In a different situation, you want to use acid-base extraction to separate compound A (pK, = 5.9) from compound B (pK, = 12.5). You can add either a solution of NaOH or Na,CO, to act as your aqueous layer. You may look up any relevant pK, values. %3D Which solution should you choose and why would the other one not work?
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- 1. You will use 0.5mM PNPP, 0.2M Tris-HCl, and 1mM P; stock solutions to prepare two sets of five samples (Sets A and B), each with varying P; concentrations. The PNPP concentration for all samples in Set A will be 0.05mM; and 0.150mM for all samples in Set B. Fill out the tables below and use them to prepare your samples. Be aware of the following: • Prepare the samples directly in cuvettes. Prepare one sample at a time to minimize exposing PNPP to air. You can prepare the next sample while the current one is being measured. • Each sample before adding enzyme (i.e., the cuvette only contains PNPP, Pi, and Tris-HCI) is its own blank. In other words, you add the appropriate amounts of PNPP, Pi, and Tris- HCI to a cuvette, press "Measure Blank", then add 100μL of AP to the same cuvette, mix, and press "Measure Sample". • You must blank the instrument (before adding the enzyme) each time you prepare a new sample. Table 1. Sample Set A (PNPP concentration = 0.05mM) Final [Pi] (μM) Vol of…Benzoic acid, C6H5COOH (pKa = 4.19), is only slightly soluble in water, but its sodium salt, C6H5COO Na", is quite soluble in water. In which of the following solutions will benzoic acid dissolve more readily than in pure water? O NAHCO; O LIOH O H;SO4 O HCI OK½CO3The value of Ksp for Mg3(AsO4)2 is 2.1 * 10-20. The AsO43- ion is derived from the weak acid H3AsO4 (pKa1 = 2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molar solubility of Mg3(AsO4)2 in water.
- 8. Given Ka for CH(CH2) COOH - 1.5 x 105 Mat 298 K. Calculate the pHof a. An aqueous solution of 0.10 M CH,(CH:).COOH (Hint: assume (H,O') = [CH3(CH))CO0) b. An aqueous solution of 0.050 M CH,(CH)»COON and 0.050 M CH(CHa);COOH c. 1Lofthe solution in (b) after the addition of 1.0 x 10 molof solid NaOH.A solution is prepared in which [Pb2+]= 0.0150 M and [Br 0.00350 M. Given that PbBr2 has a Kgo = 2.1 x 106, which of the following is true? %3D Select one: O a. Qsp Kg. and the solution is supersaturated %3D O d. Q.,< Kgp and the solution is supersaturated(a) In performing a titration, why is it better to use a solution of a concentration such that 30-45 mL is required, instead of a more concentrated solution that might only require about 5 mL to reach the end point? (b) To make a standardized NaOH solution, why is it better to prepare a NaOH solution of approxi- mate concentration and then standardize with KHP, rather than to weigh accurately some NAOH pellets, dissolve them, and dilute the solution in a volumetric flask? (c ) In analyzing a 0.003 weak acid by titration with 0.00300 M NaOH, why would you be able to obtain greater accuracy by using a pH meter instead of using a color-change indicator such as phenolphthalein?
- From the following data find the percentages of Na2CO3 and NaHCO3 in a mixture of these chemicals and inert constituents: a) A 0.5000 g sample required 45.50 mL 0.1050 N HCl to reach the methyl orange end point. b) 25.00 mL of 0.1000 N KOH is added to 0.2500 g of the sample; BaCl2 is added to precipitate the BaCO3 and 12.00 mL 0.1050 N HCl is required to reach the phenolphthalein end point.Q2) Q2) How much mole of NH3 to be added to 500 ml of the solution with pH=8.9 to dissolve 5x10 * of AgSCN? PKSP(AGSCN)=12, PKa(NH.') =9.2 , PKDA9(NH3)*/Ag+=7.23.A sample is known to contain NaOH, Na2CO3 NaHCO3 or compatible mixture of these together with inert matter. With methyl orange, a 1.100 g sample requires 31.40 mL of HCl ( 1.00 mL is equivalent to 0.0140g CaO). With phenolphthalein indicator, the same weight of sample requires 13.30mL of the acid. What is the percent composition of the sample? ww ww
- 3. 40.00 mL of 0.0900 M NaOH is diluted to 100mL and titrated with 0.1000M HCI. Calculate the pH after the addition of the following volumes of titrant (mL); (a) 0.00; (b) 10.00 ; (c) 18.00: (d) 30.00 ; (e) 35.95 ; (f) 36.00 (g) 36.05 ; (h) 40.00.2) 3) Using equilibrium table, calculate the molar solubility of PbF2 [Ksp - 4x10"] in 0.035 M NaF aq. solution. mL. Using equilibrium table, calculate the Ksp of CaCO3 at this temperature. [Molar The solubility of CaCO3 in water at a certain temperature is 3.5x102 g/50 mass of CaCO3 is 100 g/mol] 4) Calculate the moles of acetic acid CH3COOH that should be added to 2.5 L of 0.35 M sodium acetatc CH3COONa aq. solution to prepare a buffer solution with pH of 4.8. [Ka acetic acid = 1.8x10-]A series of solutions containing NaOH, Na.CO, and NaHCO, alone or in compatible combination, was titrated with o.1202 needed to titrate 25.00-mL portions of each solution to (1) a phenolphthalein and (2) a bromocresol green end point. Use this information to deduce the composition of the solutions. In addition, calculate the mass in milligrams of each solute per milliliter of solution. M HCI. Tabulated below are the volumes of acid (2) (1) (а) 22.42 (Ъ) 15.67 (c) 29.64 (d) 16.12 (е) о.00 22.44 42.13 36.42 32.23 33.333