Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound name - K Br O NH₂ ☐ Ba(OH)2 ☐ acetic acid type of compound (check all that apply) strong weak strong weak ionic molecular acid acid: base base 0 0 O 0 0 O ☐ 0 O 0 Do × 5

Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound name - K Br O NH₂ ☐ Ba(OH)2 ☐ acetic acid type of compound (check all that apply) strong weak strong weak ionic molecular acid acid: base base 0 0 O 0 0 O ☐ 0 O 0 Do × 5

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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Calculate pH of a salt solution. What is the pH of a 6.65x102 M aqueous solution of sodium hypochlorite, NACIO? (K, for HCIO = 3.5×10*) pH = Check & Submit Answer Show Approach
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Example Problem: Consider The Titration of 100.0 mL of 0.200 M CH3NH2 by 0.100 M HCl. Calculate The pH After 65.0 mL of HCl Added. (Kb for CH3NH2 = 4.4 x 10-4): a. 10.96 b. 9.75 c. 7.00 d. 3.68 e. 2.54
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Example Problem: Consider The Titration of 100.0 mL of 0.200 M CH3NH2 by 0.100 M HCl. Calculate The pH After 65.0 mL of HCl Added. (Kb for CH3NH2 = 4.4 x 10^-4): a. 10.96. b. 9.75. c. 7.00. d. 3.68. e. 2.54.
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Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Expected color at end point Volume of NaOH used (mL) 48.08 47.98 47.89 Compute for the ff: a. Average moles of acetic acid (mol)? b. Average molarity of acetic acid (M)? c. Average molarity of acetic acid (M)?
Results and Conclusion First Paragraph: First sentence matches with the first sentence of the Objective First sentence is: to identify the given ammonium salt and to determine determine its equivalent mass via acid-base titration Please calculate Average molar mass, % relative range, error, Identity of Unknown stated Second Paragraph: sources of errors discussed Please please please answer super super fast it's super important