When 20 mmol Pb(NO3)2 is added to 250 mL of 1.0 M NaX, the [PbX4]²- ion forms. At equilibrium, [Pb2*] = 3.1 x 10-6 M. Calculate Kę for [PbX4]²-. %3D
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- A buffer solution is prepared by taking 0.400 moles of acetic acid (pKa = 4.76) and 0.250 moles of sodium acetate in sufficient water to make 1.400 liters of solution. Calculate the pH of this solution.Calculate the solubility of PbF2 in water at 25°C.Consider a buffer prepared by mixing 0.100 M propionic acid (CH3CH2COOH, pKa = 4.87) and 0.200 M sodium propionate (NaCH3CH2COO). Which species will most likely react upon addition of aqueous HCl solution? CH3CH2COOH CH3CH2COO– H2O Na+
- a. A solution is prepared by dissolving 1.50 g of NaOH in enough water to make 1.250 L of solution. What is the [H3O+] in M of this solution? molar mass of NaOH = 40.0 g/mol b. Estimate the pH of a buffer that is 0.52 M in HClO2 and 0.44 in KClO2. The Ka for HClO2 = 1.20 x 10-2Iminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from industrial waste waters. It forms a 2:1 complex with many heavy metals, with a high selectivity for divalent over monovalent ions. A 14.50 mL sample of 0.0315 M Ni2+ was added to 14.50 mL of 0.187 M iminodiacetic acid (the completely protonated form is abbreviated as H3A+) buffered at pH 7.00. Given that ?A2− is 4.6×10−3 at pH 7.00, what is the final concentration of Ni2+ remaining in solution? Ni2+(aq)+2A2−(aq)↽−−⇀NiA2−2(aq)?f=2.00×1014 [Ni2+]= __________ MWhat will be the appropriate pH of a buffer prepared by mixing 100 ml of 0.1 M Na2HPO4 and 100 ml of 0.1 M NaH2PO4? (For H3PO4, pKa1 = 2.1; pKa2 = 6.8; pKa3 = 12.5)
- Chemistry 0.0250 mol/L solution of Mn2+ is buffered with NH 3 and NH4Cl in such a waythat there is no precipitation of manganous hydroxide, Mn(OH)2. Under these conditions, the concentrationmaximum permissible OH in the aqueous medium is ..........................mol/L. If the ammonia concentration is0.60 mol/L, then the ammonium concentration must be at least equal to ...............mol/L, and fortherefore, the mass of ammonium chloride present in the solution is equal to ....................... Data:KPS Mn(OH)2 = 2.0.10-13;Kb NH3 = 1.8 x 10-5MMNH4Cl = 53.45 g/mol.Which of the followinf salts could be added to the PbCl2 solution to decrease Pb2+ concebtration, while not decreasing the Cl concentration? NaCl KNO3 PbNO3 CaSO41. Calculate the pH of a buffer solution that is 0.20 M in sodium hypobromite (NaBrO) and 0.10 M in hypobromous acid (Ka of HBrO= 2.5 ×10−9) a 4.15 b 4.45 c 8.60 d 8.90 e 8.30 2. A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa). [Ka= 1.8 ×10–5] What is the new concentration of CH3COOH after buffering? a. 0.2437 b. 0.2014 c. 0.1615 d. 0.3213 e. 0.2589 3. A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa). [Ka= 1.8 x 10–5] What is the new concentration of NaOH after dilution? a 0.0273 b 0.0439 c 0.0185 d 0.0267 e 0.0385
- Calculate the pH of a buffer solution obtained by dissolving 11.011.0 g of KH2PO4(s and 29.0g of Na2HPO4(s) in water and then diluting to 1.00 L.If a solution contained Ni2+ ions at a concentration of 0.1 M, what pH would have to be reached toprecipitate 99% of the Ni2+ as Ni(OH)2?How many grams of sodium acetate (82.03 g/mol) must be added to 1.00 L of 0.50 M solution of acetic acid to produce a buffer solution at pH 4.00? (Kₐ = 1.75 ⨯ 10⁻⁵)