constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 2 3 NEXT > The Ka for CH3COOH is 1.8 x 10-5. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0] [0.300 -x] 1.8 x 10-² [0.300] [0.0300 + x] 5.6 x 10-1⁰ 0 2.75 Kb 1.30 x 10-² [0.0300] [0.0300 -x] 5.6 x 108 5.04 [0.150] [0.150 + x] A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 0.523 8.96 < PREV 1 3 Based on your ICE table and the equilibrium expression for Kb, determine the pH of this solution at the equivalence point.. 2 [0.0150] [0.150 -x] pH = 1.20 11 7.72 x 10-1⁰ 4 [x] [2x] [0.0150+x] [0.0150 -x] 4.89 RESET [0.300 + x] 1.8 x 10-5 11.3 RESET 9.11

constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 2 3 NEXT > The Ka for CH3COOH is 1.8 x 10-5. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0] [0.300 -x] 1.8 x 10-² [0.300] [0.0300 + x] 5.6 x 10-1⁰ 0 2.75 Kb 1.30 x 10-² [0.0300] [0.0300 -x] 5.6 x 108 5.04 [0.150] [0.150 + x] A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 0.523 8.96 < PREV 1 3 Based on your ICE table and the equilibrium expression for Kb, determine the pH of this solution at the equivalence point.. 2 [0.0150] [0.150 -x] pH = 1.20 11 7.72 x 10-1⁰ 4 [x] [2x] [0.0150+x] [0.0150 -x] 4.89 RESET [0.300 + x] 1.8 x 10-5 11.3 RESET 9.11

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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Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. CaCl2 3C,2- Reset > 1 3 4 6 7 8. 9. + ) (s) (1) (g) (aq) NR Са OH- CI H¿O x H20 Tap here or pull up for additional resources LO 2.
Maps [References] Suppose you want to make a CH3 COOH/CH;COO¯ buffer solution with a pH of 5.11. The acetic acid concentration is to be 0.27 M. What should the acetate ion concentration be? (pK,(CH3 COOH) = 4.74.) %3D Concentration %3D
7:30 1 y gmail x H Folde x A FINAL X E Prese x Prese x E PRESE X * Ceno x Y short x RI Anno x w weba x y chem x à app.101edu.co Time's Up! Write the acidic equilibrium equation for CH.NH:. 1 3 4 5 6 8 9 Os + (s) (1) (g) (ag) HO OH H:O H Reset • x H:O Delete (0) 7°C Mostly doudy a O od0 ENG P Type here to search
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6. Open the bags and add 3 drops of bromothymol blue to each bottle. The indicator turns yellow if vinegar is still present and is blue-green when vinegar is not present. Record the color of each solution in the table provided. Data Table 1: Reaction Data Sample 7. Add a 4 teaspoon of baking soda to each bag. Effervescence of CO₂ occurs if excess vinegar is present. Record your observations in the table provided. Moles of vinegar (mol) Moles of baking soda (mol) mistry Relative size of bag Was excess vinegar present? Color with indicator? Reacts with additional baking soda? Moles of gas produced (mol) Watch the limiting reagent! #1 0.042 0.014 чем yes yellow #2 0.042 0.028 #3 yes yellow 0.042 0.042 Experiment 11 yes yellow #4 Stoichiometry 0.042 0.88 more small big bigger bigger No 0.071 #5 NO Geen 0.042 Blue Calculations 1. Use Table 1 to determine which reactant was limiting in each trial. Use the amount of limiting reactant to calculate the moles of carbon dioxide gas that were…
in le chatelier lab a student found the equilibrium constant for HB-(aq) + H2O (l) --> H30+ (aq) + B2- (aq) to be 2.33 *10 ^ -9 if the student were to add acid to a flask of this mixture at equilibrium what effect will this have on the ratio of reactants to products? give as much detail as possible please
A 0.0614 M solution of butyric acid, C₂HCOOH is 0.066 % ionized. a) Calculate concentration at equilibrium for each reagent. Report your answer to 4 significant figures. [C₂H₂COOH] = [H₂O¹] = [C₂H,COO]=[ M M b) What is the pH of the acidic solution? c) What is K, of the acid? 2.68-10 06.09-108 pH = 02.57-10 0.0613 01.01-10-10
$ 4 The value of K, for hypochlorous acid, HCIO, is 3.50x10-8. Write the equation for the reaction that goes with this equilibrium constant. (Use H3O+ instead of H*.) 000 000 F4 R F Submit Answer % + 5 T G FS Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining A Cengage Learning Cengage Technical Support 6 MacBook Air Y F6 H 87 & + F7 U * 8 F8 9 K >> F9 O 0 F10 P F11 Previous + Next> Save and Ex F12 11
tab esc For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp compound 1 CaBr, CaCO3 Ca (OH)₂ Q Does solubility change with pH? 2 O yes O no O yes no -0. F2 yes W no # 3 pH = 7 80 F3 E highest solubility pH = 8 $ 4 X 000 F4 R pH = 9 % 5 S F5 T MacBook Air < F6 Y & 7 AA F7 U 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility * 00 8 DII F8 9 Save For Later F9 Submit Assignment F10 P F11 + 11 { [ 000 18 Ar F12 ?
Determine the Kb for an unknown base by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > The pH for a 0.185 M solution of an unknown weak base, B, is 12.95. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) B(aq) + H₂O(1) = OH-(aq) + BH*(aq)
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