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Kb for methylamine at 25°C is 4.4 x 10-4 what is its pH if 0.10M solution is used.
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- The base constant for ammonia, NH3, is Kb = 1.8 x 10-5. A solution was made up with ammonium chloride so that (NH4Cl] = 0.250 M and ammonium ion is a weak acid. What will be the pH of this solution? (The chloride ion is a spectator ion; it is the conjugate base of a strong acid, and so it has no acidic or basic contribution to the solution pH.)9) What will be the pH (aq., 25 oC) of 100.0 mL of a solution of 1.50 M C2H5NH3Br and 1.25 M C2H5NH2, after 2.00 mL of 10.00 M HCl has been added to it? Kb C2H5NH2 = 5.6 x 10–4(a) Calculate the pH in the solution formed by adding 10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoic acid (C6H5COOH, Ka = 6.3 * 10-5). (b) Calculate the pH in the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.
- An organic acid (HA) has a molecular weight of 100. g mol-1, a Kow = 5.6 and a K, = 2.7 x 10-2. If originally 2.0 g of the acid is dissolved in 100 mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100 mL of water, what will be the pH of the water? (Consider the equilibrium processes to be sequential and unrelated chemically) O 1.89 1.48 O 2.01 1.74 O 1.61Given that Ka's for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 x 10-4 and 5.4 x 10-10, respectively, calculate the pH of the following solutions: (a) The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b) The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.10. 0.02 mole of NH,OH and 0.03 mole of NH,Cl are mixed in 300 ml, what is the pH of the solution? Kb = 1.8 X 10s
- (a) Calculate the pH in the solution formed by adding10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoicacid (C6H5COOH, Ka = 6.3 x 10-5). (b) Calculate the pHin the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.A solution is prepared at 25 °C that is initially 0.051M in benzoic acid (HC,H,CO,), a weak acid with K,=6.3 × 10 °, and 0.079M in potassium benzoate (KC,H,CO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = [|A solution is prepared at 25 °C that is initially 0.30 M in methylamine (CH, NH,), a weak base with K, = 4.4 x 10 -4 and 0.12 M in methylammonium bromide (CH,NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. PH Continue
- The acid dissociation constants for sulfurous acid are: Ka = 1.2 x 10-2 and Kaz = 6.6 x 10-8. (i) Calculate the pH of a solution of 0.100 M H2SO3. (ii) Calculate the pH of a solution of 0.100M NazSO.. (iii) Calculate the pH of a solution resulting when equal volumes of the solutions described in parts (i) and (ii) are mixed.Determine the pH of the resulting solution when the following two solutions are mixed: 50.0 mL of 0.500 M HNO2 and 30.0 mL of 0.200 M Ca(OH).. The value of Ka for HNO2 is 6.8 × 104. 1 3 4 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. HNO:(aq) ОН (аq) H:O(1) NO: (aq) + + Before (mol) Change (mol) After (mol) 5 RESET 0.500 0.200 +x -X 0.500 + x 0.500 - x 0.200 + x 0.200 - x 0.0060 -0.0060 0.0120 -0.0120 0.0250 -0.0250 0.0190 -0.0190 0.0130 -0.0130V A solution is prepared at 25 °C that is initially 0.27M in chloroacetic acid (HCH₂CICO₂), a weak acid with K=1.3 × 10-³, and 0.48M in sodium chloroacetate (NaCH₂CICO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. -3 pH = 1 X Ś