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 the final pH of this solution?
A a 50.00-mL sample of bleach solution contains 0.289 M HClO and 0.602 M NaClO. The...
A a 50.00-ml sample of bleach solution contains 0.233 M HClO and 0.499 M Nacio. The K, of hypochlorous acid is 3.0 x 10-8 Find the pH of the solution. C 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...
(a) What is the pH of a solution that contains 0.100 M HClO and 0.300 M KClO? (b) If 50.00 mL of 0.100 M HCl is added to 1.00 L of the above buffer, what is the new pH? (b) If 50.00 mL of 0.100 M HCl is added to 1.00 L of the above buffer, what is the new pH?
A solution was prepared by dissolving 0.200 moles of sodium hypoch lorite (NaClO) in water to a final volume of 1.00 Liter. Ka 2.96x10 for hypochlorous acid (HCIO). Show equations and work steps for these calculations. 1) Calculate Kb of sodium hypochlorite. 2) Calculate the pH of the NaClO solution. 3) Calculate the pH if 10.0 mL of 1.00 M HCl is added to 100.0 mL of the original NACIO solution. 4) Calculate the pH if 20.0 mL of 1.00...
You are given a 100.0 mL buffer that is 0.50 M HClO and 0.76 M in NaClO (Ka for HClO= 3.5x10^-8). What would the pH of the buffer solution change to if we added 10.0 mL 1.00 M HCl?
A 30.0 mL sample of 0.200 M hypochlorous acid (HClO; Ka = 3.0 x 10-8) is titrated with 0.100 M KOH. Calculate the pH after the following volumes have been added 0.0mL 15.0 mL 30.0 mL 45.0 mL 60.0 mL
A buffer solution contains 0.100 mol of HCIO and 0.100 mol of NaClO in 1.00 L. What is the pH of this buffer after 0.010 mol of NaOH are added? HCIO has a Ka = 3.0 x 10-8 07.61 8.47 7.52 O 6.57 7.43
Consider the following two buffers: (i) 10.0 mL of a buffer that contains 0.10 M HClO and 0.10 M NaClO (ii) 10.0mL of a buffer that contains 0.050 M HClO and 0.10 M NaClO b.) 8 drops of 1.0 M NaOH (aq) is added to each of these buffers. 1.)Give the balanced net-ionic equation for the reaction that occurs when the NaOH (aq) is added. 2.)For which buffer (i or ii) does the pH change the greatest amount when the...
A 0.200 M solution of NaClO prepared by dissolving NaClO in water. A 55.0 mL sample of this solution is titrated with 0.200 M HCl.K_a for HClO is 3.5 times 10^-8. Calculate the pH of the solution at each of the following points of the titration: a. Prior to the addition of any HCl b. Halfway to the equivalence point c. At the equivalence point d. After 6.00 mL of HCl has been added beyond the equivalence point
A scientist is performing a titration of HClO in bleach samples (10.00 mL aliquot) with 0.0500 M NaOH. She does the initial titration with a pH meter, and it is found to take 32.1 mL of base to reach the endpoint, which shows a pH of 10.07. She now wants to prepare a buffered reference solution with the same pH and same ionic strength as the titration solution at the equivalence point (so the titration can be done routinely without the need...
What is the pH of a 0.10 M NaClO solution if Ka for HClO is 3.0 x 10^-8?