QUESTION 3What is the equilibrium constant expression (Ka) for the acid dissociation of nitrous acid HNO 2? The equation of interest isHNO 2( aq) +H 2O()=H30 *(aq) + NO 2 (aq).O Ka ((H30*)[NO2 )/([HNO2])O Ka ((H3O*][NO2 )/([HNO2][H2O])O Ka ((HNO2]|[H20]]/[H3O*][NO2)O Ka ([HNO2)/([H3O*][NO2"])%3D%3DClick Save and Submit to save and submit. Click Save All Answers to save all answers.MacBook AirDIIF8F9F7F6F5F4F3F2&C@2324234.ET00

Ka is the dissociation constant of an acid and it is ratio of dissociated and undissociated acid at equilibrium For liquids and solids consider unity Ka = [product ]eq / [reactant]eq Ka = ([ H3O+] [NO2-] )/ ([ HNO2]) Hence answer is Ka = ([ H3O+] [NO2-] )/ ([ HNO2])

Science

Chemistry

QUESTION 3 What is the equilibrium constant expression (Ka) for the acid dissociation of nitrous acid HNO 2? The equation of interest is HNO 2( aq) + H 20()H 30 *(aq) + NO 2 "(aq). O Ka = (H30*INO02/([HNO2) O Ka = (H3O*IN02/([HNO2][H2O) O Ka = (HNO2||H20])/([H3O*J[NO2) O Ka = (HNO2)/([H30*)[NO2) Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air

QUESTION 3 What is the equilibrium constant expression (Ka) for the acid dissociation of nitrous acid HNO 2? The equation of interest is HNO 2( aq) + H 20()H 30 (aq) + NO 2 "(aq). O Ka = (H30INO02/([HNO2) O Ka = (H3OIN02/([HNO2][H2O) O Ka = (HNO2||H20])/([H3OJ[NO2) O Ka = (HNO2)/([H30*)[NO2) Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air

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...

See similar textbooks

Similar questions

Question 5 of 8 Submit Construct the expression for Ka for the weak acid, HC,H,O4. HC3H,O,(aq) + H,O(1) = H;O*(aq) + C3H,O,-(aq) 1 Based on the definition of Ka, drag the tiles to construct the expression for the given acid. Ka = 5 RESET [H,O] [H,O*] [OH] [HC,H,0,] [H,C,H;O,'] [C,H,O,] 2[H,O] 2[H,O*] 2[OH-] 2[HC,H,O,] 2[H,C,H,0,"] 2[C,H;O,] [H,O]? [H,O*)? [OH]? [HC,H,O,]² [H,C,H,O,*]? [C,H;O, ]²
Part B Fe* (aq) + 6H2O(1) = Fe(H20),* (aq) O H20 is the Lewis Acid and Fet is the Lewis Base O Fet is the Lewis Acid and H20 is the Lewis Base
What the heck is pKa? Well, pKa is the negative log of Ka: pKa = - log (Ka)Nifty, but what the heck is Ka? Ka is the equilibrium constant expression for the reaction of a weak acid with water. (aren't you glad you took this course?) For instance: H2CO3 (aq) + H2O (l) double arrows HCO3- (aq) + H3O (aq)Given all of this fun info, why does the equation for the Ka of carbonic acid not include water? Water is a reactant Water can evaporate Water is a pure liquid The equation can be written without including the water
Which of the acids listed below has the weakest conjugate base? O O HBr, K₂ = 10+9 O H3PO4; K₂ = 7.520x10-3 O HNO3; Ka = 20 H2O2; Ka = 2.400x10-12
Question 17 On acidity and basicity of aqueous solutions, the following relationships are valid, except Каx Къ - 1.0х 10-14 If pOH< 7, then [H*] < [°OH]; more basic for a weak acid and its conjugate base: pka + pkb=pKyw [H*]rOH] = 1.0 x 10-14 =Kw pH + pOH = 14 for a weak base: ↑Kp. + pKp, more basic, more ["OH] If pH < 7, then [H*] < [°OH]; more acidic
What is the concentration of OH- in 0.1863 M HNO2 ? See reaction belowHNO2 + H2O ↔ NO-2 + H3O+ Ka = 4.600x10-4
Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species N₂ CHẠNH, CH₂CH₂COO HN₂ ОН H₂O CH₂CH₂COOH + relative pH of 0.1 M aqueous solution 6 5 (Choose one) (Choose one) 8 (highest) (Choose one) 3 X ? 00. 18 Ar
What are the products of the acid-base reaction: H₂S (aq) + HO¯ (1) OH2 H2SO OH3SO H3O^+ H3S^+ HS^- H2O 02 OS^2- ?
6:15 Question 18 of 22 Construct the expression for Ka for the weak acid, HC,H,O4. Ka = HC,H,O,(aq) + H2O(l) = HgO*(aq) + C,H,O, (aq) 1 Based on the definition of Ka, drag the tiles into the numerator or denominator to construct the expression for the given acid. Submit [H₂O] [H3O+] [OH-] [H₂C9H₂O4*] [C₂H₂O4] 2[H₂O] 2[OH-] 2[HC₂H₂O4] 2[H₂C9H₂O4*] [H₂O]² [H3O+]² [OH-]² [H₂C9H₂O4*]² [C₂H₂O₂-]² Tap here or pull up for additional resources RESET [HC₂H₂O4] 2[H3O+] 2[C9H₂O4] [HC,H,O]
Calculate the hydroxide ion concentration for a solution with [H3O+]eq = 2.8 × 10-5 M. Use "E" for scientific notation. i Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105)
Gen Chemistry 2, Q5
[H₂O] 2[OH-] [NH₂)² Construct the expression for Ka for the weak acid, NH4*. NH4+ (aq) + H₂O(1) H3O+ (aq) + NH3(aq) Based on the definition of Ka, drag the tiles to construct the expression for the given acid. [H₂O*] 2[NH₂*] [NH₂-]² Ka [OH-] 2[NH3] = [NH₂*] 1 2[NH₂] [NH3] [H₂O]² [NH₂] [H3O+]² 2[H₂O] [OH-]² RESET 2[H3O+] [NH₂*]²