2. The reaction utilized in Part I of the experiment is:НС-Н:О- (аq) + NaOH (aq) — Н,0 () + СH;0; (ад)What chemical species are present at the equivalence point in Part I of the experiment? List theirformulas.а.b. Is the equivalence point in Part I of the experiment in the acidic, basic, or neutral range?c. Account for this observation by writing the relevant chemical reaction and discussing the pH nature ofits product(s).

The reaction taking place in the experiment is, HC2H3O2 (aq) + NaOH (aq)→H2O (l) + C2H3O2-(aq)

2. The reaction utilized in Part I of the experiment is: НС-Н,О2(ад) + NaOH (aq) — Н,0 () + C-H;О2 (аq) a. What chemical species are present at the equivalence point in Part I of the experiment? List their formulas. b. Is the equivalence point in Part I of the experiment in the acidic, basic, or neutral range? c. Account for this observation by writing the relevant chemical reaction and discussing the pH nature of its product(s).

2. The reaction utilized in Part I of the experiment is: НС-Н,О2(ад) + NaOH (aq) — Н,0 () + C-H;О2 (аq) a. What chemical species are present at the equivalence point in Part I of the experiment? List their formulas. b. Is the equivalence point in Part I of the experiment in the acidic, basic, or neutral range? c. Account for this observation by writing the relevant chemical reaction and discussing the pH nature of its product(s).

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 4RQ: How is acid strength related to the value of Ka? What is the difference between strong acids and...

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Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. In addition, write Lewis structures for all starting materials and products. Label the original acid and its conjugate base; label the original base and its conjugate acid. If you are uncertain about which substance in each equation is the proton donor, refer to Table 4.1 for the relative strengths of proton acids. (a) NH3+HCl (b) CH3CH2O+HCl (c) HCO3+OH (d) CH3COO+NH4+
How is acid strength related to the value of Ka? What is the difference between strong acids and weak acids (see Table 13-1)? As the strength of an acid increases, what happens to the strength of the conjugate base? How is base strength related to the value of Kb? As the strength of a base increases, what happens to the strength of the conjugate acid?
Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or base? Explain.
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.)
6. Find Ka and Kb of each of the following amphiprotic anions and determine if they act as an acid or a base in water solution. а) НРО- Ka = (С.А. 3D Kb = A or B b) HC,H;0, Ka = (C. A. = ) Kb = A or B c) HSO; Ka = : (C. A. = Kb = A or B
8. Identify each molecule as an acid or a base, then give the formula for the conjugate base or acid (what is formed after it accepts H+ or donates H+.. IF amphiprotic, then label as amphiprotic and write the conjugate acid AND base. а. НBrОз d. NH3 b. SO;- е. CO;²- c. HCI f. HC2O;'-
8. How would you describe the solution of the salt formed from the reaction of a weak acid and a strong base? A. Acidic В. Basic C. Neutral D. Slimy 9. The Bronsted-Lowery acid in the reaction H20 + NH3 = NH, + OH- is С. ОН D. NH4 10.In the following equilibrium: HC2O4 + HCO3! = C2042 + H2CO3 identify the А. Н.О B. NH3 conjugate base. C. HC2O4-1 D. H.COз А. НСО-1 В. C2042
a. What is the base ionization constant for CH,BrCOO-? Kb: CH -7 -5 ニフ 7.14 x 10 "CH zBV CoOlH Ś CHZBV C00 b. What is the standard free energy of formation of CH2BRCOO ? CHz Br c O0 c. What is the pH of a 0.027 M NACH;B1COO? Note: More space on next page.
The chemical 5-amino-2,3-dihydro-1,4-phthalazinedione, better known as luminol, is used by forensic scientists in analyzing crime scenes for the presence of washed-away blood. Luminol is so sensitive that it can detect blood that has been diluted 10,000 times. A basic solution of luminol is often sprayed onto surfaces that are suspected of containing minute amounts of blood. Luminol has a molecular weight of 177 g/mol The technician must dilute the luminol solution to a concentration of 5.00×10−2 M . The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the diluted spray?
The chemical 5-amino-2,3-dihydro-1,4- phthalazinedione, better known as luminol, is used by forensic scientists in analyzing crime scenes for the presence of washed-away blood. Luminol is so sensitive that it can detect blood that has been diluted 10,000 times. A basic solution of luminol is often sprayed onto surfaces that are suspected of containing minute amounts of blood. Luminol has a molecular weight of 177 g/mol. The forensic technician at a crime scene has just prepared a luminol stock solution by adding 17.0 g of luminol into a total volume of 75.0 mL of H₂O. What is the molarity of the stock solution of luminol? Express your answer with the appropriate units. ► View Available Hint(s) molarity of luminol solution = 1.28 M Submit Correct Part B Previous Answers Before investigating the scene, the technician must dilute the luminol solution to a concentration of 4.00 × 10-2 M. The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many…
1. The following equilibrium exists when ammonium is dissolved in water: NH4+ (aq) + H2O (l) « H3O+ (aq) + NH3 (aq) The Ka of NH4 is 5.6 x 10-10. Find the pH of a 3.00 M solution of NH4Cl. (hint: since NH4Cl completely ionizes, the concentration of the ammonium ion is 3.00 M) NH4Cl (s)àNH4+ (aq) + Cl- (aq)

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