Question

if 10.0 ml of 0.20 m naoh is added to 50.0 ml of 0.10 m hcl, what will be the ph of the resulting solution?

Answer 1

The pH of the resulting solution can be calculated using the concept of acid-base titration. When NaOH is added to HCl, they react to form NaCl and water. The molar ratios between NaOH and HCl can be used to determine the final concentration of HCl. Once we know the final concentration of HCl, we can calculate the pH using the equation for the pH of a strong acid.

Step-by-step explanation:

The ph of the resulting solution can be calculated using the concept of acid-base titration. When NaOH is added to HCl, they react to form NaCl and water. The molar ratios between NaOH and HCl can be used to determine the final concentration of HCl. In this case, the final volume of the solution will be 60.0 mL (50.0 mL + 10.0 mL).

To calculate the final concentration of HCl, we can use the equation:

moles of HCl = moles of NaOH

Molarity x Volume = Molarity x Volume

0.10 M x 50.0 mL = C x 60.0 mL

From this equation, we can solve for C which is the final concentration of HCl. Once we know the final concentration of HCl, we can calculate the pH using the equation for the pH of a strong acid:

pH = -log[H+]

Where [H+] is the concentration of H+ ions in the solution. Since HCl is a strong acid, it completely dissociates in water, so the concentration of H+ ions is equal to the concentration of HCl.

So, plugging in the final concentration of HCl into the pH equation, we can calculate the pH of the resulting solution.

Answer 2

pH= 7.00

Step-by-step explanation:

Keep in mind that the volume of the solution changes during this titration, so to compute the amount of hydronium that is neutralized during this addition of base (in order to calculate the final pH of the solution), we must calculate the moles of all species in solution initially present. Because both NaOH and HCl ionize completely:

initial mol OH−=mol NaOH=(0.010 L)(0.50 molL)=0.0050 mol OH−

initial mol H3O+=mol HCl=(0.050 L)(0.10 molL)=0.0050 mol H3O+

Notice that the moles (and, consequently, the concentrations) of hydronium and hydroxide in solution are exactly equal: this means we are done! If [H3O+]=[OH−], the solution is perfectly neutral, with a pH of exactly 7.00.