Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH solution. Calculate the pH for the point at which 100 mL of the base has been added. Show all calculations
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.
Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH...
5. Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH solution. Calculate the pH for [10 pts] the point at which 100 mL of the base has been added. 5. Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH solution. Calculate the pH for [10 pts] the point at which 100 mL of the base has been added.
50.0 mL of 0.090 M nitrous acid (HNO2, Ka = 7.1 x 10-4), is titrated with 0.100 M NaOH, requiring 45.0 mL of strong base to reach the equivalence point. (a) What will be the pH after 35.0 mL of NaOH have been added? (b) What will be the pH at the equivalence point? (c) What will be the pH after 60.0 mL of NaOH have been added?
A 15.0 mL sample of 0.21 M nitrous acid (HNO2), Kg = 4.6x10-4) is titrated with 0.15 M NaOH. Calculate the pH after the addition of the following volumes of base: a. 0.00 mL b. 10.00 mL c. 21.00 mL d. 25.00 mL
A 15.0 mL sample of 0.21 M nitrous acid (HNO2), Ka = 4.6x10-4) is titrated with 0.15 M NaOH. Calculate the pH after the addition of the following volumes of base: a. 0.00 mL b. 10.00 mL c. 21.00 mL d. 25.00 mL
1.A 25.00 ml smaple of 0.523 M nitrous acid, HNO2, solution is titrated with a 0.213 M NaOH. For HNO2, Ka = 4.0 X 10^-4 a) What is the pH before any NaOH is added? b) Write the reaction that takes place as KOH solution is added to the HNO2 solution. c) write the reaction that determines the pH at the equivialnce point. -What is the pH at the equivilance point -what is the pH at the 1/2 equivilance point...
2. A sample of 50 ml of nitrous acid (KA = 5.6 x 10“) is titrated with 0.070 M NaOH. The equivalence point is reached after the addition of 43.2 ml of the strong base. a) (3 marks) What is the pH of the solution at the equivalence point? b) (3 marks) What is the pH of the solution after 50 ml of NaOH has been added to the original nitrous acid solution?
2. A sample of 65 ml of nitrous acid (KA = 5.6 x 104) is titrated with 0.075 M NaOH. The equivalence point is reached after the addition of 44.5 ml of the strong base. a) (3 marks) What is the pH of the solution at the equivalence point? b) (3 marks) What is the pH of the solution after 60 ml of NaOH has been added to the original nitrous acid solution?
2. A sample of 60 ml of nitrous acid (KA= 5.6 x 104) is titrated with 0.075 M NaOH. The equivalence point is reached after the addition of 45.8 ml of the strong base. a) (3 marks) What is the pH of the solution at the equivalence point? I b) (3 marks) What is the pH of the solution after 60 ml of NaOH has been added to the original nitrous acid solution?
1.A 20.0-mL sample of 0.150 M nitrous acid (HNO:) is titrated with 0.200 M NaOH at 25°C. Calculate the pH after 10.0 mL of the NaOH solution has been added. K. for HNO2 = 4.5x 10 A) 3.65 B) 10.35 C) 10.95 D) 3.17 E) 3.52 2. Consider the following reaction: NO, (ag)+H(aq) + l:(s) NO:(g) + H20(D 10, (ag) Which of the following statements is correct? A) The species reduced is I B) Oxidation umber of oxygen increases C)...
A 50.0 mL sample of 0.11 M nitrous acid is titrated with 0.22 M NaOH. Calculate the pH to one decimal place when the following volumes of NaOH have been added. 0.00 mL 22.0 mL 25.0 mL 33.0 mL