For solving this question we will be using the concept of salt hydrolysis. Salt in presence of water( high dielectric constant) undergoes dissociation to form its parent acid and base. We can infer that since it is salt of strong acid(HCL) and weak base(NH4OH) therefore the pH of the salt solution will be less than 7. Detailes solution is given in the image.
QUESTIONS What is the pH of a 0.150 M aqueous solution of ammonium chloride (NH4Cl-)2 Kb...
What is the pH of a 0.250 M aqueous solution of ammonium chloride (NH4+Cl-)? Kb (NH3) = 1.2 × 10-5 A. 5.04 B. 4.95 C. 4.77 D. 4.84 E. 6.26
What is the pH of a 1.50 mol/L solution of ammonium chloride (NH4Cl) kb = 1.8 10^-5 2. What is the pH of a 1.50 mol/L solution of ammonium chloride (NH4Cl)?
What is the pH of a 0.820 M solution of ammonium chloride, NH4Cl? At 25 °C, ko for ammonia, NH3, is 1.8 x 10-5: Kw = 1.0 x 10-14 Select one: Ca. 4,67 b. 5.49 OOO c. 4.34 d. 0.09 e. 2.42
Calculate the approximate pH of an aqueous solution of ammonium chloride, NH4Cl , 0.03 M, and sodium acetate, CH3COONa, 0.12 M at 25°C. (Note: consider one decimal place for the pH answer.) pKa NH4+/NH3 = 9.24 pKa CH3COOH/CH3COO- = 4.76
Kb for NH3 is 1.8x10^-5. What is the pH of a 0.35-M aqueous solution of NH4Cl at 25°C?
What is the pH of a 0.10 M NH4Cl solution? (Kb(NH3) = 1.8 x 10-5 A. 7.25 B. 11.3 C. 5.63 D. 3.40 E. 10.6
What is the pH of a 0.01 M NH4Cl solution? (Kb(NH3) = 1.8 x 10-5 A. 7.25 B. 11.3 C. 5.63 D. 3.40 E. 10.6
please answer both questions QUESTION 18 An aqueous solution contains 0.27 M ammonium chloride, NH4Cl. One liter of this solution could be converted into a buffer by the addition of 1.0.27 mol NH4Br 6.0.27 mol HBC 6.0.13 mol HCI 1.0.26 mol NH3 9.0.26 mol KCI QUESTION 19 A 29.9 ml. sample of 0.299 M methylamine, CH3NH2, is titrated with 0.331 M hydroiodic acid, HI at 25°C. (Xb for methylamine is 4.2 * 10-4) What is the pH at the equivalence...
(a) Determine the Kb of a weak base if a 0.847 M aqueous solution of the base at 25°C has a pH of 10.88. (Enter your answer in scientific notation.) (b) Determine the concentration of a solution of ammonium chloride (NH4Cl) that has pH 5.19 at 25°C. (c) Calculate the pH of a 0.011 M NaF solution. (Ka for HF = 7.1 × 10−4.)
Consider an aqueous solution comprised of 0.150 M NH3 and 0.200 M NH4Cl. The pKb of NH3 is 4.75 and the volume of the solution is 1.00 L. a) What is the pH of this solution? Show your work. b) What is the chemical reaction (balanced chemical equation) that occurs when NaOH solution is added to the original solution? c) How many moles of NaOH(s) could this solution react with before its pH rises to 10.00? Show your work.