Multiple ChoiceCalculate the [H+] of a 0.50 M solution of methylammonium bromide, CH3NH3Br. The Kb of methylamine, CH3NH2, is given as 4.4 x 10-4.260views1rank2comments
Multiple ChoiceAn unknown weak acid has an initial concentration of 0.55 M. What is the pH of the solution if the weak acid also has a pKa of 5.79?216views1rank
Textbook QuestionAn acid solution with a concentration of 0.500 M has a pH = 3.21. What is the Ka of the acid? (LO 16.8) (a) 1.2 * 10-5 (b) 1.7 * 10-6 (c) 7.6 * 10-7 (d) 5.4 * 10-3530views
Textbook Question(b) Calculate the percent ionization of 0.0075 M butanoic acid in a solution containing 0.085 M sodium butanoate.515views1comments
Textbook Question(a) Calculate the percent ionization of 0.0075 M butanoic acid 1Ka = 1.5 * 10-52.611views
Textbook Question(a) Calculate the percent ionization of 0.125 M lactic acid 1Ka = 1.4 * 10-42.913views
Textbook QuestionYou are asked to prepare a pH = 3.00 buffer solution starting from 1.25 L of a 1.00 M solution of hydrofluoric acid (HF) and any amount you need of sodium fluoride (NaF). (a) What is the pH of the hydrofluoric acid solution prior to adding sodium fluoride?306views
Textbook QuestionYou are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid 1C6H5COOH2 and any amount you need of sodium benzoate 1C6H5COONa2. (a) What is the pH of the benzoic acid solution prior to adding sodium benzoate?324views
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. a solution that is 0.20 M in HCHO2 and 0.15 M in NaCHO22006views
Textbook QuestionCalculate the percent ionization of a 0.15 M benzoic acid solution in pure water and in a solution containing 0.10 M sodium benzoate. Why does the percent ionization differ significantly in the two solutions?1965views
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. c. a mixture that is 0.15 M in HF and 0.15 M in NaF1756views
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. 0.15 M HF1218views
Textbook QuestionThe following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have been omitted for clarity. (e) What is the percent dissociation in the solution of HZ?479views
Textbook QuestionThe following pictures represent initial concentrations in solutions that contain a weak acid HA (pKa = 6.0) and its sodium salt NaA. (Na+ ions and solvent water molecules have been omitted for clarity.) . (b) Draw a picture that represents the equilibrium state of solution (1) after the addition of two H3O+ ions.496views
Textbook QuestionPhenylacetic acid 1C6H5CH2COOH2 is one of the substances that accumulates in the blood of people with phenylketonuria, an inherited disorder that can cause mental retardation or even death. A 0.085 M solution of C6H5CH2COOH has a pH of 2.68. Calculate the Ka value for this acid.1284views1comments
Textbook QuestionA 0.100 M solution of chloroacetic acid 1ClCH2COOH2 is 11.0% ionized. Using this information, calculate 3ClCH2COO-4, 3H+4, 3ClCH2COOH4, and Ka for chloroacetic acid.767views
Textbook QuestionA 0.100 M solution of bromoacetic acid 1BrCH2COOH2 is 13.2% ionized. Calculate 3H+4, 3BrCH2COO-4, 3BrCH2COOH4 and Ka for bromoacetic acid.818views
Textbook QuestionIf a solution of HF 1Ka = 6.8 * 10-42 has a pH of 3.65, calculate the concentration of hydrofluoric acid.440views
Textbook QuestionThe acid-dissociation constant for chlorous acid 1HClO22 is 1.1 * 10-2. Calculate the concentrations of H3O+, ClO2-, and HClO2 at equilibrium if the initial concentration of HClO2 is 0.0125 M.1062views
Textbook QuestionCalculate the percent dissociation of 0.10 M hydrazoic acid (HN3, Ka = 1.9 X 10^-5). Recalculate the percent dissociation of 0.10 M HN3 in the presence of 0.10 M HCl, and explain the change.918views
Textbook QuestionCalculate the percent ionization of propionic acid 1C2H5COOH2 in solutions of each of the following concentrations 1Ka is given in Appendix D): (a) 0.250 M628views
Textbook QuestionDetermine the pH of an HNO2 solution of each concentration. In which cases can you not make the simplifying assumption that x is small? a. 0.500 M b. 0.100 M c. 0.0100 M1858views1comments
Textbook QuestionDetermine the pH of an HF solution of each concentration. In which cases can you not make the simplifying assumption that x is small? (Ka for HF is 6.8 * 10-4.) a. 0.250 M b. 0.0500 M c. 0.0250 M2055views1comments
Textbook QuestionA 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka) for the acid.3083views2rank
Textbook QuestionEphedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base: C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2 A 0.035 M solution of ephedrine has a pH of 11.33. (a) What are the equilibrium concentrations of C10H15ON, C10H15ONH+, and OH-?1221views
Textbook QuestionCalculate the percent ionization of a formic acid solution having the given concentration. d. 0.0500 M416views
Textbook QuestionCalculate the percent ionization of a formic acid solution having the given concentration. c. 0.100 M341views
Textbook QuestionCalculate the percent ionization of a formic acid solution having the given concentration. b. 0.500 M885views
Textbook QuestionCalculate the percent ionization of a formic acid solution having the given concentration. a. 1.00 M1138views
Textbook QuestionA 0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.2817views1rank1comments
Textbook QuestionPyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (c) A solution of pyridinium bromide has a pH of 2.95. What is the concentration of the pyridinium cation at equilibrium, in units of molarity?452views
Textbook QuestionA vitamin C tablet containing 250 mg of ascorbic acid 1C6H8O6; Ka = 8.0 * 10-52 is dissolved in a 250 mL glass of water. What is the pH of the solution?1488views
Textbook QuestionAcetic acid 1CH3COOH; Ka = 1.8 * 10-52 has a concentration in vinegar of 3.50% by mass. What is the pH of vinegar? (The density of vinegar is 1.02 g/mL.)1380views
Textbook QuestionA typical aspirin tablet contains 324 mg of aspirin (acetylsalicylic acid, C9H8O4), a monoprotic acid having Ka = 3.0 * 10-4. If you dissolve two aspirin tablets in a 300 mL glass of water, what is the pH of the solution and the percent dissociation? 1815views1rank
Textbook QuestionButyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (b) Calculate the pH of a 0.050 M solution of butyric acid.898views1rank
Textbook QuestionThe amino acid glycine 1H2N¬CH2¬COOH2 can participate in the following equilibria in water: H2N¬CH2¬COOH + H2OΔ H2N¬CH2¬COO- + H3O+ Ka = 4.3 * 10-3 H2N¬CH2¬COOH + H2OΔ+H3N¬CH2¬COOH + OH- Kb = 6.0 * 10-5 (b) What is the pH of a 0.050 M aqueous solution of glycine?461views
Textbook QuestionCalculate the pH and the percent dissociation of the hydrated cation in 0.020 M solutions of the following substances. See Appendix C for values of equilibrium constants. (a) Fe1NO322396views
Textbook QuestionCalculate the pH and the percent dissociation of the hydrated cation in the following solutions. See Appendix C for the value of the equilibrium constant. (a) 0.010 M Cr1NO323722views
Textbook QuestionWhen NO2 is bubbled into water, it is completely converted to HNO3 and HNO2: 2 NO21g2 + H2O1l2S HNO31aq2 + HNO21aq2 Calculate the pH and the concentrations of all species present (H3O+ , OH-, HNO2, NO2 -, and NO3 -) in a solution prepared by dissolving 0.0500 mol of NO2 in 1.00 L of water. Ka for HNO2 is 4.5 * 10-4.966views
Textbook QuestionA 1.000 L sample of HF gas at 20.0 °C and 0.601 atm pressure was dissolved in enough water to make 50.0 mL of hydrofluoric acid. (a) What is the pH of the solution?269views
Textbook QuestionYou may have been told not to mix bleach and ammonia. The reason is that bleach (sodium hypochlorite) reacts with ammonia to produce toxic chloramines, such as NH2Cl. For example, in basic solution: OCl-1aq2 + NH31aq2S OH-1aq2 + NH2Cl1aq2 (b) The following mechanism has been proposed for this reaction in basic solution: H2O + OCl-HOCl + OH- Fast, equilibrium constantK1 HOCl + NH3 S H2O + NH2Cl Slow, rate constantk2 Assuming that the first step is in equilibrium and the second step is rate-determining, calculate the value of the rate constant k2 for the second step. Ka for HOCl is 3.5 * 10-8.405views
Open QuestionCalculate [H3O+], [ClO4–], and [OH–] in an aqueous solution that is 0.130 M in HClO4(aq) at 25 °C.94views
Open QuestionWhat is the H+(aq) concentration in 0.05 M HCN(aq)? (the Ka for HCN is 5.0 x 10-10.)79views
Open QuestionWhat is the pH of a 0.0620 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-10)?102views
Open QuestionWhat is [H+] in a 0.270 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 × 10-5)?88views
Open QuestionFormic acid is found in ant venom. What would be the pH of a 0.30 m formic acid solution? The Ka of formic acid is 1.8 x 10-4. a. 0.52 b. 4.27 c. 2.13 d. 8.61 e. 5.3970views
Open QuestionCalculate [H3O+], [ClO4–], and [OH–] in an aqueous solution that is 0.130 M in HClO4(aq) at 25°C.100views
Open QuestionWhat is [H⁺] in a 0.270 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 × 10⁻⁵)?89views
Open QuestionNitrous acid, HNO2, has a ka of 7.1 x 10–4. what is the [H3O+] in a 0.60 M solution of HNO2?69views
Open QuestionFind the percent ionization of a 0.337 m HF solution. the ka for hf is 3.5 × 10-4. What would you expect the percent ionization to be for the same concentration of hydrochloric acid (HCl)? Explain.103views