75 mL of 0.50 M solution of NaOH is titrated with a 0.50 M solution of HCl. Calculate the initial...
Question:
75 mL of 0.50 M solution of NaOH is titrated with a 0.50 M solution of HCl. Calculate the initial pH.
Acid-Base Titration:
The procedure of identifying an unknown acid/base concentration by titrating it with an acid/base of known concentration is called acid-base titration. Indicators are used to recognize the endpoint of the titration.
Answer and Explanation:
Become a Study.com member to unlock this answer! Create your account
View this answerHere, 75 mL of 0.50 M NaOH solution is titrated with HCl. We have to determine the initial pH of the NaOH solution.
NaOH dissociates completely in the...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Titrations with Weak Acids or Weak Bases
from
Chapter 11 / Lesson 10
20K
Learn about titrations of weak acids and strong bases, strong acids and weak bases, and weak acids and weak bases. Explore types of titration curves and the pH.
Related to this Question
- 35 mL of a 0.20 M solution of HI is titrated with a 0.20 M solution of NaOH. Calculate the initial pH.
- 35 mL of a 0.15 M solution of HN_3 is titrated with a 0.15 M solution of NaOH. Calculate the initial pH.
- Given 100.0 mL of a 0.100 M solution of H3A . Calculate the pH of the solution after 10.0 mL of 1.00 M NaOH has been added to the original solution.
- 120 mL of a 0.75 M solution of H_2NNH_2 is titrated with a 0.75 M solution of HCl. Calculate the initial pH.
- Calculate the pH of a solution of 20 ml of 0.2 M HBr that has been titrated with 19.9 ml of 0.2 M NaOH.
- Calculate the pH of the solution when 20.00 mL of 0.10 M CH3CO2H (Ka= 1.76 x 10^-5) has been titrated with 20.00 mL of 0.10 M NaOH.
- 25 ml of a solution of 0.1 M acetic acid (K_a=1.5 \times 10^{-5}) is titrated with a 0.05 M NaOH. a) Calculate the initial pH . b) Calculate the pH after adding 25 ml of NaOH .
- Determine the pH of a solution after 20.00 mL of 0.4963 M HI has been titrated with 12.64 mL of 0.5174 M NaOH.
- Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1= 1.0 x 10-6, Ka2= 1.0 x 10-10) is titrated with the following volume of 1.00 M NaOH: 250.0 mL of 1.00 M NaOH.
- Consider 100.0 mL of a 0.100 M solution of H3A. Calculate the pH of the solution after 25.0 mL of 1.00 M NaOH has been added to the original solution.
- 12. Calculate the pH during the titration of 100.0 mL of 0.200 M HCI with 0.400 M NaOH. First what is the initial pH (before any NaOH is added)? 13. What is the pH after 31.5 mL of NaOH are added? 1
- A titration is performed on 50mL of a 0.10 M solution of HN3 (Ka + 1.9 x 10^{-5}) with 0.10 M NaOH as the titrant. (a) What is the initial pH of the HN3 solution? (b) Calculate the pH of the solution after 25 ml of NaOH have been added. (c) How many mL
- Calculate the pH of a solution made by adding 1.0 mL of 3.0 M NaOH to 50.0 mL of l.0 * 10^-3 M HCl.
- For each solution, calculate the initial and final pH after adding 0.01 mol of NaOH a. 250.0 ml of pure water.
- Calculate the pH of the solution when 25.0 mL of 0.0920 M HCl is titrated with 0.15 mL, 23.0 mL, and 30.0 mL of 0.10 M NaOH.
- Calculate the pH during the titration of 100.0 mL of 0.200 M HCl with 0.400 M NaOH. First what is the initial pH (before any NaOH is added)? . 1. What is the pH after 32.6 mL of NaOH are added?
- a.) Calculate the pH during the titration of 100.0 mL of 0.200 M HCl with 0.400 M NaOH. First what is the initial pH (before any NaOH is added)? b.) What is the pH after 31.9 mL of NaOH are added? c.)
- For a 300.0 mL solution of pure water, calculate the initial pH and the final pH after adding 0.005 moles of NaOH.
- Calculate the pH of the resulting solution if 18.0 mL of 0.180 M HCl (aq) is added to 28.0 mL of 0.230 M NaOH (aq).
- Calculate the pH of the resulting solution if 33.0 mL of 0.330 M HCl (aq) is added to (a) 43.0 mL of 0.330 M NaOH (aq). (b) 23.0 mL of 0.430 M NaOH (aq).
- For the following solution, calculate the initial pH and the final pH after adding 0.010 mol of NaOH . 270.0 mL of a buffer solution that is 0.215 M in HCHO2 and 0.280 M in KCHO2.
- For the following solution, calculate the initial pH and the final pH after adding 0.010 mol of NaOH. 300.0 mL of a buffer solution that is 0.320 M in C H 3 C H 2 N H 2 and 0.300 M in C H 3 C H 2 N
- Calculate the pH of a solution containing 0.20 g of NaOH in 2.00 mL of solution.
- For 300.0 mL of pure water, calculate the initial pH and the final pH after adding 0.005 mol of NaOH.
- For 270.0 mL of pure water, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.
- Determine the pH if 2.63 g of NaOH is dissolved in 156 mL of solution.
- Calculate the pH during the titration of 100.0 mL of 0.200 M HCI with 0.400 M NaOH. First what is the initial pH (before any NaOH is added)? What is the pH after 28.0 mL of NaOH are added? What is th
- Determine the pH of a solution in which 35 mL of 0.01M NaOH has been added to 15 mL of 0.02M HCl. 1. pH = 13.7 \\2. pH = 13.3 \\3. pH = 8 \\4. pH = 11 \\5. pH = 2.54 \\6. pH = 13 \\7. pH = 12.5
- A 20 ml sample of 0.150 HNO3 is titrated with 0.150 NaOH. Calculate the initial pH and calculate the pH after the addition of 15.0 mL of the NaOH.
- Determine the pH of the solution when 27.8 mL of 0.12 M HNO3 is mixed with 21.4 mL of 0.100 M NaOH.
- Calculate the pH of the solution after the addition of 12.31 mL of 0.1654 M HBr to 25.00 mL of 0.1996 M NaOH.
- Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 times 10^{-10}) solution.
- Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 x 10^-10) solution. A) 5.85 B) 9.91 C) 8.71 D) 13.0 E) 5.15
- Calculate the pH of a 400.0-mL solution with a concentration of 0.75 M NaOH.
- Calculate the pH of the solution when 40 mL of 0.1M HCl reacts with 0.1M NaOH solution after 23 mL of base is added.
- Calculate the pH of the solution when 40 mL of 0.1M HCl reacts with 0.1M NaOH solution after 51 mL of base is added.
- Calculate the pH of the solution when 40 mL of 0.1M HCl reacts with 0.1M NaOH solution after 39.7 mL of base is added.
- Calculate the pH of a solution made by adding 1mL of 6M NaOH to 3 mL of water.
- Calculate the initial pH and the final pH after adding 0.005 mol of NaOH.
- 1. A 25.00 mL sample of 0.260 M NaOH analyte was titrated with 0.750 M HCl at 25 C. Calculate the initial pH before any titrant was added. pH= Calculate the pH of the solution after 5.00 mL of the
- A 1-mL solution of 0.1 M NaOH is diluted to 1 L at 25�C. What is the pH of the resulting solution?
- What is the pH of a solution of 20.00 mL of 3.00 M HCl that is titrated with 10.00 mL of a 6.00 M solution of NaOH?
- Calculate the pH of the solution after combining 10.0 mL of 0.30 M HCl and 15.0 mL of 0.30 M NaOH.
- 35 mL of a 0.20 M solution of HI is titrated with a 0.20 M solution of NaOH. The pH when 10.0, 20.0, 30.0, 40.0, 50.0, and 60.0 mL of 0.20 M NaOH is added.
- Calculate the pH during the titration of 40.00 mL of 0.1000 M HCI with 0.1000 M NaOH solution after the following additions of base: (a) 30.00 mL pH = ________. (b) 39.10 mL pH = __
- Determine the pH of a solution made by mixing 27 mL of 0.18 M HCl with 15 mL of 0.35 M NaOH.
- For 250.0 mL of a buffer solution that is 0.3187 M in CH_3CH_2NH_2 and 0.2987 M in CH_3CH_2NH_3Cl, calculate the initial pH and the final pH after adding 0.0200 mol of NaOH (K_b = 6.46 \times 10^{-4}).
- For 270.0 mL of a buffer solution that is 0.215 M in HCHO_2 and 0.285 M in KCHO_2, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.
- For 260.0 mL of a buffer solution that is 0.2922 M in CH_3CH_2NH_2 and 0.2677 M in CH_3CH_2NH_3Cl, calculate the initial pH and the final pH after adding 0.0100 mol of NaOH (K_b = 5.6 times 10^-4).
- calculate the initial pH, final pH, and change in pH when 3.5 mL of 0.25M NaOH is added to 100.0 mL of pure water
- If 22.0 mL of 0.182 M NaOH solution is added to 100 mL of a solution that is 0.100 M in HA (Ka = 5.00 x 10-5) and 0.100 M in NaA, what will be the pH of the new solution? Give your answer to four decimal places.
- Calculate the pH of a solution obtained by adding 30 mL of 0.20 M HOAc to 25 mL of 0.10 M NaOH.
- Find the pH of a 400.0 mL solution with a concentration of 0.75 M NaOH.
- Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the addition of 54.00 mL of the NaOH solution.
- Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the addition of 39.10 mL of the NaOH solution.
- Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the addition of 27.00 mL of the NaOH solution.
- A 100 mL sample of 0.503 M H2A(diprotic acid) is titrated with 0.200 M NaOH. After 125.0 mL of 0.200 M NaOH has been added, and the pH of the solution is 4.50. Calculate Ka1 for H2A and explain in detail.
- Calculate the pH of the resulting solution if 33.0 ml of 0.33 M HCl(aq) is added to, (a) 43.0 mL of 0.33 M NaOH (aq) (b) 23.0 mL of 0.430 M NaOH (aq).
- Calculate the pH of the resulting solution if 26.0 mL of 0.260 M HCl(aq) is added to: a. 31 mL of 0.260 M NaOH b. 36 mL of 3.10 M NaOH
- Calculate the pH of a solution that contains 0.3 g of NaOH dissolved in water to give 200 mL of solution.
- Calculate the pH during the titration of 40.00 mL of 0.1000 M HCI with 0.1000 M NaOH solution after additions of base: a. 18.00 mL pH = b. 39.50 mL pH = c. 48.00 mL pH =
- Calculate the pH of the solution when the substance is added together: 200 mL of 0.01 M HCl and 8 mL of 0.25 M NaOH
- Calculate the volume of 1.50 x 10^-2 M NaOH that must be added to 500.0 mL of 0.200 M HCl to give a solution that has pH = 2.15.
- Calculate the pH that results when 25 mL of 0.1 M HCl is titrated with 0.1 M NaOH solution run in from a burette at each of the stages of volume of 0.1 M NaOH add in 5.0 mL incrememnts beginning with
- A 50 ml sample of 0.5 M HCl is titrated with 0.5 M NaOH. What is the pH of the solution after 28 ml of NaOH have been added to the acid?
- A 20.0-mL sample of 0.300 M HBr is titrated with 0.150 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?
- A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid? A. 0.85 B. 2.96 C. 2.85 D. 1.49 E. 3.81
- Calculate the pH of a solution after the addition of 10 ml of a 0.1 M NaOH to a solution of 25 ml of 0.1 M HCl. (Total volume of the solution is 35 ml)
- For 280.0 mL of a buffer solution that is 0.210 M in HCHO2 and 0.280 M in KCHO2, calculate the initial pH and the final pH after adding 0.010 moles of NaOH.
- For 290.0 mL of a buffer solution that is 0.200 M in HCHO2 and 0.310 M in KCHO2, calculate the initial pH and the final pH after adding 0.010 moles of NaOH.
- For 300.0 mL of a buffer solution that is 0.215 M in HCHO2 and 0.295 M in KCHO2, calculate the initial pH and the final pH after adding 0.005 moles of NaOH.
- A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. Find the pH after the addition of 10.0 mL of NaOH.
- For the titration of 25.00 mL of 0.150 M HCl with 0.250 M NaOH, calculate (a) the initial pH; (b) the pH when neutralization is 50% complete; (c) the pH when neutralization is 100% complete; and (
- Calculate the pH if you have 10.0 mL of a 0.1 M NaOH solution and 7.1 mL of H2O is added.
- Calculate the pH of a solution formed by mixing 40.0 mL of 0.1000 M HCl with 39.95 mL of 0.1000 M NaOH and then diluting the entire solution to a total volume of 100 mL.
- A 25.0 mL sample of .100M HClO4 is titrated with .200M NaOH A. What is the initial pH of the solution? B. What is the pH of the solution after the addition of 10.0mL of NaOH? C. What volume of NaOH
- Calculate the volume of 0.1M NaOH which must be added to 50 mL of 0.1M HCl to give a final solution of pH 6?
- 14 mL of 0.010 M NaOH are added to 29 mL of water. Determine the pH of the resulting solution.
- A 50.0 mL sample of 0.100 M acetic acid solution is titrated with 0.100 M NaOH solution. Calculate the pH of the system. a) At the beginning of the titration b) When 15.0 mL of NaOH has been added
- If 30.0 mL of 4.8 x 10^{-2} M HBr is added to 21.5 mL of 3.6 x 10^{-2} M NaOH, what is the pH of the solution?
- Calculate the pH when 20.0 mL of a 0.10 M NaOH solution is mixed with 60.0 mL of a 0.85 M HF solution.
- Consider the titration of 10.00 mL of 0.400 M hypochlorous with 0.500 M NaOH. What is the initial pH (before any NaOH is added)?
- Calculate the pH of 30.0 mL of 0.025 M NaOH.
- Calculate the pH at the beginning of a titration of 50.00 of 0.005 M HA (k_a = 2.0 times 10^{-2}) with NaOH solution.
- 125 ml of 0.025 M NaOH are added to 175 mL of 0.030 M HCl. What is the pH of the resulting solution?
- Calculate the pH of a solution made by mixing 100.0mL of 0.1M HCl with 150.0ml of 0.1M NaOH.
- Calculate the pH at the equivalence point when 20.0 mL of 0.55 M HCl is titrated with 20.0 mL of 0.55 M NaOH. A. 5.00 B. 9.00 C. 0.26 D. 14.00 E. 7.00.
- The titration is 0.010 M NaOH. Calculate pH at the starting point, 0.00 mL titrant added.
- A 100. mL solution of NaOH has a pH of 13.51. If you add 110 mL of water to the original solution, what will the resulting pH be?
- Consider the titration of 100.0 mL of 0.200 M HCl with 0.400 M NaOH. What is the initial pH before any NaOH is added?
- 50 mL of 0.1 M HNO3 solution is mixed with 25 mL of 0.1 M NaOH. What is the pH?
- Calculate the pH when 30 mL of 0.1 M NaOH is added to 200 mL of 3.5 x 10-5 M HCl.
- Determine the pH of 30.0 mL of 0.025 M NaOH
- What is the pH and pOH of a solution that was made by adding 400 mL of water to 350 mL of 5.0 times 10^{-3} M NaOH solution?
- Calculate the pH of the solution in a flask after 25 mL of NaOH has been added. Presume 0.413 g of KPH is dissolved in 25 mL of water and then titrated with 0.1 M NaOH.
- Calculate the pH of a mixture of 20.0 mL of 0.150 M HCl and 10.0 mL of 0.300 M NaOH?
- Calculate the OH- and pH for 2.33 g of NaOH in 500 mL of solution.
- Question 8 10 mL of 0.010 M NaOH are added to 21 ml of water. Determine the pH of the resulting solution. Question 9 Calculate the pH of a 0.10 M NaHX salt solution. Ka(H_2X) 2.1 x 10^-2.H_a(HX^-) =
- Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. a. What is the initial pH (before any NaOH is added)? The Ka for HOCI is 3.0 times 10^-8 M. b. How ma
- A 427 mL sample of 0.2553 M HBr is mixed with 539 mL sample of NaOH (which has a pH of 13.87). What is the pH of the resulting solution?
Explore our homework questions and answers library
Browse
by subject