pH of solution when 25.00 mL of o. 100M ammonia solution is treated with 10.00mL of...
A 0.102 M solution (25.00 mL) of ammonia (pKb =4.76) is titrated with 0.100 M hydrochloric acid. Calculate the pH of the solution after the addition of 15.91 mL acid solution. Present your answer as a numerical value only, to 2 decimal places .
The following table shows the data for the titration of 25.00 mL of 0.200 M CH3COOH (pKa= 4.75) with 0.200 M NaOH (sodium hydroxide). Volume of NaOH added (mL) pH of the solution (measured) Mols of CH3COO-formed Mols CH3COOH remained pH of the solution (calculated) 0.00 2.72 0 0.005 2.70 10.00 4.57 0.002 0.003 4.57 12.50 4.7 0.0025 0.0025 4.75 24.90 7.14 0.0049 2 x 10-5 7.14 24.99 8.14 0.00 2 x 10-6 8.15 25.00 8.88 0.005 0 8.88 25.01...
Calculate the pH values in 20.00 mL of a 0.500 M solution of ammonia to which the following volumes (in mL) of a 0.500 M HBr solution are added in a titration (pKb of NH3 = 4.75). (5) a. 0.00 b. 6.00 c. 10.00 d. 20.00 e. 30.00
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
A 1.000-mL aliquot of a solution containing Cu2* and Ni2+ is treated with 25.00 mL of a 0.04152 M EDTA solution. The solution is then back titrated with 0.02204 M Zn2 solution at a pH of 5. A volume of 16.29 mL of the Zn2+ solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and N solution is fed through an ion-exchange column that retains NP. The Cu2" that passed through the column...
A chemist starts her experiments with 25.00 mL of 0.125 mol L-1 NaCN solution. The pKa of HCN = 9.20. a) What volume of 0.100 mol L-1 HCl will be required to fully react with the above salt? b) After the reaction in part a) takes places, will the pH of the solution be acidic, basic or neutral? c) What volume of 0.100 mol L-1 HCl is needed to adjust the pH of the originally provided solution to pH =...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.04328 M EDTA solution. The solution is then back titrated with 0.02246 M Zn2 solution at a pH of 5. A volume of 21.60 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...
A 1.000-mL aliquot of a solution containing Cu and Ni2 is treated with 25.00 mL of a 0.05182 MEDTA solution. The solution is then back titrated with 0.02198 M Zn2 solution at a pH of 5. A volume of 21.82 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu and Ni2 solution is fed through an ion-exchange column that retains Ni2. The Cu2 that passed through the column is...
10. Calculate the pH of a solution made by mixing 40.0 mL of 0.150 M ammonia with 10.0 mL of 0.100 M HCl
5.00 mL of 0.250 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl). The Kb for ammonia is 1.75 x 10-5. What is the pH of the solution after the addition of 25.00 mL of HCl?