IWCI. 5) What is the H30 pH values? (a) 0.00 concentration to the correct number of...
AUSWC. 5) What is the H30* concentration to the correct number of significant figures for solutions with the following pH values? (a) 0.00 (b) 7.00 (C) 2.63 (d) -0.42 (e) 11.21 (a) Calculate the pH of a buffer solution that is 0.45 M in NH4Cl and 0.15 M in NH3. (b) How would you prepare an NH4Cl-NH3 buffer that has a pH of 9.00? (The Kb for NH3 is 1.8 x 10)
both 5 and 6 please 5) What is the H30* concentration to the correct number of significant figures for solutions with the following pH values? (a) 0.00 (b) 7.00 (c) 2.63 (d) -0.42 (e) 11.21 6) (a) Calculate the pH of a buffer solution that is 0.45 M in NH4Cl and 0.15 M in NH3. (b) How would you prepare an NHACI-NH3 buffer that has a pH of 9.00? (The K. for NH3 is 1.8 x 10)
Answer Both questions please. (11) (6 points) What is the HO. concentration to the correct number of significant figures for solutions withthe following pH values? (a) pH-0.00 (b) pH-7.00 (pH--0.20 ID) (4 points) Calculate the pH of 0.16 M KOH solution.
What amount of NH4Cl must be added to 50.0 mL of 0.30 M NH3 in order to produce a buffer of pH 9.00? Assume the addition of NH4Cl does not change the volume of the solution. Kb = 1.8 × 10-5 for NH3
4.13 Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, pKa=−logKa The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH=pKa+log[base][acid] Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. Part B How many grams of dry NH4Cl need to be added to 2.10 L of a 0.400 M solution of ammonia,...
help calculating pH. not sure if answwer is correct (B)Increases concentration of O2 (C) Equilibrium constant decreases (D) Equilibrium constant increases 28. Consider 0.15 M NH3 solution? Kb of ammonia is 1.8 x 105 (ii) What is the pH? a 11.68 (b. 2.79 3.42 C. d. 10.58 Which species predominate, reactants or products in a solution of (iii) Calculate the % dissociation. (iv)
Calculate the pH of a buffer prepared by dissolving 0.10 mol of NH4Cl in 1.00 L of 0.15 M NH3. Kb = 1.8 x 10 % for NH3. O a. 11.34 O b. 2.72 O ü O ö Oe. 4.56
What is the pH of a buffer formed from 50 mL of 15.0 M NH3 and 53.5 g of NH4Cl in enough water to make 500 mL of solution? (Kb = 1.8 x 10-5)
What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 5.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3. (Select One) 10.26 or 11.13
A certain weak base has a K of 7.50x107. What concentration of this base will produce a pH of 10.23? Number 00017 NH3 is a weak base (Kb = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.069 M in NH4Cl at 25 °C? Number pH-