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.
Consider an aqueous solution comprised of 0.150 M NH3 and 0.200 M NH4Cl. The pKb of...
2. Consider an aqueous solution comprised of 0.200 M NH3 and 0.150 M NHACI. The pKb of NH3 is 4.75 and the volume of the solution is 1.00 L. a) (2 marks) What is the pH of this solution? Show your work. b) (1 mark) What is the chemical reaction (balanced chemical equation) that occurs when NaOH solution is added to the original solution? c) (3 marks) How many moles of NaOH(s) could this solution react with before its pH...
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L upon addition of 0.090 mol of solid NaOH to the original buffer solution.
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L upon addition of 0.050 mol of solid NaOH to the original buffer solution. Thanks!
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb = 4.75.Part A Calculate the pH of 1.0 L of the original buffer, upon addition of 0.020 mol of solid NaOH.
QUESTIONS What is the pH of a 0.150 M aqueous solution of ammonium chloride (NH4Cl-)2 Kb (NH3)-1.2 x 10-5 0 A. 4.77 0 B.6.26 U 0 0 O D. 4.95 E. 4.84
How many moles of NH4Cl must be added to 3.0 L of aqueous 0.10 M NH3 to form a buffer whose pH is 9.00? Kb of NH3 is 1.8x10 (Assume addition of NH4Cl to the solution does not alter its volume). 0.36 O 0.54 0.18 O 0.42 0.11
A 0.200 M solution of HCl is added to a solution containing 0.150 moles of sodium phosphate (Na3PO4). The resulting solution is then diluted to exactly 1.00 L, at which time the pH was found to be pH 8.00. What is the concentration of H2PO4- in the solution? For phosphoric acid, Ka1 = 7.11 x 10-3, Ka2 = 6.32 x 10-8, and Ka3 = 7.1 X 10-13.
A buffer solution consists of 0.00300 M ammonia (NH3) and 0.00500 M ammonium chloride (NH4Cl). What is the change in pH when 0.00100 moles of NaOH are added to one litre of the solution without any change in volume? The pKa of NH4+ is 9.24.
Questions 1: A) Calculate the pH of a buffer solution that is 0.246 M in HCN and 0.166 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). B) Calculate the pH of a buffer solution that is 0.200 M in HC2H3O2 and 0.160 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) C) Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L of the...
Consider a buffer prepared by mixing 75ml of 0.03640 M ammonia (NH3) solution with 28ml of 0.02454 M ammonium chloride solution (pKb of ammonia is 4.75) 5. If you added 1 mL of 0.2550 M NaOH to 103 mL of pure water, what would the pH be?