16. Which of the following water-soluble compounds would cause a significant decrease in pH when dissolved in water? 9 CH₂CH₂C-OH CH3 "CH, -NH, CH3 -CH₂-OH more than one response is correct no correct response 17. Athlete's foot can be treated with which carboxylic acid salt? Osodium stearate O calcium propanoate O sodium benzoate zinc-10-undecylenate

16. Which of the following water-soluble compounds would cause a significant decrease in pH when dissolved in water? 9 CH₂CH₂C-OH CH3 "CH, -NH, CH3 -CH₂-OH more than one response is correct no correct response 17. Athlete's foot can be treated with which carboxylic acid salt? Osodium stearate O calcium propanoate O sodium benzoate zinc-10-undecylenate

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...

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The value of Ka for benzoic acid is 6.30×10-5.What is the value of Kb, for its conjugate base, C6H5COO-? The value of Ka for acetylsalicylic acid (aspirin) is 3.00×10-4.What is the value of Kb, for its conjugate base, C9H7O4-? The value of Ka for acetic acid is 1.80×10-5.What is the value of Kb, for its conjugate base, CH3COO-?
I only need help with problem 4 please. 3. The concentration of carbonic acid, H2CO3, in a typical carbonated drink is approximately 7.0 x 10-2 M. Carbonic acid is a diprotic weak acid with the following pKa values for the 1st and 2nd ionizations: H2CO3 + H2O <===> H3O+ + HCO3- pKa = 6.3 HCO3- + H2O <===> H3O+ + CO32- pKa = 10.3 From highest concentration to lowest concentration, what are the molecular and ionic species present in an aqueous solution of 7.0 x 10-2 M H2CO3 (note: you do not have to calculate the concentrations, just rank them in order of highest to lowest). 4. What is [H3O+] and the pH of a solution of H2CO3 with [H2CO3]Total = 4.5 x 10-4 M? (Use the pKa value for H2CO3 given in Problem 3.) Hint: This is not a buffer.
pH = 10.31 Use the following table to predict the best acid/ base pair for the desired pH/pOH values below (hint: remember buffer range = ± 1 pKa unit). Acid Base Name Acid Base pKa Hydrochloric acid HCl Cl- -7.00 Phosphoric acid H3PO4 H2PO4- 2.12 Hydrofluoric acid HF F- 3.18 Lactic acid Lactic acid Lactate 3.85 Acetic acid CH3COOH CH3COO- 4.74 Carbonic acid H2CO3 HCO3- 6.36 Dihydrogen phosphate H2PO4- HPO42- 7.21 Ammonium NH4+ NH3 9.25 Hydrocyanic acid HCN CN- 9.31 Bicarbonate HCO3- CO32- 10.25 Methylammonium ion CH3NH3+ CH3NH2 10.62 Hydrogen phosphate HPO42- PO43- 12.38
What is the [H+] (M) of a weak basic solution with a concentration of 1.4 × 10-2 M and Kb is 6.4 × 10-4 at 25.0 °C? 1.4 × 10-2 2.7 × 10-3 3.0 × 10-3 3.3 × 10-12 11.43
solution made with 0.126 moles of a triprotic acid dissolved in 180 mL of solution has the following KA's... (rest in pic) please answer
Solve the following: A solution of ammonia is 3.2% ionized at 25.0°C. What was the original concentration (in M) of the ammonia solution? The Kbat 25.0°C for ammonia is 1.8×10-5. Calculate the pOH of 0.716 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for aniline is 3.83 × 10-4.
How many equivalents of K+ and SO42- are in 1.0 L of 1.0 M solution of K2SO4? Question 3 options: 1.0 Eq K+ 1.0 Eq SO42- 1.0 Eq K+ 2.0 Eq SO42- 2.0 Eq K+ 2.0 Eq SO42- 2.0 Eq K+ 1.0 Eq SO42-
Question:Codeine is a weak organic base with a Kb = 1.6 x 10-6 C18H21NO3(aq) + H2O(l) ⇌ C18H21NO3H+(aq) + OH-(aq) 1. What are the values of pKa and pKb? 2. Calculate the equilibrium concentrations for [C18H21NO3(aq)], [C18H21NO3H+(aq)], and [OH-(aq)] if the initial concentrations are [C18H21NO3(aq)]o = 0.1 M [C18H21NO3H+(aq)]o = [OH-(aq)]o = 0.01 M 3. What is the pH of the given codeine solution? Please answer all sub-parts.thanks
The Kb of (CH3)3N is 6.4 x 10 -5. Calculate the pH of a 0.10 M solution of (CH3)3NH +. (answer: 4.40)
Betaine hydrochloride (C5H11NO2HCl) dissolves according to Reaction 5.1 below. Reaction 5.1: C5H11NO2HCl (s) → C5H11NO2 (aq) + H+ (aq) + Cl- (aq) How many milligrams of betaine hydrochloride (C5H11NO2HCl) would you need to ensure a patient with 50.0 mL of gastric acid has a pH of 2.0?
3) A solution contains0.023Macetic acid and0.0.018Msodium acetate. The Ka for acetic acid is1.8×10−5. What is thepHof the solution? ( Please type answer note write by hend )
Part D Part complete Pancreatic juice, pH = 7.9 Pancreatic juice, = 7.9 acidic basic SubmitPrevious Answers Correct Part E Part complete Estimate [H3O+] value for pancreatic juice. Express your answer using one significant figure. [H3O+] [H3O+] = 1×10−8 M SubmitPrevious Answers Correct Significant Figures Feedback: Your answer 1.26⋅10−8 = 1.26×10−8 M was either rounded differently or used a different number of significant figures than required for this part. Part F Estimate [OH−] value for pancreatic juice. Express your answer using one significant figure. [OH−] [OH−] = nothing M