Determine the dissociation constants for the acids. Express the answers in proper scientific notation where appropriate.Acid A: pKa = 6.0KaAcid B: pKa = 9.60Ka= -2.0Acid C: pKaKa =

We have to calculate the dissociation constant of acid.

Answered: Determine the dissociation constants…

Appl Of Ms Excel In Analytical Chemistry

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Author:Crouch

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Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 15P

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Hydrazine (N2H4) is like CO32 in that it is a polyprotic base (Kb1 = 85 107 and Kb2 = 8.9 1016). The two conjugate acids are N2H5+ and N2H62+. What is the expected pH of a 0.025 M solution of N2H4? (a) 3.83 (b) 8.32 (c) 10.16
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Explain why the following are done, both of which are related to acidbase chemistry. a. Power plants burning coal with high sulfur content use scrubbers to help eliminate sulfur emissions. b. A gardener mixes lime (CaO) into the soil of his garden.
A certain sodium compound is dissolved in water to liberate Na+ ions and a certain negative ion. What evidence would you look for to determine whether the anion is behaving as an acid or a base? How could you tell whether the anion is a strong base? Explain how the anion could behave simultaneously as an acid and a base
Identify two oxides that are key producers of acid rain. Write chemical equations that illustrate how these oxides form acid rain.
Write the ionization equation and the Ka for each of the following acids. (a) AsH4+(b) H2C3H5O7- (c) H2SO3
Pure liquid ammonia ionizes in a way similar to that of water. a Write the equilibrium reaction of liquid ammonia. b Will sodium amide, NaNH2, be an acid or a base in liquid ammonia? Why? c Ammonium chloride can be used to titrate sodium amide in liquid ammonia. Write the chemical equation for the titration of sodium amide with ammonium chloride in liquid ammonia.
Pure liquid ammonia ionizes in a manner similar to that of water. (a) Write the equilibrium for the autoionization of liquid ammonia. (b) Identify the conjugate acid form and the base form of the solvent. (c) Is NaNH2 an acid or a base in this solvent? (d) Is ammonium bromide an acid or a base in this solvent?
Arrange the following acids in order of decreasing acid strength, 1 being the weakest and 4 being the strongest. 1 2 3 4 H₂S (pKa = 7.02) HCO3- (pka = 10.33) HF (pKa = 3.17) HPO4²- (pKa = 12.38) Which of these solutions will have the lowest pH? O 0.1 M acetic acid (pka = 4.76) 0.1 M HCN (pKa = 9.21) O 1 x 10-6 M HCl O 0.1 M NH3 (pKb = 4.76)
ises 5 of 21 I Review | Constants | Periodic Table Another way to express acid strength is by using pKa: pKa = – log Ka Another way to express base strength is by using pKb: pKp = – log Kp - log Part A A new potential heart medicine, code-named X-281, is being tested by a pharmaceutical company, Pharma-pill. As a research technician at Pharma-pill, you are told that X-281 is a monoprotic weak acid, but because of security concerns, the actual chemical formula must remain top secret. The company is interested in the drug's Ka value because only the dissociated form of the chemical is active in preventing cholesterol buildup in arteries. To find the pK, of X-281, you prepare a 0.092 M test solution of X-281 at 25.0 °C. The pH of the solution is determined to be 2.70. What is the pKa of X-281? Express your answer numerically. • View Available Hint(s)
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
4.74 = For HC1O2 /KC102, pKa = 1.96; for HC10/KCIO, pKa = 7.54; and, for NH; MISSED THIS? Read Section 18.3 (Pages 799 - 802) . pKa 14.00 – pKb The following table shows the values of ionization 14.00 – 4.754 constants for a number of acids and bases at 25 9.25 °C: So, HC1O/KCIO is the best choice to create a buffer with pH = 7.30 because HC | Formula Ka value that is closest to 7.30. |НС2 Н3О2 | 1.8х 10 3 -5 HC1O2 1.1 × 10-2 NH3 1.76 x 10-5 Part B HC1O 2.9 x 10-8 For the best system, calculate the ratio of the masses of the buffer components required to ma Express your answer to two significant figures. m(KC1O) = 41.62 m(HC10) Submit Previous Answers Request Answer * Incorrect; Try Again; 3 attempts remaining

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Determine the dissociation constants for the acids. Express the answers in proper scientific notation where appropriate. Acid A: pKa = 6.0 Ka = Acid B: pK = 9.60 Ka = Acid C: pKa = -2.0 Ka =