What is the pH of a 0.10 M NaClO solution if Ka for HClO is 3.0 x 10^-8?
Calculate the pH for 0.50 M solution of the salt NaClO. The Ka for HClO is 3.0x10^-8
What is the pH of a 0.255 M aqueous solution of sodium hypochlorite, NaClO? (Ka for HClO = 3.5×10-8)
a. A buffer solution is 0.480 M in HClO and 0.367 M in NaClO . If Ka for HClO is 3.5×10-8 , what is the pH of this buffer solution? b. A buffer solution is 0.481 M in H2S and 0.294 M in NaHS. If Ka1 for H2S is 1.0x10^-7, what is the pH of this buffer solution?
What is the pH of a 0.025 M solution of HClO? The Ka for HClO is 3.5 x 10-8. 4.16 2.89 3.18 5.27 4.53
Determine the hypochlorite concertration for a solution of NaClO that has pH of 8.00. HClO ka=2.95*10^-8
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 0.014 M in NaClO at 25 °C?
A buffer solution is made that is 0.319 M in HClO and 0.319 M in NaClO . (1) If Ka for HClO is 3.50×10-8, what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.089 mol KOH is added to 1.00 L of the buffer solution.
A a 50.00-mL sample of bleach solution contains 0.289 M HClO and 0.602 M NaClO. The Ka of hypochlorous acid is 3.0 ✕ 10−8. Find the pH of the solution. The solution is then divided in half. A) To one half of the original solution, 10.00 mL of 0.100 M NaOH is added. What is the final pH of this solution? B) To the other half of the original solution, 1.00 mL of 0.100 M HCl is added. What is...
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?
HClO is a weak acid (Ka= 4.0x10^-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?