3.Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2-Tris or THAM] is a weak base frequently used to prepare buffers in biochemistry. Its Kb is 1.2 x 10^-6 and pKb is 5.92. The corresponding pKa is 8.08, which is near the pH of the physiological buffers, and so it exhibits good buffering capacity at physiological pH. What weight of THAM must be taken with 100 mL of 0.50 M HCl to prepare 1L of a pH 7.90 buffer?
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- The Tris buffer system is commonly used in biochemistry as its pKa of 8.1 allows it to buffer close to physiological pH. (CH2OH)3CNH2 + H+ Û (CH2OH)3CNH3+ What concentrations of Tris and Tris H+ are obtained in a 200 mL solution at pH 8.20 containing 6.1g of Tris? The molecular mass of Tris is 121.1 gmol-1 Please do this step by step thank you!(a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/LGiven that the Ksp for Ag2S is 6×10^-51, Kf=1.1×10^5 for AgCl2-, and Ka1 and Ka2 for H2S are 9.5×10^-8 and 1×10^-19, respectively, calculate the equilibrium constant for the following reaction .
- At 25oC the Ksp for PbCl2 is 1.6 × 10–5. See Periodic Table Calculate Q for the following: 125.0 mL of 0.0200 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25oCThe Ksp of ZnCO3 (MM: 125.38) is 1.20 xx 10^(-10). a) What is the molar solubility of ZnCO3? b) What is the solubility of ZnCO3 in g/L?What is the concentration of free Ag+(aq) in a solution that is initially 0.01254 M in AgNO3 and 1.04842 M NH3? These two compounds react together to form [Ag(NH3)2]+. Kf([Ag(NH3)2]+) =1.600e7 1.023 7.484e-10 0.01254 6.250e-8
- What is the pH of a saturated solution of sodium carbonate? (Solubility in water is 21.6g/100ml at rtp and for carbonic acid Ka1 = 4.5×10^-7, Ka2 = 4.7×10^-11)TypeFormulaKsp Solubility Product Constants (Ksp at 25 oC) TypeFormulaKspBromidesPbBr26.3 × 10-6AgBr3.3 × 10-13CarbonatesBaCO38.1 × 10-9CaCO33.8 × 10-9CoCO38.0 × 10-13CuCO32.5 × 10-10FeCO33.5 × 10-11PbCO31.5 × 10-13MgCO34.0 × 10-5MnCO31.8 × 10-11NiCO36.6 × 10-9Ag2CO38.1 × 10-12ZnCO31.5 × 10-11ChloridesPbCl21.7 × 10-5AgCl1.8 × 10-10ChromatesBaCrO42.0 × 10-10CaCrO47.1 × 10-4PbCrO41.8 × 10-14Ag2CrO49.0 × 10-12CyanidesNi(CN)23.0 × 10-23AgCN1.2 × 10-16Zn(CN)28.0 × 10-12FluoridesBaF21.7 × 10-6CaF23.9 × 10-11PbF23.7 × 10-8MgF26.4 × 10-9HydroxidesAgOH2.0 × 10-8Al(OH)31.9 × 10-33Ca(OH)27.9 × 10-6Cr(OH)36.7 × 10-31Co(OH)22.5 × 10-16Cu(OH)21.6 × 10-19Fe(OH)27.9 × 10-15Fe(OH)36.3 × 10-38Pb(OH)22.8 × 10-16Mg(OH)21.5 × 10-11Mn(OH)24.6 × 10-14Ni(OH)22.8 × 10-16Zn(OH)24.5 × 10-17IodidesPbI28.7 × 10-9AgI1.5 × 10-16OxalatesBaC2O41.1 × 10-7CaC2O42.3 × 10-9MgC2O48.6 × 10-5PhosphatesAlPO41.3 × 10-20Ba3(PO4)21.3 × 10-29Ca3(PO4)21.0 × 10-25CrPO42.4 × 10-23Pb3(PO4)23.0 × 10-44Ag3PO41.3 × 10-20Zn3(PO4)29.1 ×…When a drop (taken to be 0.20 cm3) of 1.0 M HCI(aq) is added to 25 cm3 of pure water, the resulting hydroniumion concentration rises to 0.0080 mol dm- 3 and so the pH changes from 7.0 t o 2.1, a big change. Now suppose the drop is added to 25 cm3 of an ethanoate buffer solution that is 0.040 MNaCH3CO2(aq) and 0.080 M CH3COOH(aq). What will be the change in pH?
- If the concentration of PB2+, is found to be 1.3*10^-9mol/L in a saturated solution of Pb3(PO4)2, what is the ksp of Pb3(PO4)2?For each pair of compounds, use Ksp values to determinewhich has the greater molar solubility: (a) CdS or CuS,(b) PbCO3 or BaCrO4, (c) Ni(OH)2 or NiCO3, (d) AgI orAg2SO4.The Ksp for CoCO3 = 1.0 × 10–10 and the Ksp for PbCO3 = 7.4 × 10–14. When Na2CO3 is added dropwise to a solution containing 0.010 M Co2+ and 0.010 M Pb2+, which ion will precipitate first? What must the [CO32–] be so that the first ion to precipitate comes out of solution, but the second ion does not?