An initial 0.010 M solution of a weak acid (HA) is measured to have 0.0015 M of its conjugate weak base (A") in solution at equilibrium. Calculate the pKa for the weak acid. 2.82 3.58 3.65 0.18 0.82
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A: Solution - According to the question - Given - we use Henderson Hasselbach equation, pH = pKa + log…
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A: The solution is given below -
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A: MH2CO2 = 1.100 M VH2CO2 = 225.3 mL = 0.2253 L MKOH = 1.200 M VKOH = 99.62 mL = 0.09962 L pKa = 3.74
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- Write the dissociation equation for c2h2o4 (acid or base), write the expression for the constant equilibrium according to the law of mass action for c2h2o4, from pKa calculate the value of Ka and Kb for c2h2o4How do you find the equilibrium constants value for Na2CO3,NH4Cl,ZnCl2 and KAl(SO4)2. And would they Ka or Kb?Benzoic 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?
- The equalibrium constant for the following equation HC2H3O2(aq) + H2O(l) ⇌ H3O+(aq) + C2H3O2-(aq)Consider a solution that is made from mixing 122.3ml of 0.333M ZnCl2 and 83.57ml of 0.654M Na2CO3 a. What is the concentration of cations and anions at equilibrium(in molarity)? Use x-is-small approximation. b. What is the ‘net’ amount of precipitate produced(in moles)? ksp (ZNCO3) = 1 x 10^-10Write the Ksp expression for the sparingly soluble compound silver sulfide, Ag2S. Ksp = If either the numerator or denominator is 1, please enter 1. --- Write the Ksp expression for the sparingly soluble compound silver iodide, AgI. If either the numerator or denominator is 1, please enter 1. Ksp =
- What's the molar solubility of Ag2CrO4 in a solution containing 0.050M AgNO3? Given: Ag2CrO4 Ksp=1.12x10-12Groundwater containing 0.0001468 M of Mg2+ is at equilibrium. Use the solubility constant Ksp=1.35×10−11. Assuming no other ions are present, what is the equilibrium pH? Round the final answer to only 2 decimals places.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 ×…
- Solid sodium hydroxide is slowly added to 175 mL of a manganese(II) bromide solution until the concentration of hydroxide ion is 0.0521 M. The maximum amount of manganese(II) ion remaining in solution is __ M. Solubility Product Constants (Ksp at 25 oC) Type Formula Ksp Bromides PbBr2 6.3 × 10-6 AgBr 3.3 × 10-13 Carbonates BaCO3 8.1 × 10-9 CaCO3 3.8 × 10-9 CoCO3 8.0 × 10-13 CuCO3 2.5 × 10-10 FeCO3 3.5 × 10-11 PbCO3 1.5 × 10-13 MgCO3 4.0 × 10-5 MnCO3 1.8 × 10-11 NiCO3 6.6 × 10-9 Ag2CO3 8.1 × 10-12 ZnCO3 1.5 × 10-11 Chlorides PbCl2 1.7 × 10-5 AgCl 1.8 × 10-10 Chromates BaCrO4 2.0 × 10-10 CaCrO4 7.1 × 10-4 PbCrO4 1.8 × 10-14 Ag2CrO4 9.0 × 10-12 Cyanides Ni(CN)2 3.0 × 10-23 AgCN 1.2 × 10-16 Zn(CN)2 8.0 × 10-12 Fluorides BaF2 1.7 × 10-6 CaF2 3.9 × 10-11 PbF2 3.7 × 10-8 MgF2 6.4 × 10-9 Hydroxides AgOH 2.0 × 10-8 Al(OH)3 1.9 × 10-33 Ca(OH)2 7.9 × 10-6 Cr(OH)3 6.7 × 10-31 Co(OH)2…The pH of a saturated solution of a metal hydroxide MOH is 9.55. Calculate the Ksp for this compound. Enter the answer in scientific notation.5. For the solubility of a molecule A2B explain how the concentrations of the species A+ and B2- dictate if a precipitate will form or not. Formulate your answer using the idea of the reaction quotient (Q) and Le Chatlier’s principle. (hint: What must be true about the concentrations of these two species with regard to the Ksp for a precipitate to form or not form.)