What is the pH of a 0.050 M HClO(aq) solution? Ka,HClO = 4.0 × 10−8 M.
What is the pH of a 0.050 M HClO(aq) solution? Ka,HClO = 4.0 × 10−8 M.
HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.036 M in NaClO at 25 °C?
What is the pH of a 0.10 M NaClO solution if Ka for HClO is 3.0 x 10^-8?
Determine the PH and [h3o+] in a .265 M HClO solution. The Ka of HClO is 2.9x10^-8
Determine pH, pOH, [H3O+] and [OH-] of a 0.265 M HClO solution. Ka of HClO is 2.9 x 10-8.
what is the approximate pH of a solution labeled 0.050 M HClO? I realized my mistake on my last post but this isnt a strong acid nor a strong base so how do i solve this?
A solution of 0.357 M HClO (Ka = 3.5 x 10-8) with volume 75. mL is mixed with 50. mL of a 0.800 M KOH solution. What is the final pH?
The pH of a 1.50 M solution of HClO is 3.67. a. Calculate the Ka of HClO. (6 pts)
Calculate the pH for each case in the titration of 50.0 mL of 0.230 M HClO(aq)0.230 M HClO(aq) with 0.230 M KOH(aq).0.230 M KOH(aq). Use the ionization constant 4.0×10–8 for HClO. What is the pH after the addition of 50.0 mL KOH?
Given that Ka for HClO is 4.0 × 10-8 at 25 °C, what is the value of Kb for ClO– at 25 °C? Given that Kb for (CH3)2NH is 5.4 × 10-4 at 25 °C, what is the value of Ka for (CH3)2NH2 at 25 °C?
Find the initial concentration of a solution of HClO with pH=4.28 and Ka= 3.0 x 10-8. ( include ICE chart if possible)