What the class of organic compound is UNKNOWN D based on the given qualitative tests below: UNKNOWN 2% AgNO3 litmus paper test HYDROXAMIC TEST clear solution acidic burgundy solution burgundy solution burgundy solution bluish-red colored complex clear solution acidic white ppt clear solution C acidic basic acid anhydride ester alcohol amide

What the class of organic compound is UNKNOWN D based on the given qualitative tests below: UNKNOWN 2% AgNO3 litmus paper test HYDROXAMIC TEST clear solution acidic burgundy solution burgundy solution burgundy solution bluish-red colored complex clear solution acidic white ppt clear solution C acidic basic acid anhydride ester alcohol amide

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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Phenolphthalein reacts to basic solutions (pH above 7) by changing to a pink color. If you had phenolphthalein in both an acidic (~6 pH) solution and an even more acidic solution (~5 pH), which solution would take more NaOH (a basic substance) to turn the solution pink?
Data Sheet: Unknown acid #9 Mass of the Unknown acid: (letter or number on the unknown bottle) Volume NaOH added pH 0.5ml 364 3.26 mi 3.69 3:24 3:26 TEST 2.0ml 2.5ml 3.0ml 3.5ml tom? 4.5ml 5.0ml tus's 6.0m) 6.5ml 1.0m) 7.5ml 8.5ml 9.0m 9.5m1 100ml 10.5 ml 11.0m 11.5MI 12.0ml 12.5 ml 13.0 ml B.5 ml 14.0 ml 145 ml 2 Concentration of NaOH(aq): 0.209 15.0 ml 3:28 3:28 3:30 3:35 3:44 3,39 TSE est 3.54 3.58 3.64 3.72 3.80 3.867 3.93 $ 4.00 4.061 4:13 473 4.20 4.28 T 4.35 4.43 4.46 4.64 4.83 5.05 2.93 9.91 Volume NaOH added 15.5ml 16.0 ml 16.5ml 17.0m1 17.5ml 0.0995M pH 10.63 10:03 11.25 11.37 11.50 4
Use the References to access important values if needed for this que Assign each species on the left to a category on the right. HNO2 Ba(OH)2 NO₂ C6H5COOH tv Submit Answer Retry Entire Group Cengage Learning Cengage Technical Support S 0 strong acid weak acid strong base Clear All weak base 2 more group attempts remaining Previous P
Use the information in the pK table to rank the molecules in order of decreasing basicity. For example, select "1" in the second column for the strongest base a and "2" for the next strongest base and so on. CH3 HS F CH,CO, Molecules (Choose one) (Choose one) (Choose one) (Choose one) X Ś CHA 4 NH₂ H₂ CH3NH₂ 2 48 38 36 33 pk table pKa CH,NH, CH₂SH 10.4 H₂O* HCN + 10.6 9.4 NH H₂O 15.7 H₂S CH₂OH 15.5 CH,CO,H 4.76 9.2 7.00 HF CH₂OH₂ H₂SO4 HC1 HBr 3.17 -1.7 -2.2 -3.0 -7 -9
PLEASE ANSWER QUESTION 7 SHOW SOLUTION THANK YOU i WILL RATE YOUR ANSWER
In an aqueous solution of a certain acid the acid is 0.22% dissociated and the pH is 4.39. Calculate the acid dissociation constant K of the acid. Round answer to 2 significant digits.
Hi can you answer the following question: Using the data from questions 3 and 4, calculate the experimental value of Ka for this unknown acid using an ICE table. The data from question 3 and 4 are attached. Thank you! Aditional information if needed: unknown acid concentration: 0.042mol/L unknown acid volume: 0.25L NaOH concentration: 0.1M NaOH volume at the equivalence point: 0.105L Initial [H30+] is 5.01 x 10-4 mol/L
Unknown Acid Acid name Acetic acid Group #5 Group #6 Group #7 Mean Standard Deviation % Error STATISTICAL ANALYSIS: Calculate mean values for molar mass, pKa, and Ka. Calculate % error and standard deviation: Unknown acid # 1 Molar Mass of unknown acid (calculated), g/mol Group #1 Group #2 Group #3 Group #4 Reaction Initial conc. / M: Change in conc. at equilibrium / M: Equilibrium conc. / M: Acetic acid | Molar Mass, g/mol: 60.05 | pka = 4.76 Accepted Values Molar mass, g/mol 60.05 Ka = Part II 1. Using initial molarity of acid and measured pH of the acid before titration, build a RICE table and calculate the Ka of the acid. You can use examples 1, 2 (pp. 3-4) from the Manual (posted on Canvas) Initial Molarity of [HA], M 0.219 Initial pH of Acid pka = HA(aq) + H₂O(1) [HA] -X 58.8 57.4 60.4 61.0 58.4 59.2 59.7 59.3 1.13 0.01 [HA] + X 台 pH: H3O+ (aq) = 0 +X 2. Use the Henderson-Hasselbauch equation to perform the same calculation. +X pka 4.76 Ka = pka 4.78 5.00 4.64 4.89 4.62 4.68 4.82…
Question Completion Status: QUESTION 19 Based on the acid dissociation constants (Ka) given, which of these acids is the strongest? CH3 COOH (Ka = 1.7 x 10-5) o Hz PO4 (Ka = 6.3 x 10-8) O NH4* (Ka = 6.3 x 10-10) HNO2 (Ka = 5.1x 10-4) %3D O HCO3 (Ka = 5.0x 10-11) %3D QUESTION 20 Click Save and Submit to save and submit. Click Save All Answers to save all answers. prt sc
Post-lab Question #3: Compare with the pH of a 0.1 M solution of KC2H3O2, the pH of a 0.1 M solution of NaC2H3O2 is (same/higher/lower)
Water solution of an unknown compound is basic. When a small piece of solid is heated in a dry test tube, water droplets are observed around the sides of the test tube. Which compound is it? a. Na2B4O7. 10H2O b. K2C2O4 c. CuSO4.5H2O d. H2C2O4 Clear my choice
Hadising Name: 2: Hailey Gary H3C Pre-Lab: Determination of Vinegar Acidity by Titration RES 1. Complete the following neutralization reaction. Identify the weak acid and conjugate base. O Acidic proton OH + OH + Nat Acetic Acid CHM 102