A solution is prepared with 1.0×102 M NaCl, 2.0×10-² M Caci 1.0x10-³ M NaHCO3 and 5.0×10-4 M Na₂HPO4. (a) What is the ionic strength of this solution? (b) Estimate the activity coefficients for monovalent, divalent and trivalent ionic species using the Davies equation.
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- A water sample has exact alkalinity of 220 mg/L CaCO3. The sample contains150.0 mg/L HCO3 at a pH of 7.1 (Temperature = 25 oC).(a) Calculate the carbonate alkalinity in mg/L as CO3.(b) Calculate the approximate alkalinity.(c) Comment on the difference between the exact and the approximate alkalinity10.) Calculate the activity coefficient of K* in 0.050 M KNO3.A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate the molar concentrations of H2PO4–and HPO42–, respectively, in thesolution. (b) What is the pH of the solution? (H2PO4– has Ka = 6.2 x 10–8) (c) Write a net ionic equation for the buffering reaction against a strong acid by this buffer. (d) If 0.012 mole of hydrochloric acid (HCl) is added to the solution, create a reaction table to show the buffering reaction and calculate the molar concentration of H2PO4–and HPO42–, respectively, in the resulting solution after the buffering reaction. (e) What is the pH of the resulting solution?
- 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.The thermodynamic solubility product of A9CN is 6.0×10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.75e-9 mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.81e-16 X mol·L-1(2). For the buffer system, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer? Given: • 20.0 ml of 3.00 M sodium bicarbonate = conjugate base in molarity [? −] • 50.0 ML OF 2.00 M carbonic acid = weak acid in molarity [??] • 4.30 × 10−7 ?? of carbonic = ??? (acid-dissociation constant) • Base: (a) 15.0 ml of 0.500 M HCl (b) 15.0 ml of 0.750 M NaOH
- Phosphate-buffered saline (PBS) is a solution commonly used in studies of animal tissues and cells. Its composition is 137 mM NaCl, 2.7 mM KC1, 10 mM Na, HPO, (pK, = 2.14), and 1.8 mM KH₂PO, (pK, = 6.86). Calculate the pH and osmolarity of PBS. Give the osmolarity in units of osmoles per liter (osm/L). pH = 7.605 osmolarity 313.0 Incorrect osm/L7) 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*]=?What is the molar solubility (in mols/L)of silver chloride in 2.00 M NH3(aq) given that Kgp of AGCI = 1.77x10-10 and Kf of Ag(NH3)2* is 1.70×107? Express your answer in decimal notation rounded to three significant figures.
- (a) Write all the reactions and equations for an open carbonate system. (b) Derive the equations for log[H,CO;*], log[HCO;-], and log[CO32-]. Show detailed steps. (c) Assume that we, humankind fails to control the carbon emission and climate change. Determine the rainwater pH for pco2 = 200,000 ppm by drawing a logC-pH diagram for the open carbonate system. Don't forget the lines for [H+] and [OH-]. Use the grid paper.Calculate the DHLL activity coefficient for Cl- or Fe3+in a solution of FeCl3 that is 0.1 m in concentration. Suppose you dissolve NaCl in a 0.1 m HCI solution so that the final concentration of the salt is 0.2 m NaCl. What will be the DHLL activity coefficients for Na+, H+, and Cl-?(a) If the molar solubility of YF3 at 25 °C is 4.23e-06 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 0.00100 g of BaCO3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-product constant for BaCO3. Ksp = (c) The Ksp of ZnCO3 at 25 °C is 1.46e-10. What is the molar solubility of ZnCO3? solubility = mol/L