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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Balance the eq. by electroneutrality. solve because there is no concentrations, set up the eq. please show work Note not to A) NO3 + H₂O → NO₂¯ assume a pH of 4 B) Fe³-→ Fe²+ assume a pH of 6
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How titration technique can be used to determine the concentration of acetic acid in vinegar sample? (3 sentences)
Experiment: Determination of the dissociation constant and concentration of a weak acid
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4. 7 8. 9. 10 11 12 13 14 A solution is prepared at 25 °C that is initially 0.29M in chloroacetic acid (HCH,CICO,), a weak acid with K=1.3 x 10, and 0.18M in sodium chloroacetate (NaCH, CICO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = Submit Assignment Continue MacBook Air FI F10 80 F3 esc O00 FA F5 FI
Limit to 3 significant figures or 3 decimal places 1. A buffer is prepared containing 0.800 molar acetic acid and 1.00 molar sodium What is its pH?
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Time (sec.) pH of distilled water pH of buffered solution 20 7.99 8.61 40 7.46 8.43 60 7.15 8.31 80 6.75 8.22 100 6.54 8.16 120 6.39 8.10 140 6.22 8.05 160 6.11 8.01 180 6.03 7.97 Conclusion Explain your observations from the data table. Which resists a change in pH the most, water or the buffered solution? Give reasons. When you blow into the water, the pH goes up. Is the solution becoming more basic or acidic? A buffer is usually made of a weak acid and a weak base. When you blow into a buffer the pH doesn’t change. What do you think is happening?
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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)?