Calculate the molar concentration of Ba2+ in saturated BaC2O4 solution. The pH was kept at 4.5. Ksp of BaC2O4 = 1.0 x 10^-6 , Ka1 = 5.4 x 10^-2, Ka2 = 5.42 x 10^-5
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- Given the following activity coefficient data: Ion Ion Size (pm) Ionic Strength (μ, M) 0.001 0.005 0.01 0.05 0.1 Zn2+ 600 0.870 0.749 0.675 0.485 0.405 Calculate the ionic strength of a solution that is 0.0213 M Mg(CN)2. Based on your results in part 1, what is the activity coefficient of Zn2+? 3. Zinc cyanide, Zn(CN)2, has a Ksp of 3.0 x 10−16. Using the activity coefficient you calculated in part 2, find the concentration of Zn2+ in a saturated solution of Zn(CN)2 in 0.0213 M Mg(CN)2. (Note: The activity coefficient for cyanide in at this ionic strength is 0.791.)A buffer solution was prepared by adding 4.92 g of sodium acetate, NaCH3CO2, to 2.50 x 10^2 mL of 0.170 M acetic acid, CH3CO2H (Ka= 1.8 x 10^-5).If the base (NaOH) is standardized to 0.12 M in Part A of this experiment, calculate the amount of oxalic acid dihydrate (H2C2O4•2 H2O, MW = 126.06 g/mol) required to neutralize 35 mL of this NaOH solution.
- The Ksp of BaF2 is 2.45 x 10-5. Given that value, calculate the molar concentration of Ba2+ ion in a saturated solution. (a) 3.2 x 10-4 (b) 8.00 x 10-7 (c) 1.04 x 10-5 (d) 1.83 x 10-2Using the following choices, determine which will result in a brightly and dimly lit light bulb when subjected to the conductivity test. a. Mixture of 10.0 mL 1.0 M Mg(OH)2 and 10.0 mL 1.0 M HNO3 b. 70% (v/v) ethanol c. 1.0 M citric acid d. Glacial acetic acid Brightly: _________ Dimly: _________Calculate the solubility of Ca(OH)2(s) (Ksp = 1.6 x 10–15) in an aqueous solution buffered to pH 8.0. Show your work and justify any approximations made.
- What is the fluoride ion concentration for a saturated solution of SrF2 if the Ksp for SrF2 is 2.5 x 10-9?There are many organic acids and bases in our cells, and their presence modifies the pH of the fluids inside them. It is useful to be able to assess the pH of solutions of acids and bases and to make inferences from measured values of the pH. A solution of equal concentrations of lactic acid and sodium lactate was found to have pH= 3.08. (a) What are the values of pKa and Ka of lactic acid? (b) What would the pH be if the acid had twice the concentration of the salt?I would need help with these problems, please show step by step: 1. A beaker containing 500.0 mL was determined to contain 0.150 M ammonia (NH3) and 0.150 M ammonium chloride NH4 To this solution was added 50.0 mL of 0.15 M hydrochloric acid (HCl). What was the change in pH of the ammonia, ammonium ion solution? 2. Calculate the isoelectric and isoionic pH of 0.010 M threonine? pK1 = 2.15, pK2 = 9.12 3. Find the pH of a 1.00 L aqueous solution containing 12.43 g of tris (FM 121.14) plus 4.67 g of tris hydrochloride ( FM 157.60) ? What would be the new pH after adding 12.0 mL of 1.00 M NaOH to this buffer?
- KSP =1.2 X10^-5 FOR PbCl2 in water at room temperature what is the maximum concentration in mol/L of Pb2+ ion in this solution?Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn of the solution after 30 mL of titrant have been added?What is the equilibrium constant for the hydrolysis of acetate ion at 25°C. Ka = 1.74 x 10-5