How many moles of HClO are required in a 1.00L solution to create a buffer with a pH of 7.22 if the solution contains 0.39 moles of NaClO?
Ka HClO = 3.0 x 10-8?
How many moles of HClO are required in a 1.00L solution to create a buffer with...
How many moles of NH3 are required in a 1.00L solution to create a buffer with a pH of 8.81 if the solution contains 0.64 moles of NH4Cl? Kb NH3 = 1.8 x 10-5?
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?
A 1.00L buffer solution is formed by adding 0.250 moles of KOH (aq) to 0.300 moles of HA. The Ka for HA = 3.1 x 10-5. A. What is the initial pH of the buffer? B. What will pH be after the addition of 0.0500 moles of H3O+? C. 10ml of a 3.5 M solution of NaOH are added to the buffer. What is the resulting pH?
What is the pH of a 0.10 M NaClO solution if Ka for HClO is 3.0 x 10^-8?
A buffer is prepared by adding 0.250 mol of NaF to 1.00L of 0.100 M HF. Calculate the pH of the resulting solution. Use Ka value of 7.2× 10^4 How many moles of NaOH must be added to this buffer solution to change the pH by 0.38 units?
A 1.0 L buffer mixture contains 0.15 moles of HClO and 0.20 moles of NaClO. Which of the following additions would destroy the buffer (exceeds the buffer capacity)? A. Adding 0.20 moles of NaOH B. Adding 0.15 moles of HCl C. Adding 0.20 moles of NaClO D. None of the above
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?
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 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...
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