15.0 mL of 0.50 M NaOH is added to a 100.-mL sample of 0.442 M NH3 (Kb for NH3 = 1.8 x 10–5). What is the equilibrium concentration of NH4+ ions?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
15.0 mL of 0.50 M NaOH is added to a 100.-mL sample of 0.442 M NH3...
15.0 mL of 0.50 M HCl is added to a 100.-mL sample of 0.462 M HNO2 (Ka for HNO2 = 4.0 x 10–4). What is the equilibrium concentration of NO2– ions?
20. If 10 mL of 0.05 M NaOH is added to a 20 mL solution of 0.1 M NaNO2 and 0.1 M HNO2, what will be the pH of the resultant solution? Assume that volumes are additive. Ka for HNO2 = 7.1x10-4. 21. At 25°C, 50.0 mL of 0.50 M NaOH(aq) is added to a 250 mL aqueous solution containing 0.30 M NH3 and 0.36 M NH4Cl. What is the pH of the solution after the addition of the base?...
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)
A solution prepared by mixing 100 mL of 0.10 M NaOH 140 mL of 0.10 M HCl 100 mL of 0.10 M NH3 has a pH of: Kb (NH3) = 1.8 x 10-5 A. 9.08 B. 4.57 C. 7.00 D. 4.92 E. 9.43
Calculate the pH after 4.0 mL of 0.50 M NaOH is added to 110.0 mL of a buffer made of 0.40 M CH3COOH and 0.50 M NaCH3COO. The Ka of acetic acid is 1.8 x 10.
A 20.0-mL sample of 1.50 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 12.00 mL of acid have been added to ammonia? Kb for NH3 = 1.8 × 10–5
A 20.00 mL sample of 0.150 M NH3 is being titrated with 0.200 M HCl. What is the pH after 20.00 mL of HCl has been added? Kb of NH3 = 1.8 × 10−5
Ka * Kb = Kw = 1.0 X 10-14 A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI. Calculate the pH of the solution after 0.00, 10.0, 20.0, 30.00, and 40.0 mL of acid have been added; Kb of NH3= 1.8 X 10-5 at 25 °C. Hint: First find the moles after each 10.00 ml of acid is added. Then find the concentration after equilibrium is reached.
A 20.0-mL sample of 1.50 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 12.00 mL of acid have been added to ammonia? Kb for NH3 = 1.8 × 10–5 5.93 9.30 8.06 9.07 10.45
Part C A 75.0-mL volume of 0.200 M NH3 (Kb = 1.8 x 10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 15.0 mL of HNO3 . Express your answer numerically. Part D A 52.0-mL volume of 0.35 M CH3COOH (Ka = 1.8 x 10-5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 19.0 mL of NaOH. Express your answer numerically.