Answered: A 40.00 solution of 0.1430 M…

A 40.00 solution of 0.1430 M chloroacetic acid (pKa = 2.865) is titrated with a 0.1500 M solution of NaOH. Find the initial pH of the solution.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.3: Acid-base Titrations

Problem 17.6CYU: The titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of...

See similar textbooks

Related questions

Q: Equal quantities of 0.010 M solutions of an acid HA and a base B are mixed. The pH of the resulting…

A: Equilibrium equation : Given data: Equal quantities of 0.010 M solutions of an acid HA and 0.010 M…

Q: Consider the titration of a 40.0 mL of 0.189 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH. How…

A: The halfway point of the titration is that point where half of the acids has been reacted. The…

Q: In a titration experiment of a 25.00 ml of 0.100 M CH3CO2H with 0.100M NaOH, 12.50 mL of NaOH were…

A: We have 25 mL of 0.1 M acetic acid and 0.1 M 12.5 ml NaOH , we have to calculate the pH of resulting…

Q: An analytical chemist is titrating 109.0mL of a 0.4900M solution of hydrazoic acid HN3 with a…

Q: Calculate the pH of a buffer solution that is 0.100 M acetic acid and 0.200 M sodium acetate.The Ka…

A: pH of a buffer solution is calculated using formula,

Q: Calculate the pH of a solution made by dissolving 26.5 g potassium acetate in 150 mL solution.…

A: We have to calculate the pH of solution.

Q: A 40.00 solution of 0.1430 M chloroacetic acid (pKa = 2.865) is titrated with a 0.1500 M solution of…

A: Given, Volume Of the Solution = 40ml Concentration Of Chloroacetic acid = 0.1430 M Concentration…

Q: Hydrohalpinic acid, HJh(aq), is a weak monoprotic acid with Ka = 4.09 x 105 at 25.0 °C. 25.0 mL of a…

Q: Chloroacetic acid is a weak acid with Ka = 1.4x104. What is the pH at the equivalence point when…

A: ClCH2COOH + NaOH -----> ClCH2COONa + H2O So, at equivalent point it exist as an aqueous…

Q: Calculate the pH of a solution that is 0.45 M CH3COOH and 0.75 M NaCH3COO. Sodium acetate/acetic…

A: Buffer is a solution which consists of a weak acid and it's conjugate base or weak base and it's…

Q: 2. At 25°C, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate. A) If the…

Q: 8. Calculate the pH at the equivalence point when 0.104 g sodium acetate (NaC2H3O2; K, = 5.6x10-10)…

A: The pH shows characteristics properties of solutions whether they contain high or low amount of…

Q: 1. A buffer solution is prepared by taking 0.25 moles of acetic acid (pKa = 4.76) and 0.400 moles of…

A: 1. Given,

Q: Calculate pH during the titration of 40.00 mL of 0.1000 mol L-1 propanoic acid, CH3CH2COOH, after…

Q: A solution of HA (0.197M; 81.7mL; Kp =5.5E-7) is titrated with 0.4334M KOH. Determine the pH at the…

A: pH of solution at different points can be calculated using Henderson hasselbalch equation.

Q: 30.0 mL of 0.200 M HCN is placed in an Erlenmeyer flask. After titrating the solution with 15.0 mL…

A: The reaction taking place is,

Q: Question is attached

A: Given in the question : Volume of HCl = 5 ml Molarity of HCl = 0.1 M Volume of water = 50 ml Moles…

Q: 50.00 mL of 0.1000 M ammonia solution is titrated with 0.1000 M HCl. Calculate the pH of the…

A: Given : concentration of NH3 = 0.1 M = concentration of HCl volume of NH3 = 50 mL = 0.050 L And…

Q: Find the pH of a solution produced by the reaction of 250 mL 0.1 M NaOH and 150 mL 0.03 M acetic…

A: Gvien, 250 mL 0.1 M NaOH and 150 mL 0.03 M acetic CH3COOH

Q: A buffer solution is prepared by taking 0.25 moles of acetic acid (pKa = 4.76) and 0.400 moles of…

A: Given: Moles of acetic acid = 0.25 mol Moles of barium acetate = 0.400 mol Volume of solution =…

Q: 55.0 mL of a 0.15 M weak acid (K, = 1.8 x 105) is titrated with 10 mL of a 0.80 M strong base.…

Q: What is the pH of a solution

Q: You are working in a lab and someone has just handed you a beaker filled with 110 ml of a mysterious…

A: pH of a buffer is calculated using Hasselbach Henderson equation: pH =pKa+log([Conjugate…

Q: A buffer solution is prepared by adding 40.0 g of sodium acetate CH;COON to 500 mL of a 0.200 M…

A: The no of moles of sodium acetate and acetic acid are as follows:

Q: What is the pH of a solution that results from mixing together equal volumes of a 0.070 M solution…

Q: Find the pH of the solution when 0.0200 M an amino acid (NH:"RCO0') is titrated to the equivalence…

A: Ka1 and Ka2 represents the acid dissociation constants of carboxy terminal and amino terminal,…

Q: A student dissolves 0.0100 mol of an unknown weak base in 100.0 mL of water and titrates the…

A: Given: moles of weak base = 0.010 mol concentration of HNO3 = 0.100 M Volume of HNO3 = 40.0 mL pH =…

Q: A 25.0-mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH…

A: The explanation is given below-

Q: For the titration of sulfuric acid (H2SO4) with sodium hydroxide (N2OH), how many moles of sodium…

A: The reaction taking place can be written as NaOH + H2SO4 --------> Na2SO4 + H2O Balancing :…

Q: b) An acid-base titration experiment was conducted by using Nitric acid, HNO; and sodium hydroxide,…

A: Given, Concentration of HNO3 solution = 0.1 M = 0.1 mol/L Volume of HNO3 solution = 50 mL = 0.05 L…

Q: A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NAOH solution. What is the pH…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: what is the pH of a buffer that is 0.260 M in a weak acid and 0.250M in the acids conjugate base?…

A: Given Buffer of 0.260 M in a weak acid and 0.250M in the acids conjugate base with pKa for the acid…

Q: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka = 1.8 x 105)…

Q: H 10 15 20 25 30 35 40 45 50 0.1 M base added e pH curve represents the titration of a acid with a v…

A: Here, we have the pH curve for titration of 25 ml of a 0.1 M monoprotic acid solution with a 0.1 M…

Q: 20.00 mL of 0.035 M formic acid solution is titrated with 0.0175 M sodium hydroxide. Calculate the…

A: Molarity of formic acid, M1 = 0.035 M Volume of formic acid, V1 = 20.00 mL = 0.020 L Molarity of…

Q: Calculate the pH of a buffer solution prepared by dissolving 19.50 g of sodium cyanate NaCNO…

A: Mass of NaCNO = 19.50 g The number of moles of NaCNO, n = mass of NaCNO/molar mass of NaCNO…

Q: Calculate the pH at the equivalence point of 50 mL of hypochlorous acid, HCIO, titrated with 31 mL…

A: GIVEN: Volume of HOCl = 50 ml Concentration of HOCl = M Volume of KOH = 31 ml Concentration of KOH =…

Q: Calculate the pH of a solution containing 17 mL of 0.71 M of a weak weak base B OH, like NH4OH, or…

A: Initially the number of moles of NH3 is calculated as shown below.

Q: 50.0 mL solution is prepared to be 1.29 M acetylsalicylic acid. In the first step, 8.55 mL of NaOH…

A: Volume of solution = 50.0ml Volume of NaOH = 8.55 ml

Q: 5) Part 1 Calculate the pH at the stoichiometric point when 25 mL of 0.10 M pyridine is titrated…

A: Pyridine ( a weak base) reacts with HCl ( a strong acid ) to undergo neutralisation reaction to form…

Q: 2. A. Calculate the pH of a 0.500 L buffer solution composed of 0.700 M formic acid (HCOOH, Ka =…

A: Use the Henderson-Hasselbalch equation to calculate pH of buffer solution for part A and then solve…

Q: Calculate the pH of a buffer solution prepared by mixing 25 mL of 0.5 M lactic acid and 75 mL of 1.0…

A: Buffer solution buffer solution is a solution that only changes slightly when an acid or a base is…

Q: calculate the pH of a asolution that is made when 0.10 L of 0.24 M benzoic acid (pKa=4.19) and 0.050…

A: Benzoic acid is a weak acid and sodium hydroxide is a strong base. The reaction between them results…

Q: What is the pH of a mixture that contains 0.20 M Ca(OH)2 and 0.20 M LiOH?

A: Strong bases completely ionize when dissolved in water. Both the base, Ca (OH)2 and LIOH are strong…

Q: A 25 mL sample of 0.15M hydrazoic acid is titrated with a 0.15M NaOH solution. What is the pH after…

A: Answer:- This question is answered by using the simple concept of calculation of pH during the…

Q: A buffer solution is prepared by taking 0.250 moles of acetic acid (pKa = 4.76) and 0.400 moles of…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2,M(OH)2, is mixed with pure water.…

A: Given that,PH of the solution = 10.28Ksp =?You know thatPH + POH = 14

Q: What is the pH of a buffer solution made by mixing 50.0 ml of 0.100M potassium hydrogen phthalate…

Q: If a 50 mL solution of 0.1 M HCN (Ka = 6.2 x 10-10) is titrated with 0.1 M NaOH, what is the pH of…

Question

A 40.00 solution of 0.1430 M chloroacetic acid (pK_a = 2.865) is titrated with a 0.1500 M solution of NaOH. Find the initial pH of the solution.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
A solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of solution. A 30.00-mL sample of the solution is titrated with 0.272 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.
Two acids, each approximately 0.01 M in concentration, are titrated separately with a strong base. The adds show the following pH values at the equivalence point: HA, pH = 9.5, and HB, pH = 8.5. (a) Which is the stronger acid, HA or HB? (b) Which of the conjugate bases, A or B, is the stronger base?
Calculate the pH of a solution that is 0.20 M HOCl and 0.90 M KOCl. In order for this buffer to have pH = pKa, would you add HCl or NaOH? What quantity (moles) of which reagent would you add to 1.0 L of the original buffer so that the resulting solution has pH = pKa?
A 40.00 solution of 0.1430 M chloroacetic acid (pKa = 2.865) is titrated with a 0.1500 M solution of NaOH. Find the initial pH of the solution and find the pH of the resulting solution at the equivalence point.
20.00 mL of 0.250 M propanoic acid, C3H7COOH, is titrated with 0.125 M NaOH. Calculate the pH for the following five situations after the indicated amount of NaOH solution has been added. The Ka of propanoic acid is 1.34 x 10 ̄5 a) 40.00 mL b) 50.00 mL
At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.16. What is the Ksp of the salt at 22 °C?
1) In the laboratory, a general chemistry student measured the pH of a 0.554 M aqueous solution of nitrous acid to be 1.787. Use this information she obtained to determine the Ka for this acid? Ka .......................... ? 2) How many grams of solid potassium hydroxide ( molar mass= 56.1 g/mol) are needed to react with 26.7 mL of a 1.75 M hydroiodic acid solution? KOH + HI......> kI + H2o ................ grams
In the titration of 100.0 mL of 0.050 M CH3COOH (pKa = 4.74) solution, what will be the pH after adding 20.0 mL of a 0.10 M NaOH titrant?
What is the pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7 ?
What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml of 3.66M Sodium Formate (NaHCO2) together? If you were to now add 18 ml of 1.2M NaOH to the buffer solution, what would the new pH be?
Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a citric acid concentration of 0.3 M and produce 20 mL. What is the pH after 20 mL of 0.6 KOH has been added?