creq2req2req#320EDAn aqueous solution contains 0.417 M nitrous acid.Calculate the pH of the solution after the addition of 5.38x102 moles of sodium hydroxide to 250 mL of this solution.(Assume that the volume does not change upon adding sodium hydroxide).pH =CSubmit Answer4RF%5Use the References to access important values if needed for this question.VRetry Entire GroupTCengage Learning | Cengage Technical SupportG65 more group attempts remainingMacBook ProBYH←&7UN▶* 008J▶1M(9K%0)OL→PVPreviousEmail InstructorT+ 11{[=NextSave and ExitO11?I11Ć

pH of buffer solution can be calculated using Henderson hasselbalch equation.

An aqueous solution contains 0.417 M nitrous acid. Calculate the pH of the solution after the addition of 5.38x102 moles of sodium hydroxide to 250 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide). pH = Submit Answer Retry Entire Group 5 more group attempts remaining

An aqueous solution contains 0.417 M nitrous acid. Calculate the pH of the solution after the addition of 5.38x102 moles of sodium hydroxide to 250 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide). pH = Submit Answer Retry Entire Group 5 more group attempts remaining

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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Please help with part b, c and d
Initial pH: 1.55 Molarity: 0.081158
22.
Calculate the pH of the solution after the following addition to the 42.0 mL of 0.135 M HCl: C) 37.8 mL 0.150 M NaOH Step 2: Identify the initial moles of each reactant. Round each answer to FIVE places post the decimal. . . 00567 Step 4: What is the pH? Round your answer to TWO places past the decimal. .00567 Step 3: Determine what is present after neutralization, and identify the conditions of this solution. choose your answer... V is present in excess. Because this solution contains choose your answer... V On the titration curve, this is at/in choose your answer... mol H+ (from HCI) mol OH (from NaOH) the solving method entails using choose your answer..... type your answer.....
Solve for question 3a, b and c
II Review | Constants | Periodic Table You may want to reference (Pages 340 - 346) Section 10.6 while completing this problem. [H3O+] = 7 x 10-8 M Express your answer using one decimal place. Calculate the pH of each solution given the following. ΑΣΦ pH = Submit Request Answer Part B [H3O*] = 2 x 10-6 M Express your answer using one decimal place. ΑΣΦ pH = Submit Request Answer
A chemist dissolves 649. mg of pure barium hydroxide in enough water to make up 90. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits. Ar Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cente Accessibiity MacBook Air DD F12 80 F7 FB esc FS F6 F4 F3 F1 F2 * & @ 23 $ delet 4 6 7 9. 1 2 3 P Q W E R Y tab 11 F G H. J K D レー .. .-
Calculate the pH of an aqueous solution of 0.2900 M sodium sulfite. pH = Submit Answer Retry Entire Group 2 more group attempts remaining
A cvg.cengagenow.com OWLV2 | Online teaching and le. Content Flipgrid | 3ffc3c3b GRLContent OWLV2 | Online tea [Review Topics) [References) Use the References to access important values if needed for this question. The compound dimethylamine is a weak base like ammonia. A solution contains 9.81×102 M (CH3),NH," and 0.400 M dimethylamine, (CH3),NH. The pH of this solution is Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next Email Instructor Save and Exit Cengage Learning | Cengage Technical Support MacBook Ai DII DD
I JUST GOT an answer, but i think it is wrong, in the answer you write: 0.233 mol/0.1 L = 0.0233 M But I get 2.33 !! that will change the pH. Please give me my question back if the previous answer was wrong. Step 1 Given that, Percentage of acetic acid solution = 14% It means, 14 g of acetic acid dissolved in 100 g or 100 mL of water. Moles of acetic acid in 14 g = 14 g/60.052 g/mol = 0.233 mol Molarity of 0.233 mol of 100 mL acetic acid solution = 0.233 mol/0.1 L = 0.0233 M Ka value of acetic acid = 1.7×10-5 Step 2 Now, acetic acid dissociates in water as follows; CH3COOH <----> CH3COO- + H+ Ka = [CH3COO- ][H+]/[CH3COOH] Let, [CH3COO- ] = [H+] = x Then we have, 1.7×10-5 = x.x/0.0233M x = 0.629×10-3 M Now, pH of the acetic acid solution will be pH = -log[H+] = -log0.629×10-3 M = 2.8
Calculate the pH of an aqueous solution that contains 0.121 M sodium sulfite and 0.448 M sodium hydrogen sulfite. pH = CHECK ANSWER
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