Question 23
1 Point
What is the pH of 0.00187 M HCl? (HCl is a strong acid) BLANK-1 (give your answer to 3 significant figures)
Question 23 1 Point What is the pH of 0.00187 M HCl? (HCl is a strong...
Question 24 1 Point What is the pH of 1.94 x 10-5 M NaOH? (NaOH is a strong base) BLANK-1 (give your answer to 3 significant figures) BLANK-1
Question 17 (1 point) What is the pH of stomach acid in which [HCl] = 0.151 M? Enter your answer with no units to the correct number of significant figures. Your Answer Answer Save ch
QUESTION 2 The strong acid, HCl, is titrated with a strong base, NaOH, in aqueous solution. What is the pH of the titration solution after the addition of 17.94 mL of 0.100 M NaOH to a 50.00 mL of 0.100 M HCI? Write your answer using 3 significant figures,
QUESTION 2 Suppose you have 20 mL of 0.1 M HCl. What will the pH of the solution be after 10 mL of 0.1 M NaOH is added? Report your answer to 2 significant figures (i.e., 2 decimal places). Suppose you have 20 mL of 0.1 M HCl. What will the pH of the solution be after 30 mL of 0.1 M NaOH is added? Report your answer to 2 significant figures (i.e., 2 decimal places).
PRE-LAB for pH titration of a Strong Acid with Base This is due before the lab begins, Name 1. Calculate the pH of the following solutions: (a) 1 M NaCl Does not dissociate in water to produce either hydrogen or nyot thus it is a neutral Sall, so 7. (b) 1 M HOAc (Ka - 1.8 x 10-5) duce either hydrogen or hyd xde ion, (c) 1 M NHOH (Kb = 1.8 x 10-5) (d) 0.1 M NaOAC (e) 0.1...
Titration of 25.00 mL of 0.100 M HCl with 0.100 M NaOH (strong acid, strong base): Answer the following questions: 4. Calculate the initial pH 5 Why is pH = 7 at the equivalence point? 6Why does the pH rise slowly at first, very rapidly near the equivalence point, and slowly after the equivalence point? 7. Why does it require 25.00 mL of NaOH to reach the equivalence point?
Calculate the pH of each of the following strong acid solutions. (a) 0.00851 M HCl pH = (b) 0.714 g of HNO3 in 18.0 L of solution pH = (c) 62.0 mL of 4.90 M HCl diluted to 3.00 L pH = (d) a mixture formed by adding 55.0 mL of 0.00326 M HCl to 46.0 mL of 0.00896 M HNO3 pH =
1. Using a 0.20 M phosphate buffer with a pH of 6.7, you add 0.79 mL of 0.53 M HCl to 40. mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) 2. Using a 0.20 M phosphate buffer with a pH of 6.7, you add 0.79 mL of 0.53 M NaOH to 40. mL of the buffer. What is the new pH of the solution? (Enter your answer to three...
1) Using a 0.25 M phosphate buffer with a pH of 7.2, you add 0.79 mL of 0.48 M HCl to 54 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) 2) Using a 0.25 M phosphate buffer with a pH of 7.2, you add 0.79 mL of 0.48 M NaOH to 54 mL of the buffer. What is the new pH of the solution? (Enter your answer to three...
If you mix 100.0 mL of 0.125 M HCl (strong acid) with 50.0 mL of 0.175 M NaOH (strong base) what will be the pH of the resulting solution? Have you reached the endpoint of the reaction (circle your answer)? YES NO Explain your answer: