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- The equivalent conductance of a 0.0140N solution of chloroacetic acid is 109.0 at 25 degrees C. What is the ionization constant (Ka) of chloroacetic acid?The equivalent conductance of a 0.0140N solution of chloroacetic acid is 109.0 at 250C. What is the ionization constant (Ka) of chloroacetic acid?The molar conductivity of a 0.05 M solution of a weak base (B) is 4.9 x 10-1 mSm2/mol and the sum of the limiting ionic conductivities for BH+ and OH‑ is 23.7 mSm2/mol. What is the value of the base constant Kb?
- Use the equation below to find the partial pressure of H2 above liquid water given a total pressure of 101.325 KPa and a temperature of 90 °C. The vapor pressure of water at 90°C is 70.10KPA. PH = Protal- PH30The conductivity of 0.001 M acetic acid is 4 × 10-5 S/cm. Calculate the dissociation constant of acetic acid, if molar conductivity at infinite dilution for acetic acid is 390 S cm2/mol.9. The molar conductivity values at infinite dilution, in units of Sm?mol1, of NHẠCI, NaCl and N2OH are 1.497 x 10², 1.2645 x 10² and 2.478 x 10², respectively. (a) Calculate the molar conductivity at infinite dilution of NH4OH. (b) The molar conductivity of 0.0100 moldm3 NH,OH is 1.13 x 103 Sm?mol. What is the degree of dissociation and the dissociation constant, Kp, of 0.0100 moldm3 NHẠOH?
- According to Henry’s law the atmospheric partial pressure of CO2 dictates the concentration of aqueous CO2 according to the following equilibrium expression where k is the Henry’s law constant for CO2. CO2 (g) <-> CO2 (aq) k=1x10^-1.5 The acid dissociation constant Ka for carbonic acid applies to CO2 (aq). Given pKa1=6.35 and pKa2=10.33 and the fact that the partial pressure of CO2 in the atmosphere is 10^-3.5 atm, find the pH of water in equilibrium with the atmosphere.1. It is found that 16.34 mL of a solution containing Ni* is required to titrate a sample of pure KCN weighing 0.5024 g. The reaction is Ni* + 4 CN" → Ni(CN),“ . Calculate the molarity of the nickel solution. From the following data calculate the normalities of the acid and base solutions: weight of pure Na2CO3 = 0.2448 g; volume of acid = 43.65 mL ; volume of base used in back titration = %3D 0.84 mL ; 1.000 mL of base = 0.982 mL of acid. Reaction: CO, + 2H* → H2CO3Assuming 100% dissociation, calculate the freezing point (?f) and boiling point (?b) of 3.29 ? AgNO3(aq).
- In which solution will NH,NO, be most soluble in? 1.0 Μ ΗΝO; О 1.0 м КОН O 1.0 M NaCl O 1.0 M NH4B1 Ο 1.0 ΜΚΝ, 1.0 Μ KNΟ;To analyze an aspirin sample, 0.3470 g of crushed tablets are weighed and treated with 50.00 mL 0.1155 M sodium hydroxide, boiling for 10 minutes. Under these conditions the acid acetylsalicylic (MW, 180) reacts according to: CH3COO-C6H4-COOH + 2 OH- → OH-C6H4-COO- + CH3COO- The excess NaOH is then titrated with 11.5 mL of 0.2100 M HCl. What is the purity of said show ?.Calculate the ionization constant of propanoic acid (CH3CH2COOH) using the following data: Parameter Value pH 4.51 1.18 x 105 µS-cm1·M-1 3.866 x 105 uS-cm-1·M-1 Molar conductivity of HZ, Am Conductivity at infinite dilution, Ao To calculate the ionization constant, calculate the following: (report all answers in 3 SF) 1. fraction of propanoic acid ionized: 2. equilibrium concentrations of the conjugate base of propanoic acid and hydronium ion: M 3. initial concentration of the acid: M 4. ionization constant: