A 1-L unbuffered solution needs the pH adjusted from 4.5 to 2.5. How many mL of 12 molar HCl solution need to be added to reduce the pH?
Report your answer using exponential notation to two decimal places! For example 100 would be 1E2, or 0.001 would be 1e-3
For this question, assume the volume of HCl being added is negligible and the total volume of the solution does not change.
A 1-L unbuffered solution needs the pH adjusted from 4.5 to 2.5. How many mL of...
A 0.5-L unbuffered solution needs the pH adjusted from 6 to 3. How many microliters of a 2 molar HCl solution need to be added to adjust the pH? Report your answer to four decimal places. For this question: Assume the volume of HCl being added is negligible and the total volume of the solution does not change. The volume of the solution is *not* 1 L like it was in the practice pools. The question requests your answer be...
QUESTION 44 5 points Save Answer A 0.5-L unbuffered solution needs the pH adjusted from 6.8 to 2.5. How many microliters of a 6 molar HCl solution need to be added to adjust the pH? Report your answer to four decimal places. For this question: • Assume the volume of HCl being added is negligible and the total volume of the solution does not change. • The volume of the solution is *not* 1 L like it was in the...
A 0.5-L unbuffered solution needs the pH adjusted from 4 to 3.5. How many microliters of a 2 molar HCl solution need to be added to adjust the pH? Report your answer to four decimal places.
A 0.5-L unbuffered solution needs the pH adjusted from 6 to 5. How many microliters of a 2 molar HCl solution need to be added to adjust the pH? Report your answer to four decimal places.
How do pH, propionic acid, and propionate change when HCl, a strong acid solution, with a final concentration of 0.0005 mole/L, is added to the solution containing 10-3 M sodium propionate? HCl is added from a concentrated stock solution, so the volume change is negligible.
1.A) A 29.8 mL solution of 0.298 mol L-1 HCl is titrated using 0.173 mol L-1 NaOH.What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment? Remember you can find KA and/or KB values in your textbook in chapter 15. B) A 10.1 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCl. What will be the pH of the solution after 4.07 mL of the HCl solution is added?...
How many mL of 8.5 M NaOH should be added to a 1 L solution of 1 M His at pH 2 to increase the pH to 2.5?
7. a) Calculate the pH of a 0.10 mol l-1-methylamine at 25 ° C. b) How many moles of HCl must be added to 0.25 l of solution (according to a) in order to obtain maximum buffer effect? What is pH? Show the calculations. Disregard volume changes c) as the pH becomes in 1.00 l solution of a) after addition of 0.20 mol HCl then ignoring the volume change?
What is the pH of a solution containing 0.342 mol L-1 NH3 and 0.140 mol L-1NH4? Round your answer to 2 decimal places. Remember you can find KA and/or Kg values in your textbook in chapter 15. Answer: Check A 45.3 mL solution of 0.283 mol L-1 HCl is titrated using 0.820 mol L-'NaOH. What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment? Remember you can find KA and/or Ke values in your...
1.) An aqueous solution contains 0.431 M ethylamine (C2H5NH2). How many mL of 0.368 M hydrobromic acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.400? 2) A buffer solution contains 0.308 M ammonium bromide and 0.319 M ammonia. If 0.0500 moles of perchloric acid are added to 225 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not...