Concept explainers
(a)
Interpretation: To write the balanced equation and the net direction of the reaction along with the explanation of the observation.
Concept introduction: If a strong acid reacts with a strong base and produces a weak base and weak acid, then the net direction of the reaction will be towards the right. Similarly, when a weak acid reacts with a weak base to produce strong acid and a strong base, then the net direction of the reaction will be towards the left.
(b)
Interpretation: To write the balanced equation and also the net direction of the reaction along with the explanation of the observation.
Concept introduction: If a strong acid reacts with a strong base and produces a weak base and weak acid, then the net direction of the reaction will be towards the right. Similarly, when a weak acid reacts with a weak base to produce strong acid and a strong base, then the net direction of the reaction will be towards the left.
(c)
Interpretation: To write the balanced equation and also the net direction of the reaction along with the explanation of the observation.
Concept introduction: If a strong acid reacts with a strong base and produces a weak base and weak acid, then the net direction of the reaction will be towards the right. Similarly, when a weak acid reacts with a weak base to produce strong acid and a strong base, then the net direction of the reaction will be towards the left.
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CHEMISTRY: THE MOLECULAR NATURE OF MATTE
- A solution contains Ca2+ and Pb2+ ions, both at a concentration of 0.010 M. You wish to separate the two ions from each other as completely as possible by precipitating one but not the other using aqueous Na2SO4 as the precipitating agent. (a) Which will precipitate first as sodium sulfate is added, CaSO4 or PbSO4? (b) What will be the concentration of the first ion that precipitates (Ca2+ or Pb2+) when the second, more soluble salt begins to precipitate?arrow_forwardMost naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.arrow_forwardThe concentration of acetylcholine (a neurotransmitter) in a sample can be determined from the pH changes that accompany its hydrolysis. When the sample is incubated with the enzyme acetylcholinesterase, acetylcholine is converted to choline and acetic acid, which dissociates to yield acetate and a hydrogen ion. CНз CHз Нао — сHz— CH "N— снз но-сн— сH,-"N-CH; + CH;— с-о+ н* CH3-C-0- сHз CHз Choline Acetylcholine Acetate In a typical analysis, 11 mL of an aqueous solution containing an unknown amount of acetylcholine had a pH of 7.70. When incubated with acetylcholinesterase, the pH of the solution decreased to 6.89. Assuming there was no buffer in the assay mixture, determine the number of moles of acetylcholine in the 11 mL sample.arrow_forward
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- Hydrochloric acid does not appear in either equilibrium reaction, yet it influences the reactions. Explain how it affects the equilibrium of ammonia and phenolphthalein in water and brings about the observed color change. Be specific, and include any relevant chemical equations. Attach a file if necessary. NH3(aq) + H2O (l) ⇄ NH4+(aq) + OH (aq) HCl causes a colorless solutionarrow_forwardWhich of the following aqueous solutions are good buffer systems? O0.13 M hypochlorous acid + 0.12 M sodium hypochlorite O 0.10 M potassium fluoride + 0.30 M hydrofluoric acid 0.27 M hydrobromic acid + 0.23 M potassium bromide 0.39 M acetic acid + 0.28 M potassium acetate O 0.34 M ammonium nitrate + 0.38 M ammoniaarrow_forward7. A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of titration.arrow_forward
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