SOLUBILITY TEST distilled water Litmus paper test OBSERVATIONS clear, colorless solution no change in either red or blue litmus +/- CHEMICAL TEST Molisch test Ninhydrin test 2,4-DNP test hot acidic KMN04 iodoform test +/- OBSERVATIONS turbid colorless solution clear pale-yellow solution clear orange-yellow solution clear purple solution clear pale-yellow solution 4. based on the results, what is the most probable structure of C4H100? Draw it using line-bond and lewis structure

SOLUBILITY TEST distilled water Litmus paper test OBSERVATIONS clear, colorless solution no change in either red or blue litmus +/- CHEMICAL TEST Molisch test Ninhydrin test 2,4-DNP test hot acidic KMN04 iodoform test +/- OBSERVATIONS turbid colorless solution clear pale-yellow solution clear orange-yellow solution clear purple solution clear pale-yellow solution 4. based on the results, what is the most probable structure of C4H100? Draw it using line-bond and lewis structure

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 show all work. 1. estimate the position of the equivalance point 2. estimate the position of the half-equivalance point 3. calculate the percent error in the experimental pKa value (accepted pKa value is 4.75) 4. Identify the buffering region 5. Identify the volme ranges that corresponed to the initial color and the final color of the indicator Volume pH 0 2.88 0.05 2.9 0.14 2.95 0.55 3.14 1.15 3.35 1.45 3.44 1.97 3.56 2.36 3.63 2.77 3.69 3.17 3.75 3.78 3.84 4.09 3.86 4.59 3.92 5 3.98 5.39 4 5.8 4.03 6.3 4.09 6.6 4.11 6.99 4.13 7.5 4.17 8.01 4.22 8.31 4.23 8.8 4.27 9.2 4.3 9.5 4.3 9.91 4.34 10.53 4.37 10.92 4.4 11.33 4.41 11.63 4.44 12.14 4.47 12.53 4.47 12.94 4.51 13.35 4.52 13.74 4.56 14.14 4.56 14.54 4.59 15.04 4.62 15.33 4.64 15.73 4.65 16.22 4.67 16.62 4.71 17.02 4.72 17.33 4.73 17.73 4.75 18.34 4.79 18.63 4.8 19.02 4.82 19.43 4.84 19.92 4.88 20.33 4.9 20.73 4.92…
E 20 2 For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities. (If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.) C F3 Submit Answer 54 Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water. iron (II) hydroxide silver cyanide Ksp = Ksp = $ DOD F4 R F V % 5 Retry Entire Group 9 more group attempts remaining T Note: Multiply out any number and put it first in the Ksp expression. Combine all exponents for s. F5 G Cengage Learning Cengage Technical Support 1. Iron(II) hydroxide 2. silver cyanide ^ 6 B MacBook Air F6 Y H & 7 44 N F7 U J * 00 values if needed for this question. 8 F8 1 M ( 9 K A. Pb(OH)2 B. MgCO3 C. COCO3 D. CrPO4 F9 O ) 0 J F10 P - - ; F11 { alf Previous [ + = ? Next> Save and Exit 4) F12 11 " } 1 delete
[References] A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows: Methyl violet: violet Thymol blue: yellow Methyl yellow: orange Congo red: violet Bromocresol green: yellow What is the approximate pH of the solution? Submit Answer Try Another Version 10 item attempts remaining
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5ml = volume acid/base used to adjust 4.76 HCL concentration = 1.0 M acetate buffer = 0.1 M
6:32 SIMULATION Buffer Solutions Ireterences] -0 14-LO 14-Lo 7.00 1 7.00 4.74 1.0 M HCI 1.0 M NaOH 1.0 M HCI 1.0 M HCI Add 1.0 M NaOH 1.0 M NaO Add Add Add Add Add 10. ml 10. ml 10. ml 10. mL 10. ml 10. mL Initial Solution 100 mL Initial Solution 100 mL. 1.0 M NaCl Initial Solution 100 mL 1.0 M CH,CO,H(aq) 1.0 M NaCH,CO(ag) pt H,0 pr What is the pH of the acetic acid acetate mixxture after the addition of 10 ml of 1.0 M HC12 pt pt >(4 of 8) Check pt pr Submit Answer Try Another Wersion 10 item attempts remaining
From the given information in the table calculate for both titration1 and 2: 1)moles of thiosulphate titrated (mols) 2) moles of hypochlorite (mols) 3) mass of sodium hypochlorite (g) 4) wt% of sodium hypochlorite
Part B: Molar Solubility of Ca(OH): in presence of Ca Temperature of the Experiment:24.6°C Concentration of HCI(ag): 0,05M Trial 1 Trial 2 1) Volume of Saturated Ca(OH)2 solution used 10.05 ml 10.14ml 2) Initial Buret Reading (mL) 11.45 ml 14.85 mL 3) Final Buret Reading (mL) 14.85 mL 18.81 ml 4) Volume of Added HCI (mL) 5) Mole of Added HCI 6) Mole of OH in Ca(OH)2 + Ca" solution 7) Concentration of [OH] (mol/L) 8) Concentration of [Ca) (mol/L) 9) Molar Solubility of Ca(OH): (mol/L) 10) Average Molar Solubility of Ca(OH):
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One of the following statements is incorrect: oStandardization is not required when the titrant solution molarity is approximate O Back-titration is required when the rate of the reaction slow O A primary standard should be highly pure, has atmospheric stability and absence of hydrated water oTitration error is the difference between equivalence point volume and end point volume O A standard solution should react completely with the analyte with a definite chemical equation
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