates completely, the concentration of hydroxide ions will be the same as the concentration of NaOH, which is 4.5 * 10^-5 M.
Step 4: Recall that pH is a measure of the concentration of hydrogen ions (H+) in a solution. Since we are dealing with a strong base, which produces hydroxide ions (OH-), we can use the pOH scale to find the concentration of hydrogen ions.
Step 5: Calculate the pOH using the formula: pOH = -log[OH-]. In this case, pOH = -log(4.5 * 10^-5).
Step 6: Subtract the pOH from 14 to find the pH of the solution. pH = 14 - pOH.
Following these steps, you can calculate the pH of the NaOH solution whose concentration is 4.5 * 10^-5 M.