V(acetic acid CH₂COOμ) = 10ml с = 0,271 м titrated with potassium hydroxide solution. c= 0, 253 M a) pH=? (V(KOH) = 0.00, 3.00, 6,00, 9,00, (2,00 ml) B) [H₂0], [OH]=? (in the solutions) pka (CH₂COOk)= 4,75

V(acetic acid CH₂COOμ) = 10ml с = 0,271 м titrated with potassium hydroxide solution. c= 0, 253 M a) pH=? (V(KOH) = 0.00, 3.00, 6,00, 9,00, (2,00 ml) B) [H₂0], [OH]=? (in the solutions) pka (CH₂COOk)= 4,75

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Calculate the pH at the equivalence point in titrating 0.045 M solutions of each of the following…

A: Concept based on the finding out the pH at the he equivalence point between the acid- base…

Q: Succinic acid has the formula HOOC - CH2CH2 - COOH, if 100.0 mL of a 0.10 M of the acid is titrated…

A: To calculate the pH, we first need to determine the moles of succinic acid and NaOH that react with…

Q: The literature Ksp value for Mg(OH)2 is 1.8×10-11. (a) Calculate the theoretical [OH¯] in a…

A: a.) First we would write dissociation equation of Mg(OH)2 and use Ksp value to calculate…

Q: Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine,…

Q: Determine the acid dissociation constant, Ka, for a 0.10 Ma weak acid solution that has a pH of…

A: Given : Concentration of weak acid HA = 0.10 M And pH of the solution = 2.87 The ionisation…

Q: A buffer solution is made that is 0.370 M in CH3COOH and 0.370 M in CH3COONa. (1) If Ka for CH3COOH…

Q: A 0.1510 g KHP (Mw = 204.22 g/mol) sample required a volume of 57.04 mL of NaOH solution to reach a…

A: KHP reacts with sodium hydroxide to form NaKPH and water. One mole of KHP reacts with one mole of…

Q: An analytical chemist weighs out 0.133 g of an unknown diprotic acid into a 250 mL volumetric flask…

Q: A buffer solution is made that is 0.411 M in CH3COOH and 0.411 M in CH3CO0NA. (1) If K, for CH3COOH…

A: Answer:- This question is answered by suing the simple concept of calculation of pH of a solution…

Q: You will perform several calculations with the data you obtain in the titrations lab. Below is an…

A: Molarity is defined as the number of moles of solute divided by volume of solution in litres. By…

Q: Acid Base Tritation When 25.00 mL of HNO3 are titrated with Sr(OH)2, 58.4 mL of a 0.218 M solution…

A: A) before titration first Calculate mole of Sr(OH)2 then use Mole-mole realtionship to get mole of…

Q: A 5.55-g sample of a weak acid with Ka = 1.3 * 10 - 4 was combined with 5.00 mL of 6.00 M NaOH, and…

A: The general reaction between NaOH and diprotic acid is as follows, Calculate the moles of sodium…

Q: 12) To determine the titration acidity of a bottled cherry juice, 0.01 L of cherry juice was…

A: Cherry juice contains malic acid dominantly.Molar mass of malic acid = 134 g/ moleMalic acid…

Q: A buffer solution is made that is 0.442 M in HCIO and 0.442 M in NaCIO. (1) If Ka for HCIO is…

Q: What is the pH of the solution when Caitlin has added 50.00 mL of the 0.25 M LIOH to the 25.00 mL of…

Q: A buffer is prepared such that [CH3COOH], = [CH3C00-lo = 0.050 M. Calculate the volume of 0.10 M…

A: Millimoles of Acetic acid = M x V = 0.050 x 100.0 = 5.0 mmol = Millimoles of sodium acetate Let…

Q: The graph here shows the pH curve for the titration of 25.00 mL of a 0.100-M monoprotic acid…

A: Acid base titration is indicator based titration. It gives different colour at different pH value.…

Q: 4. (6) Calculate the concentration of sodium benzoate (NaC,HSO2) that must be present in a 0.20M…

A: Using the formula to calculate the concentration required. Neglect the common ion effect, since ka…

Q: How many grams of BHCl (acidic salt, 69.83 g/mol) would need to be added to 490 mL of 1.5 M B (a…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: A 15.00 ml aliquot of a 0.75 M solution of a weak acid (Ka = 1.50E-04 at 25°C) is titrated with…

Q: You will perform several calculations with the data you obtain in the titrations lab. Below is an…

A: The concentration of the NaOH solution is 0.473 M = 0.473mol/L.The volume of the NaOH solution is…

Q: Draw the titration curve that would result if 35 mL of a 0.2 M CH3NH2 (kb = 4.60 x 10-4) were…

A: [CH3NH2] = 0.2 M Volume of CH3NH2 = 35 mL Kb = 4.60 *…

Q: At the equivalence point for the titration of HCN with KOH, the pH is expected to be A) 7 B) greater…

A: Here HCN - is weak acid KOH - is strong base

Q: A 1.00 g sample containing NaHC0, was dissolved in water and titrated using 0.500 M HCI. The sample…

A: Given that: Molarity of HCl = 0.500M Volume of HCl required = 12.5ml = 12.5ml×1L/1000ml = 0.0125L

Q: 5.) A typical aspirin contains 324 mg of aspirin (HC,H,O4) with Ka = 2.8 x 104. If you dissolve two…

A: pH = -log[H+] Aspirin is a weak acid. For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molar…

Q: What is the pH of a solution containing 0.44 M dimethylamine, (CH3)2NH, (K₁ = 5.13 * 104) and 0.20 M…

Q: Calculate the pH at the equivalence point in titrating 0.057 M solutions of each of the following…

A: Concentration of NaOH = 0.079 MEquivalence Point: It is a point at which, equivalent quantities of…

Q: HPro (aq) + OH-(aq) H2O (1) + Pro-(aq) Identify the limiting reagent, and find the concentrations of…

A: 7. At equilibrium, we have HPrO and its salt NaPrO. The net ionic equation between the two is: HPrO…

Q: Given the following hydrolysis constants, which of the salts has the weakest parent ACID? K₂ or K,…

A: given-hydrolysis constants of given salts.SALTK2 OR K for…

Q: H3C—N̈H2 reacts with BF3 in a combination reaction, forming H3C—NH2—BF3 with a covalent bond between…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: The literature Ksp value for Mg(OH)2 is 1.8x10-11. (a) Calculate the theoretical [OH-] in a…

Q: What is the change in ph when 1.0ml of 1m hcl is added to 1) 1.000L of pure water and to 2)…

Question

V (acetic and CH ₂ COOH) = 10ml
C = 0,271 M
titrated with potassium hydroxide solution
c= 0, 253 M
a) pH=? (V (KOH) = 0,00, 3,00, 6,00, 9,00, 12,00 ml)
6) [H₂0], [OH-] = ? (in the solutions)
pka (CH₂COOH) = 4, 15

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: Write the objective

VIEW

Step 2: Calculating the pH

VIEW

Step 3: Calculating the pH

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 94 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

3. (a) Is it possible to measure SO3 in the presence of OH (each with a concentration of 0.1 M) by titration with HCl? (b) Construct the corresponding titration curve and determine the pH of different points in the curve. H2SO3: pKal = 2, pKa2 = 7 (c) If possible, select the appropriate equivalence points and explain how to calculate the concentration of each.
Question 21 of 36 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 10.0 mL of the strong base has been added. The value of Ka for HC4H,O2 is 1.5 x 10. ( PREV 1 3 4 NEXT > Based on the result of the acid-base reaction, set up the ICE table in order to determine the unknown. HC4H;O2(aq) + H20(1) H3O*(aq) + C4H,O2 (aq) Initial (M) 0.120 0.0400 Change (M) Equilibrium (М) +x +x 0.120 - x +x 0.0400 + x 5 RESET 0.100 0.120 0.140 0.0200 0.0400 +x 0.100 + x 0.100 - x 0.120 + x 0.120 - x 0.140 + x 0.140 - x 0.0200 + x -x 0.0200 - x 0.0400 + x 0.0400 - x
Q1 A mixture of acetic acid and sodium acetate makes an effective buffer. Here is the equilibrium equation for these two species: HC,H3O2 (aq) + H2O (I) = C,H3O2¯ (aq) + H3O† (aq) (a) What reaction would take place if acid were added to this buffer? (b) What reaction would take place if base were added to this buffer?
Q2.9 What would be the pH of a buffer that is composed of mh of 0.10 M CH3 CaoNa? and 125 92 mL of 0.10M CH3COOH known: Ka (CH3 COOH) = 1.81x10-5 write. your answer to 2 decimal places.
I need help please.
Which of the following does not have eight valence electrons? Cl- Xe Ti+4 Rb+ Sr+
A 25.0 mL sample of 0.450 M (CH3)2NH is titrated with HBr. What is the pH of the solution after 30.0 mL of 0.375 M HBr have been added to the methylamine solution? ((CH3)2NH; Kb Give answer to 2 decimal places. = 5.9×10-4)
5:48 PM Wed Nov 16 Today 5:48 PM 目。 oint when 15.0 ml. of o. 75% Calculate the pH of a titration at the point when 15.0 mL of 0.15 M NaOH is added to 30.0 mL of 0.20 M HNO3 Edit G ¯¯¯
What is the pH of the solution when Henry has added 35.00 mL of 0.50 M NaOH to the 50.00 mL of 0.25 M nitrous acid? KaHA = 4.0 x 10-4 pH = [?] PH Enter
4.
What is the pH at the equivalence point in the titration of 60.00 mL of 0.200 M HA (a generic acid with K, = (2.26x10^-5)) with 0.400 M NaOH? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
dont provide handwriiting solution ...