A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.0900 M KOH. What volume KOH must be added to give a pH of 5.697? K31 = 1.42 x 103 and K,2 = 2.01 x 10-6. O 67 mL O 89 mL O 11 mL O 22 mL O 44 mL

A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.0900 M KOH. What volume KOH must be added to give a pH of 5.697? K31 = 1.42 x 103 and K,2 = 2.01 x 10-6. O 67 mL O 89 mL O 11 mL O 22 mL O 44 mL

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 65E: Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate...

See similar textbooks

Related questions

Q: Choose one of the questions you circled above and explain how element could be used as a substitute…

Q: Determination of known acid concentration Trial 1 Trial 2 Trial 3 Volume…

A: Hcl + Naoh------>Naoh + H20 Moles of NaOH = Molarity of NaOH x Volume of NaOH used Moles of NaOH…

Q: Convert the concentration of 0.700 M Na:So, to g/mL STARTING AMOUNT

A: Given : Concentration of Na2SO4 = 0.700 M Assuming 1 L i.e 1000 mL of solution.

Q: We started with 20 mL 1 M acetic acid ~ 0.020 L acetic acid in a flask. (Ka acetic acid =…

A: Millimoles of acetic acid taken=Molar concentration of acid×mL of acid=1 M×20 mL=20 mmol

Q: None

A: The concept used to solve this problem is nature of solvent as well solute. "Like dissolves like"…

Q: Calculate the pH for each H,0* concentration. . [H_O*] = 1× 10-8 M pH [H,O*] = 0.01 M pH: %3D

A: GivenH3O+ = 1 × 10-8 MH3O+ = 0.01 MH3O+ =1 ×10-13 M

Q: h) H₂ Pt

A: Answer:Addition reaction is the type of reaction in which addition of new atoms or groups takes…

Q: OsO4 (cat) NMO OH OH Select to Draw > mCPBA O J Select to Edit

A: Reaction of alkene with OsO4 gives syn-1,2-diol. Reaction of alkene with mCPBA gives epoxide.

Q: Exercise 8.72 MISSED THIS? Watch KCV 8.7, IWE 8.7; Read Section 8.7. You can click on the Review…

Q: Which of these molecules would you expect to have the lowest boiling point? Select the single best…

A: Answer:-This question is answered by using the simple concept of boiling point which depends on the…

Q: If 25 grams of methane, CH 4, and 30 g of ammonia, NH 3, are combined w/ excess oxygen, how much…

Q: At 0 oC, the solubility of sodium acetate in water is 36.1 g per 100 g of water and at 40 oC, the…

A: Solubility is defined as the amount of solute in gram present in 100 mL of the solvent or solution.…

Q: SECTION 1: KNOWLEDGE 1. In nature, silicon is composed of three isotopes. These isotopes (with their…

A: The average atomic mass of an element having a number of isotopes is calculated by the formula:…

Q: 5. K4FE(CN)6 + H2SO4 + H2O → K2SO4 + FeS04 + (NH4)2SO4 + CO

A: A balanced chemical reaction is the one that contains equal number of atoms on both sides of the…

Q: Principal ingredient of an antacid is Al(OH)3 (76.98). The concentration of 0.00400 M Al(OH)3…

A: Given, Molarity of Al(OH)3 = 0.00400 M

Q: How many grams of Ba(103)2 (487 g/mol) can be dissolved in 400 mL of water at 25°C. (Ksp of Ba(103)2…

Q: Determine the dilution factor for your diluted unknown U1 based on how you prepared the solutions in…

A: Using a concentrated solution of a given compound, different concentration of the same solution can…

Q: If you are attending the question plese answer both the questions otherwise I'll downvote

Q: a šólutión óf HNO3 with a volume of 450 ml and a concentration of 0.3 M, if 225 ml of HNO3 was…

A: The volume of concentration of HNO3 solution is given in the question. As it is given, that 225mL of…

Q: c. Calculate for the mass of struvite that can be formed in the given urine sample. d. Given that…

Q: 28. The recommended concentration of chlorine in swimming pools is 2.00 – 4.00 ppm. What mass of…

Q: lable Preparatiol Of Standard affeine SOlutions Standard [Caffeine] (mg L-1 or ppm) Volume of Volume…

A: Standard [Caffeine], mg /L or ppm Vol of caffeine stock, mL Vol of internal standard, mL…

Q: An organic compound (A) has a general formula C,Hza. This compound has five carbon atoms. When the…

Q: To which sample solution the spike will be add? the distillate>130C the mass standard the…

A: A spike is a known quantity of analyte added to a sample of test solution whether to redponse to…

Q: In the laboratory, a student dilutes 24.8 mL of a 7.87 M hydroiodic acid solution to a total volume…

A: Initial Volume, V1 = 24.8 mL Initial Molarity ,M1 = 7.87 M Final Volume , V2 = 125 mL Final…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

Please Help 4

A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.0900 M KOH. What volume KOH must be added to give a pH of
5.697? K31 = 1.42 x 103 and K,2 = 2.01 x 10-6.
O 67 mL
O 89 mL
O 11 mL
O 22 mL
O 44 mL

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

The titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of the solution when 35.0 mL of the base has been added to 100.0 mL of 0.100 M acetic acid?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
The weak base ethanolamine. HOCH2CH2NH2, can be titrated with HCl. HOCH2CH2NH2(aq)+H3O+(aq)HOCH2CH2NH3+(aq)+H2O(l) Assume you have 25.0 mL of a 0.010 M solution of ethanolamine and titrate it with 0.0095 M HCl. (Kb for ethanolamine is 3.2 107.) (a) What is the pH of the ethanolamine solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 would be the best choice to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 10.0, 20.0, and 30.0 mL of the acid. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.
When a diprotic acid, H2A, is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If the pH at 50.0 mL NaOH added is 4.0, and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka1, and Ka2 for the diprotic acid.
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL b. 50.0 mL c. 100.0 mL d. 150.0 mL e. 200.0 mL f. 250.0 mL
Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). List the major species, and explain how you would go about calculating the pH of the solution at various points, including the halfway point and 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?
A buffer is made using 45.0 mL of 0.750 M HC3H5O2 (Ka = 1.3 105) and 55.0 mL of 0.700 M NaC3H5O2. What volume of 0.10 M NaOH must be added to change the pH of the original buffer solution by 2.5%?
To have a buffer with a pH of 2.50, what volume of 0.150 M NaOH must be added to 100. mL of 0.230 M H3PO4?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.