The molar H;O*concentration in 0.010M (ethylamine) C,H;NH2 (Ka for C,H;NH;*= 2.5× 105) is.... ..... 0.5 x 10-8 2 x 10-8 2 x 10-4 O 2 x 10-11 0.5 x 10-4 5 x 10-4 2 x 10-6
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- Ethanoic acid is a weak acid pka value 4.74 at 298K. What do you understand by the term pka and ka? Calculate the numerical value of ka for ethanoic acidTypeFormulaKsp 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 ×…An initial equilibrium mixture of methyl acetate, water and methyl alcohol contained 4.0 mL of methyl acetate, 3.0 mL of water, and 2.0 mL of methyl alcohol. Final analysis showed that the solution required 12.15 mL of 0.5000 M NaOH for neutralization. Calculate Keq for this hydrolysis experiment. CH3CO2CH3 + H2O <----> CH3CO2H + CH3OH Densities (g/mL): 0.9279 1.000 1.0530 0.7866 Molar masses. 74.08 18.01 60.05 32.04 CH3CO2CH3 + H2O <----> CH3CO2H + CH3OH
- (a) Given the Ksp of calcium phosphate, Ca3(PO4)2 is 1.3 ×10-32. Calculate the concentrations of Ca2+ and PO43- respectively.(b) If a hard water contains 75 mg/L of Ca2+, at what concentration of PO43− would a precipitate of Ca3(PO4)2 begin to appear?A 0.022 2 M solution of HA is 0.15% dissociated. Calculate pKa for this acid.The pKa of Cl3CCO2H is 0.64. What is the pH of a 0.580 M solution? What percentage of the Cl3CCO2H is dissociated? pH = ? = ? %
- 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-8Benzoic acid (C₂H5CO₂H), a weak acid, has a dissociation constant of K=6.3x10^-5. 1. Write the equilibrium equation of the solution. 2. Write the Ka expression of the equilibrium involved. 3. What is the equilibrium concentration of all species if the initial concentration is a.) 0.0315M, b) 0.315M² 4. What is the resulting pH and pOH for a) and b)? 5. What is the %ionization of benzoic acid in a) and b) solution?Calcium Phosphate are used to make commercial fertilizer. Its Ksp value is 2.07x10-33 at 25oC. Express answers in 4 significant figures. a. Write the Ksp expression b. What is the concentration of Ca2+ in equilibrium with solid if [PO4 3-] is 5x10-5 M? b. How many moles of PO4 3- are delivered when 275 mL of solution described in sprayed unto a field?
- I II III [HIn]initial, in M ___________. ___________. ___________ Absorbance __0.925____ __0.634_____ ___0.366___ [HIn]equil, in M___________ ___________ ___________ [In-]equil, in M ___________ ___________ ___________ [H+]equil, in M 1.1 x 10-5M 5.5 x 10-6 M 2.4 x 10-6 M Keq. ___________ ___________ ___________ Average Keq _______________________ Fill in the data for each run in terms of Molarity based on the given absorbance and H+ at equilibrium.For a 0.0448 M aqueous solution of aniline, C6H5NH2 (Kb = 7.4E-10), determine the following. Kw = 1.0E-14. a. What is the concentration of the minor species present in the solution? b. What is the concentration of the major species present in the solution? c. What is the concentration of H3O+?What is the solubility of Pb3(PO4)2 if it's Ksp is 3.000e-44?