Given 100.0 mL of a buffer that is 0.50 M in HOCl and 0.74 M in NaOCl, what is the pH after 10.0 mL of 1.0 M NaOH has been added? (Ka for HOCl = 3.5 × 10–8)
Select one:
a. 7.78
b. 7.46
c. 7.72
d. 7.66
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
1.) 1.0 L of a buffer solution was made with 0.15M in HOCl (Ka = 3.5 × 10-8) and 0.25M NaOCl. If 10.0 mL of 5.0M HCl are added into the solution, what would be the pH? a. 7.23 b. 6.15 c. 6.98 d. 7.46 e. 7.93
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?
2. A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer? A) 3.67 B) 3.78 C) 3.81 D) 3.85 E) 3.95 A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M Nalcoo. What is the pH of this buffer? Ka = 1.7 * 104 A) 2.87...
How many moles of NaOCl must be added to 150 mL of 0.025 M HOCl to obtain a buffer solution with a pH = 7.50? Ka= 2.8×10-8 for HOCl. The answer is 3.3x10-3
5. Calculate the grams of NaCH3COO required for 100.0 mL of 0.20 M CH3COOH solution to achieve a pH of 4.40. (Assume no volume change.) K = 1.8 x 10-5 6. What is the pH of 100.0 mL of buffer consisting of 0.20 M CH3COOH/0.20 M NaCH3COO after 10.0 mL of 0.20 M HC1 was added into the solution ? Kg = 1.8 x 10-5 7. The pH of a sodium acetate-acetic acid buffer is 4.80. Calculate the ratio of...
A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer? (Assume the addition cause negligible volume change.)
Calculate the following: a. The pH of a 500.0 mL buffer solution containing 0.75 M HCN (Ka = 6.2 x 10^-10) and 0.55 M NaCN b. The pH of the above buffer after the addition of 100.0 mL of 1.0 M NaOH. c. The pH of the buffer if 100.0 mL of 1.0 M HCl was added to the solution in part a.
Using a 0.25 M phosphate buffer with a pH of 7.2, you add 0.74 mL of 0.50 M NaOH to 54 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
consider 100.0 ml of a buffer solution that contains [NaCH3COO]=[CH3COOH]=0.250 M a) what is the pH of this buffer? b) what should the ph of the buffer be after 50.0ml of water is added? explain c) wtite balanced net ionic for the reaction that occurs whrn 1.0 M HCl ir added to this buffer. d) after adding 10.0 ml of 1.0 M HCl what will the ph of the solution be? e) as more 1.0 M HCl is slowly added...
Given 100. mL of each of the three aqueous buffer solutions: Buffer A is 0.50 M in ammonia and 0.10 M in ammonium chloride; Buffer B is 0.50 M in ammonia and 0.50 M in ammonium chloride; and Buffer C is 0.50 M in ammonia and 1.0 M in ammonium chloride. To each of the 100. mL samples is added 1.0 mL of 6.0 M hydrochloric acid. Which buffer solution will show the smallest change in pH? Explain why.