⚫ To 3 mL of 0.10 M HC_H₂O2 add a drop of methyl orange, then add 1 M NaC HO₂ a few 3 2 3 drops at a time, with mixing. Explain your observations in terms of the equilibrium equation and the common ion effect. • Write the equilibrium equation and explain your observations in terms of the equilibrium equation and the common ion effect in your notebook.

⚫ To 3 mL of 0.10 M HC_H₂O2 add a drop of methyl orange, then add 1 M NaC HO₂ a few 3 2 3 drops at a time, with mixing. Explain your observations in terms of the equilibrium equation and the common ion effect. • Write the equilibrium equation and explain your observations in terms of the equilibrium equation and the common ion effect in your notebook.

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 7RQ: Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations...

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What do you suppose happens to the Ksp, value of a solid as the temperature of the solution changes? Consider both increasing and decreasing temperatures, and explain your answer.
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Which compound in each of the following pairs of compounds is the more soluble one? a silver chloride or silver iodide b magnesium hydroxide or copper(II) hydroxide
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A 1.00 liter solution contains 0.59 M nitrous acid and 0.44 M sodium nitrite. If 35.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water.) A. The concentration of HNO2 will increase. B. The concentration of NO2- will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will decrease. E. The ratio of [HNO2] / [NO2-] will increase.
A 1.00 liter solution contains 0.60 M ammonia and 0.46 M ammonium iodide.If 0.23 moles of nitric acid are added to this system,indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of nitric acid.) A. The number of moles of NH3 will decrease. B. The number of moles of NH4+ will decrease. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will decrease. E. The ratio of [NH3] / [NH4+] will decrease.
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Consider the buffer system composed of benzoic acid, HC, H,O,, and its conjugate base benzoate, C,H,0;. HC,H,0, + H,0 = H,0* +C,H,0, Using Le Châtelier's principle, predict how the concentration of each substance changes by the addition of H,O*. Does the concentration of HC, H,0, increase or decrease when H,0* is added? O increase decrease Does the concentration of C, H,0, increase or decrease when H,O* is added? O decrease O increase Does the concentration of H,O* change significantly when H,O* is added? O no Does the concentration of H,O* change significantly when H,Ot is added? по yes Does the pH change significantly when H,O is added? no O yes Using Le Châtclier's principle, predict how the concentration of cach substance changes by the addition of OH. Does the concentration of HC,H,O, increase or decrease when OH is added? increase O decrease Does the concentration of C,H,O, increase or decrease when OH" is added? O decrease
9. Measurement of Acetylcholine Levels by pH Changes You have a 15 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 7.65. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. O CH3 CH3-C-O-CH2-CH2-N–CH3 Acetylcholine CH3 H₂O CH3 HỌCH, CH, N– CH3 + CH3-CHO TH 11 CH3 Choline Acetate T 4 At the end of the incubation period, you measure the pH again and find that it has decreased to 6.87. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 15 mL sample.
A solution is prepared that is initially 0.30M in hydrofluoric acid (HF) and 0.13M in potassium fluoride (KF). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H3O+]. You can leave out the M symbol for molarity. [HF] [F] [H,O] initial 0 0 change 0 final 0 0 ㅁ 1 G
A 29.2 mL sample of 0.289 M ammonia, NH3, is titrated with 0.359 M nitric acid. The pH before the addition of any nitric acid is Use the Tables link in the References for any equilibrium constants that are required.
A 1.00 liter solution contains 0.45M hydrocyanic acid and 0.58M sodium cyanide. If 0.15 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) q, A. The number of moles of HCN will decrease. ◻ B. The number of moles of CN-will remain the same. ◻ C. The equilibrium concentration pf H3O+will remain the same. ◻ D. The pH will remain the same. ◻ E. The ratio of [HCN][CN-]will increase.

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