None One way to make vinegar is to prepare a solution of acetic acid, the sole acid component of vinegar, at pH 3.0 and addappropriate flavoring agents. Acetic acid is a liquid at 25 °C with relative molecular mass (M,) of 60.1, density of 1.049 g/mL,and acid dissociation constant (K₁) of 1.7 x 10 M.Calculate the volume of acetic acid needed to produce 1.00 L of simulated vinegar from distilled water. Remember to usesignificant figures in your answer.2.53acetic acid volume:IncorrectmL

Step 1: Calculate the Hydrogen Ion Concentration [H+]The pH of the solution is 3.0. The relationship…

Answered: One way to make vinegar is to prepare a…

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 7RQ: Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a...

See similar textbooks

Similar questions

Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
An organic acid (HA) has a molecular weight of 100. g mol-1, a Kow = 5.6 and a K, = 2.7 x 10-2. If originally 2.0 g of the acid is dissolved in 100 mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100 mL of water, what will be the pH of the water? (Consider the equilibrium processes to be sequential and unrelated chemically) O 1.89 1.48 O 2.01 1.74 O 1.61
You are studying a clear solution and you added the pH indicator methyl violet. The colour range of the indicator methyl violet in a clear solution when changing from acidic to basic is yellow (pH 0) to blue purple (pH 1) to violet (pH 2). You initial pH of the solution when tested with a pH meter is O.2. You are going to add 250 drops of 0.1 M HCI. Please select the most appropriate answers to the following two questions. What is the initial colour of the solution at pH 0.2? What is the colour of the solution and what will the pH be after the addition of the HCI? Select 2 correct answer(s) The colour of the solution after the addition of HCI will be clear and the pH will be less than 0.2. The colour of the solution after the addition of HCI will be violet and the pH will be higher than 0.2.
An organic acid (HA) has a molecular weight of 100g/mol, a Kow = 5.6 and a K, = 2.7 x 10-2. If originally 2.0 g of the acid is dissolved in 100 mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100 mL of water, what will be the pH of the water? (Consider the equilibrium processes to be sequential and unrelated chemically) Possible answers: 1.89, 1.48, 2.01, 1.74, 1.61
An organic acid(HA) has a molecular weight of 100. g mol^-1, a Kow=5.6 and a Ka=2.7x10^-2. If originally 2.0g of the acid is dissolved in 100mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100mL of water, what will be the pH of the water? (consider the equilibrium processes to be sequential and unrelated chemically)
The salt K2HPO4 (potassium hydrogen phosphate) is a strong electrolyte but not a strong acid or base. Consider an F = 0.010 M solution of K2HPO4. a) Add the acid/base behavior of hydrogen phosphate by writing a “sequential dissociation scheme” for phosphoric acid (H3PO4). Then write mass balance equations for total phosphate and total potassium and give their numerical values. b) Write the charge balance equation for this solution. How may total species are there? [Count species in the charge balance equation and add any neutrals.] How many additional equations are needed for systematic treatment of equilibrium? Name them (give their usual symbols) c) Consider the KHPO4−(aq) ion pair. This is a new species, so what additional equation would you need? Tell how you would alter each charge or mass balance equation (if necessary) to include this species.
1.) Use the following acid or base dissociation constants to calculate the pH of the listed aqueous solutions. Acid Ка Base Kb hypochlorous acid, HCIO 4.0 x 10 8 methylamine, CH3NH2 5.0 x 104 hydrofluoric acid, HF 6.3х 104 pyridine, CSH5N 1.7 x 109 formic acid, HCOOH 1.8 x 104 ammonia, NH3 1.8 x 105 a.) pH of 0.155 M Ba(OH)2 b.) pH of 0.750 M hypochlorous acid, HCIO c.) pH of 0.215 M CH3NH3CI(aq)
The KHP titer of NaOH is 40.84mg/mL. Determine total acidity if 18.00mL of NaOH is required to titrate 5.00mL vinegar sample. Give the chemical reactions involved.
In the year 1980, countries near the United States experienced an increase in acid precipi- tation. During this same year, the United States had an increase in the burning of fossil fu- els to power homes and vehicles. Which statement best describes how these two occurrences are related? The United States' emissions of sulfur dioxide and nitrogen dioxide increased as a result of a decrease in the burning of fossil fuels to power homes and vehicles, and wind pat- terns caused these emissions to travel, leading to the formation of acid precipitation in other areas. The United States' emissions of sulfur dioxide and nitrogen dioxide increased as a result of an increase in the burning of fossil fuels to power homes and vehicles, and wind pat- terns caused these emissions to travel, leading to the formation of acid precipitation in other areas. The United States' emissions of sulfur dioxide and nitrogen dioxide decreased as a re- sult of an increase in the burning of fossil fuels to power…
A diprotic acid, H₂A, has acid dissociation constants of K₁1 = 3.75 x 104 and K₁2 = 5.10 × 10-¹¹. Calculate the pH and molar concentrations of H₂A, HA, and A²- at equilibrium for each of the solutions. A 0.195 M solution of H₂ A. pH = 2.08 -3 [HA] = 8.37 x107 A 0.195 M solution of NaHA. pH= 6.86 [HA] = pH= A 0.195 M solution of Na, A. Incorrect 11.78 [HA] = 6.09 X10-3 M M M [H₂A] = 0.187 [A²-] = [H₂A] = [A²-] = [H₂A] = 5.10 x10-11 6.76 x10-5 Incorrect 7.65 x10-5 Incorrect 2.67 X10-11 [A²] = 0.189 M M M M M M
Methanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 3) A 35.0 mL sample of (monoprotic) lactic acid, C3H6O3, is titrated with 20.0 mL of a 4.0 x 10-4 mol/L sodium hydroxide solution. What is the pH of the resulting solution at the equivalence point, if Ka for lactic acid is 1.4 x 10-4? PLEASE HELP THIS IS VERY URGENT

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS