* OWLV2 | Online teachinX C The Deep Blue Compound (+ https://cvg.cengagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locator=Dassignment-take&takeAssignmentSessionLocator=assignment-take [References] You have 250, mL of 0.164 M HCI Using a volumetric pipet, you take 25.00 mL of that solution and dilute it to 100.00 mL in a volumetric flark Now you take 5.00 mL of that solution, using a volumetric pipet, and dilute it to 100.00 mL in a volumetric flask. What is the concentration of hydrochloric acid in the final solution? Concentration- Submit Answer Try Another Version 9 item attempts remaining KPrevious Next

* OWLV2 | Online teachinX C The Deep Blue Compound (+ https://cvg.cengagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locator=Dassignment-take&takeAssignmentSessionLocator=assignment-take [References] You have 250, mL of 0.164 M HCI Using a volumetric pipet, you take 25.00 mL of that solution and dilute it to 100.00 mL in a volumetric flark Now you take 5.00 mL of that solution, using a volumetric pipet, and dilute it to 100.00 mL in a volumetric flask. What is the concentration of hydrochloric acid in the final solution? Concentration- Submit Answer Try Another Version 9 item attempts remaining KPrevious Next

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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we found that the percent ionization of niacin 1Ka = 1.5 * 10-52 in a 0.020 M solution is 2.7%. Calculate the percentage of niacin molecules ionized in a solution that is (a) 0.010 M
http://chemcollective.org/activities/vlab/3 Virtual lab
Part B A solution has [H3O+] = 4.2x10-5 M. Use the ion product constant of water Kw = [H3O+][OH¯] to find the [OH-] of the solution. Express your answer to two significant figures. • View Available Hint(s) ? [OH-] = M %3D Submit Part C A solution has [OH¯] = 2.1x10-2 M . Use the ion product constant of water Kw = [H3O+][OH-] to find the [H3o*] of the solution. Express your answer to two significant figures. • View Available Hint(s) | ? [H3O*] = M
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docs.google.com a No one of these O If you have a solution (1M) Hydrochloric acid in (250mL), and lg abäi you want to prepare (0.5M) HCL in (100mL), the volume you will take is * 125mL O 0.5L O 50mL O 100mL O
0/1 E View Policies Show Attempt History Current Attempt in Progress Consider the following solutions: Solution 1:0.100 L of 0.25 M NaCH3CO2 + 0.050 Lof 0.25 M HCI Solution 2:0.100 L of 0.25 M HCH3CO2 + 0.050 L of 0.25 M NaOH Part 1 Incorrect. How many moles of acid does it take to change the pH of the original Solution 1 by 0.28 pH units?
Please don't provid hand writtin solution...
he X - OWLV2 | Assigr x : OWLV2 | Online X y! google - Yahoc X e Registration - L X O selfserve.una.e X Irn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. A buffer solution is 0.478 M in H2SO3 and 0.380 M in KHSO3. If K for H2SO3 is 1.7 x 10-2, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group 9 more group attempts remaining 5:05 P 11/2/20 Cop fi2 ort sc delete home ho backspace num Iock
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Solution give me properly part a and b
Cours Courseld= 165945 XupenvellumHMAC=Tc/db25d9d903b3 •.. KAssignment 4 Item 23 23 of 42 Review Constants | Periodic Table A 0.100 M solution of bromoacetic acid (BrCH2COOH) is 13.2% ionized. A COMMUNITY COLLEC Part A Calculate (H]. ourses Express your answer to three significant figures. rse Home ? ΑΣφ C Custom eText M [H*] =
HOWICX S Geometry w/Datax S Practice 10.10 | Sex S Practice | SchoolcX G Sign in - Google/X Logins & Passwo X + gagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator= assignment-take ★ Other Booki [Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution contains 0.493 M C6H5NH3Br and 0.337 M C6H5NH2 (aniline). Determine the pH change when 0.088 mol NaOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change Submit Answer Retry Entire Group 1 more group attempt remaining HANA D ?? ak