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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?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 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?
- 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 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* → H2CO3To 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 ?.
- Assuming 100% dissociation, calculate the freezing point (?f) and boiling point (?b) of 3.29 ? AgNO3(aq).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: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;