3. At 25 °C, the groundwater is saturated with CO2 at a partial pressure of 0.2 atm. The pH of the groundwater is 5.80. Please estimate the concentration of calcium (Ca) in the groundwater sample.
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- 7) An aqueous solution containing 25.0 mg of a hormone in 150.0 mL of solution with an osmotic pressure at 25 °C of 9.00 mmHg. What is the molecular weight of the hormone? 8) (a) What is the pH of a solution in which 45 mL of 0.10 M sodium hydroxide is added to 25mL of 0.15M hydrochloric acid? (b) A brand of carbonated beverage has a pH of 3.50. Calculate [H*]=?Estimate the calcium concentration (in ppm by mass) in a groundwater sample, which has a pH of 5.63. Assume that the groundwater at this location is saturated with CO2 at a partial pressure of 0.185 atm. The atomic weight of calcium is 40.1 g/mol.Determine the pH of (a) A 0.10 M CH3COOH solution (ICE) (b) A solution that is 0.10 M CH3COOH and 0.10 M CH3COONa. Ka for CH3COOH = 1.8 X 10-5.
- 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.1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?Predict whether aqueous solutions of the following substances are acidic, basic, or neutral and write hydrolysis equations for the acidic and basic solutions. (a) CsBr; (b) Al(NO3)3; (c) KCN; (d) CH3NH3Cl
- A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.The precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the pH at whichprecipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3is added to 2000 gal of water. (b) Approximately howmany pounds of CaO must be added to the water toachieve this pH?Express in percentage the fluoride concentration in drinking water given in 0.6 ppm.
- Determine the pH of each of the following solutions (Ka and Kb values can be found in the appendices of your textbook or online): (a) 0.045 M hypochlorous acid; (b) 0.0068 M phenol; (c) 0.080 M hydroxylamine.1) Describe how you would prepare a 500.00 mL portion of 0.25M calcium hydroxide solution starting with solid calcium hydroxide. (b) What is the pH of the solution? 2) Acetone has a vapor pressure of 183.0 mm Hg at 40 °C and a heat of vaporization of 30.8 kJ/mol. What is the vapor pressure of acetone at 25 °C? 3) (a) Calculate the molality (m) of a solution containing 75.0 gm of glycol (C2H&O2) in 250.0 gm of water. (b) What is the mass percent of glycol in this solution?COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…