Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Reactant |
|
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Hydrochloric acid |
Volume used = 10ml |
|
Sodium hydroxide |
Molarity = 0.1008 |
|
Final volume = 10.7 ml |
- Calculate the molarity of the HCl solution based on the data collected from the experiment. Show your work.
- Using the molarity for HCl calculated in ( Q 2), what volume of NaOH would be required to neutralize 20mL of HCl?
- What indicates the endpoint of the titration?
You are given a concentrated solution of HCl (12 M), how would you prepare a litre of 6 M solution.
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- may want to reference (Pages 340-345) Section 10,6 while completing this problem. Part A A patient with respiratory alkalosis has a blood plasma pH of 7.50. What is the [H3O+] of the blood plasma? Express your answer to two significant figures and include the appropriate units. 6354 [H3O+]=| Value Submit μA Di Provide Feedback y₁ hr M Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining To calculate [H3O+], consider the following relationships that allow you to convert the log scale values to their correspon 10 PH 10-POH Also note that 14 = pH+pOH zel Tov- Show SA - "It Get US THIS INSTENT Ć /stane ? [H3O+] [OH-] Copyright © 2023 Pearson Education Inc. All rights reserved. I Terms of Us SAKERY hp P Pearson EST PALM B mbertan BEACHarrow_forwardConsider the following data on some weak acids and weak bases: name acid hydrocyanic acid nitrous acid solution 0.1 M KCN 0.1 M HONH3Br 0.1 M NaNO2 0.1 M KBr formula HCN HNO2 Ka 4.9 × 10 4.5 x 10 X - 10 PH choose one ✓ Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. choose one ✓ choose one choose one name S base formula hydroxylamine HONH₂ ethylamine C₂H5NH₂ | K₂ 1.1 × 10 6.4 × 10 8 4arrow_forward[H3O+1] = 10-PH [OH-1] = 10-pOH [H3O+1][OH1] = 10-14 pH - log [H3O+1] = %3D pOH = - log [OH-] pH + pOH = 14 %3D %3D What will be the pH if 0.00150 moles of HCl is added to 1.00L of water ? The reaction gives the conversion factor HCI + H2O H3O+1 + CI1 start: 0.00150 equil: O A. 1.5000 В. 2.5223 C. 2.824 D. 3.125 Е. 6.502arrow_forward
- Rate from lowest to highest, thank you.arrow_forwardConsider the following data on some weak acids and weak bases: name hydrocyanic acid acid nitrous acid 0.1 M NH4CI solution 0.1 M KBr 0.1 M CH3NH3Br 0.1 M KNO2 formula HCN Ka 4.9 × 10 HNO₂ 4.5 x 10 X - 10 -4 pH Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, '2' next to the solution that will have the next lowest pH, and so on. choose one 1 (lowest) choose one choose one name Ś base ammonia formula NH₂ Kb 1.8 × 10 -5 -4 methylamine CH3NH₂| 4.4 × 10arrow_forwardConsider the following data on some weak acids and weak bases: name hydrocyanic acid acid nitrous acid 0.1 M KNO2 0.1 M NaI solution 0.1 M CH3NH3CI 0.1 M NaCN formula Ка HCN 4.9 × 10 HNO₂ 4.5 x 10 X - 10 pH 4 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. choose one ↑ choose one ↑ choose one ↑ choose one base name ammonia formula NH3 Kh 1.8 × 10 5 -4 methylamine CH3NH₂ 4.4 × 107arrow_forward
- Consider the following data on some weak acids and weak bases: name hypochlorous acid acid hydrocyanic acid 0.1 M KI solution 0.1 M NaCN 0.1 M KCIO formula 0.1 M CH3NH3Br HCIO HCN Ka 3.0 × 10 4.9 × 10 X -8 pH - 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. choose one choose one C choose one choose one C Kb 4 methylamine CH3NH₂ 4.4 x 10 S name base aniline formula C6H5NH2 4.3 × 10 - 10arrow_forwardConsider the following data on some weak acids and weak bases: name hydrocyanic acid acid hypochlorous acid solution 0.1 M KCN 0.1 M NACIO 0.1 M HONH3Br 0.1 M KNO3 formula HCN HCIO Ka X 4.9 × 10 - 10 3.0 × 10 Use this data to rank the following solutions in order of increasing pH. In other words, elect a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. pH choose one choose one choose one choose one ✓ base Ś K₂ -8 hydroxylamine | HONH₂|1.1 × 10 pyridine name formula C₂H₂N 1.7 x 107 -9arrow_forwardPlease don't provide handwritten solution ....arrow_forward
- 2 significant digits, and Each row of the table below describes an aqueous solution at about 25 °C. r [H₂O*] to 2 Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for your entries for pH to 2 decimal places. solution [H₂O*] A 3.2 x 10 -9 PH x10 mol/L ☐ B ☐ mol/L 8 C 5.2 × 10 mol/L 4.04arrow_forwardNonearrow_forwardCH3CH2COOH Draw the Lewis structure of the acid and mark the acidic hydrogen with an asterisk (*). Draw a Lewis structure of the conjugate base of the acid. Suppose the acid is neutralized with a strong base. a) Which of the two structures you drew in 6 and 7 would be the predominant form of the species at a pH well above that at the equivalence point? b) Which of the two structures would be the predominant form of the species at a very low pH, well below that at the equivalence point and similar to the pH near the start of the titration? c) At what point in the titration, if any, would there be equal amounts of the two forms?arrow_forward
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