MasteringChemistry: CHE154 SXsession.masteringchemistry.com/myct/itemView?as w?assignmentProblemlD3D142965856CHE154-H Gen Chem II Bronikowski S20IReview IPart ApH = 8.78%3DExpress your answer using two significant figures. Enter your answers numerically separated by a comma.ΑΣφ[H3O*), [OH ] =%3DSubmitRequest AnswerPart B

The pH of the solution can be defined as the negative of the logarithm of [H3O+]. Mathematically, it…

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MasteringChemistry: CHE154 SX session.masteringchemistry.com/myct/itemView?as

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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OpenVellumHMAC=defce5f03204e95efa2fcf11b1ecff98#10001 I Review | Constants | Periodic Table [base] pH = pK, + log Tacid 3.5 x 10 2 -log(1.8 x 10-5)+ log 0.1025 4.74 – 0.467 4.28 Part C For 500.0 mL of a buffer solution that is 0.185 M in CH,CH,NH, and 0.135 M in CH3CH,NH CI, calculate the initial pH and the final pH after adding 2.0x10-2 mol of HCl (K,(CH CH,NH,) = 5.6 x 10 4) Express your answers using two decimal places separated by a comma. pHinitial. pHrinal 10.89, 11.12 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Provide Feedback Next > P Pearson at © 2022 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions Contact Us 11:57 PM 4/16/2022 lyp DDI C dele %3D backspace 00
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30 ml of 0.1 M NAOH is added to 28 ml of 0.10 M HCI (post e.p). What is the pH?
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A webassign.net VA Test #2 (Chapters 14 & 15)- CHM 152, section HYD1A, Spring 2021 | Web... Summary (B)-10: Business Management II - Stickney -1(A-E) Course: 2021SP General Chemistry II (CHM-152-HYD1A) Please use the values in the resources listed below instead of the textbook values. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ken for each of the slightly soluble solids indicated. ds, (a) PBSO4 [Pb2+] = 3.7x10-3 M, [SO,2-1 = 6.8× 10-6 M %D %D 4.0 (b) PBF2 [Pb2+] = 2.0x10-3 * M, [F] = 4.0x 10-3 M 4.0 (c) Ag,Cro4 [Ag*] = 1.9x10-5 M, [Cro,2-1 = 3.1x 10-3 M = 1.9x 10-5 4 4.0 (d) Y(OH)3 = 3.6x 10 16 M, [OH ] = 6.5x10-3 M 4.0 (e) AgBr [Ag+] = 7.3x10-7 M, [Br-] = 7.3x 10-7 M 4.0 Supporting Materials Periodic Table Constants and I Supplemental Data Factors Additional Materials Section 15.1
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7. Refer to the following table: Table 2-2. Change in pH of 0.2 M Acetate Buffer after addition of Acid or Base [Base]:[Acid] 0.005:0.195 Addition pH HC1 0.095 mol 3.1 HC1 0.075 0.025:0.175 3.9 HС1 0.05 НС1 0.025 0.05:0.15 4.2 0.075:0.125 4.5 0.1:0.1 0.125:0.075 4.7 NaOH 0.025 mol 4.9 NaOH 0.05 mol 0.15:0.05 5.2 NaOH 0.75 mol 0.175:0.025 5.5 NaOH 0.095 mol 0.195:0.005 6.3 a. Calculate the pH of a 0.2 M acetate buffer (a solution containing 0.1 mol L-' acetic acid and 0.1 mol L-1 sodium acetate), given that the pKa of acetic acid is 4.7. b. What would be the pH value after adding 0.05 mol of NaOH to 1 L of 0.2 mol L1 acetate buffer? c. Compare the pH value in (b) with that obtained after adding 0.05 mol NAOH to 1 L of water (a simple solution of 0.05 mol L-' NaOH). d. How much acid or base can be added to 1 L of the 0.2 M acetate buffer so that the pH does not change appreciably (i.e., what is its buffer range)?
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MeH When two Lewis bases are compared in the reaction with the given Lewis acid, what difference can you expect in any aspect of the reaction? Explain the difference with the proper theoretical principle. OLi Et VS Me H. Br OLi CS Scanned with CamScanner