What is the pH of a solution made by adding 0.65 m of acetic acid (H3CO2H) and 0.30 mol of sodium acetate (H3CO2Na) to enough water to make a 1.0 L solution? (K, = 1.8 x 105) %3D CH3CO2H (aq) + H2O (1) CH3CO2° (aq) + H3O* (aq) 4.74 O 5.08 04.40 8.92
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- A 50.00 mL sample of a locally made white wine required 34.50 mL of 0.0450 M NaOH to reach the end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6)Atmospheric CO2 levels have risen by nearly 20% over thepast 40 years from 320 ppm to 400 ppm. (a) Given that theaverage pH of clean, unpolluted rain today is 5.4, determinethe pH of unpolluted rain 40 years ago. Assume thatcarbonic acid (H2CO3) formed by the reaction of CO2 andwater is the only factor influencing pH.CO2(g) + H2O(l) ⇌ H2CO3(aq)(b) What volume of CO2 at 25 °C and 1.0 atm is dissolvedin a 20.0-L bucket of today’s rainwater?What is the pH of a solution that is prepared by dissolving 7.50 grams of pyruvic acid (formula weight = 88.06 grams/mol) and 8.95 grams of sodium pyruvate (formula weight = 90.04 grams/mole) in water and diluting to 500.00 mL? The Ka for pyruvic acid is 0.00324.
- A site in Pennsylvania receives a total annual deposition of 2.688 g/m² of sulfate from fertilizer and acid rain. The ratio bymass of ammonium sulfate/ammonium bisulfate/sulfuric acid is 3.0/5.5/1.0. (a) How much acid, expressed as kg of sulfuric acid,is deposited over an area of 10. km²? (b) How many pounds of CaCO₃ are needed to neutralize this acid? (c) If 10. km² is the area of an unpolluted lake 3 m deep and there is no loss of acid,what pH would be attained in the year? (Assume constant volume.)Sodium benzoate, NaC6H5COO (molar mass 144.1 g mol-1) is a common food preservative. The Ka of benzoic acid, C6H5COOH, is 1.6 X 10-5. A chemist titrates 25.00 mL of a stock solution of sodium benzoate, NaC6H5COO, with 1.20 M HCl solution using a pH meter and an indicator. f) A typical sodium benzoate solution used for preserving food has a concentration of 0.069 M (iii) Determine the mass of sodium benzoate present in this solution.Sodium benzoate, NaC6H5COO (molar mass 144.1 g mol-1) is a common food preservative. The Ka of benzoic acid, C6H5COOH, is 1.6 X 10-5. A chemist titrates 25.00 mL of a stock solution of sodium benzoate, NaC6H5COO, with 1.20 M HCl solution using a pH meter and an indicator. (f) A typical sodium benzoate solution used for preserving food has a concentration of 0.069 M Determine the pH of this 0.069 M solution.
- Sodium benzoate, NaC6H5COO (molar mass 144.1 g mol-1) is a common food preservative. The Ka of benzoic acid, C6H5COOH, is 1.6 X 10-5. A chemist titrates 25.00 mL of a stock solution of sodium benzoate, NaC6H5COO, with 1.20 M HCl solution using a pH meter and an indicator. (f) A typical sodium benzoate solution usedfor preserving food has a concentration of 0.069M. (i) Determine the volume of the stock solution that should be diluted in order to make 200. mL of 0.069 M sodium benzoate.What is the pH at 25 °C of water saturated with CO2 at apartial pressure of 1.10 atm? The Henry’s law constant forCO2 at 25 °C is 3.1 x 10-2 mol/L-atm.What is the pH of a 1.47 mol/L solution of HCN(aq) if its Ka = 3.5 ´ 10-11?
- Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the electronegativity chlorine atom pulls eloectroms way from the O-H bond and thus weakens it. What is the pH of a 0.045 M aqueous solution of chloroacetic acid? The Ka for HF is 1.3x10-3. You must solve the quadric equation for this problem. Express your answer to two decimal places. -------------------------------------------------------------------------------------------------------------------------- What is the pH of a 0.080 M aqueous solution of methylamine, CH3NH2? The Kb for methylamine is 4.4x10-4. You must solve the quadric equation for this problem. Express your answer to two decimal places.What is the concentration of the hydroxide ion, OH-, in solution at equilibrium if the pH of the solution is 7.65? Nitrogen and oxygen react at high temperatures according to the following equation: N2(g) +O2(g) ⇄ 2NO(g) where ∆H=181kJ At equilibrium what will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed? Calculate the pH of the following weak base: 0.5M NH3 with Kb =1.8x10−5The pKa of acetic acid is 4.74. The conjugate base of acetic acid (CH3COOH) is sodium acetate (CH3COONa). One has two stock solutions. One is 0.10 M in acetic acid and the other is 0.2M in sodium acetate. If one mixes 200 Ml of the acetic acid solution with 100 mL of the sodium acetate solution, what would be the final pH?