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Arrange the following 0.010M solutions in order of increasing pH:
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General Chemistry: Principles and Modern Applications (11th Edition)
- Most 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_forwardAcids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.arrow_forwardA solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?arrow_forward
- Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?arrow_forwardIn each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) HCO2H(aq) + H2O() HCO2(aq) + H3O+(aq) (b) NH3(aq) + H2S(aq) NH4+(aq) + HS(aq) (c) HSO4(aq) + OH(aq) SO42(aq) + H2O+()arrow_forwardWrite chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2C2O4 (oxalic acid) b. H2C4H4O6 (tartaric acid)arrow_forward
- Consider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an acidic solution and which gives a basic solution? (b) Which of these anions will have no effect on the pH of an aqueous solution? (c) Which ion is the strong base? (d) Write a chemical equation for the reaction of each basic anion with water.arrow_forwardIonization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.arrow_forwardCalculate the pH of the resulting solution if 22.0 mL of 0.220 M HCl(aq) is added to 32.0 mL of 0.220 M NaOH(aq). pH = Calculate the pH of the resulting solution if 22.0 mL of 0.220 M HC1(aq) is added to 12.0 mL of 0.320M NAOH(aq). pH =arrow_forward
- Which of the following are acid-base reactions? 1. AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq) 2. NH3(aq) + H2O(1) + OH-(aq) NH4" (aq) + 3. Zn(s) + 2Ag*(aq) → 2Ag(s) + Zn2+ (aq) a. 3 only b. 1, 2, and 3 c. 2 only d. 2 and 3 e. 1 onlyarrow_forwardCalculate the pH of the resulting solution if 26.0 mL of 0.260 M HCl(aq) is added to 36.0 mL of 0.260 M NaOH(aq). pH = Calculate the pH of the resulting solution if 26.0 mL of 0.260 M HCI(aq) is added to 16.0 mL of 0.360 M NaOH(aq). pH IIarrow_forwardthe ionization constant for HCN is 4.5 x 10^-10. what is the pH of a 0.43 molar solution of sodium cyanide which contains the cyanide ionarrow_forward
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