2. Determine the pH of the following solutions (a) 0.15 M NH3 (aq) (b) 6.0 M...
Calculate the pH and pOH of the following aqueous solutions: (a) 0.15 mol·L–1 CH3COOH(aq); (b) 0.15 mol·L–1 CCl3COOH (aq); (c) 0.15 mol·L–1 HCOOH(aq). When the pH of a 0.10 mol·L–1 HClO2 aqueous solution was measured, it was found to be 1.2. What are the values of Ka and pKa of chlorous acid? (b) The pH of a 0.10 mol·L–1 propylamine, C3H7NH2, aqueous solution was measured as 11.86. What are the values of Kb and pKb of propylamine?
Calculate the pH and pOH of the following aqueous solutions: (a) 0.15 mol·L–1 CH3COOH(aq); (b) 0.15 mol·L–1 CCl3COOH (aq); (c) 0.15 mol·L–1 HCOOH(aq). When the pH of a 0.10 mol·L–1 HClO2 aqueous solution was measured, it was found to be 1.2. What are the values of Ka and pKa of chlorous acid? (b) The pH of a 0.10 mol·L–1 propylamine, C3H7NH2, aqueous solution was measured as 11.86. What are the values of Kb and pKb of propylamine?
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
4. Calculate the percent ionization and pH of the following solutions: a. 0.175 M NH3 Kg = 1.8 x 10-5. b. 35.0 mL of 0.175 M NH3 is mixed with 15.0 mL of 0.10 M HCl. c. 50.0 mL of 0.275 M acetic acid is mixed with 100. mL of 0.100 M HCl. d. The equivalence point of a 50.0 mL solution of 0.120 M acetic acid titrated by 0.100 M NaOH.
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...
Calculate the [H^+], [OH^-], pH and pOH of the following solutions: a. 0.01 M HCl (aq) b. 0.02 M NaOH (aq)
1)A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid.Kb of NH3 is 1.8 × 10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the mixture is [ Select ] ["at", "before", "after"] the equivalence point on the titration curve.2) The pH of the solution after...
3. W hat is the pH of each of the following solutions? a. 0.0001 M HCl o 2 b. 0.01 M HNO3 。 c. A solution with a [H3O'] concentration of 5 x 106 M? d. A solution with a [OH-] concentration of 8 x 10 3?
a) Calculate the pH of a buffer system that contains o.200 M of NH3(aq) and o.200 M of NH4Cl(aq). The Kb of NH3(aq) is 18 x 10-5. Consult Textbook Numerical Answer pH b) Calculate the change in pH when 6.00 mL of 100 M HCl is added to 100.0 mL of the buffer solution. Numerical Answer: c) Calculate the change in pH when 6.00 mL of o.100 M NaOH is added to 100.0 mL of the buffer solution. Numerical Answer:
The solutions below are prepared. Which solution is the most basic? Group of answer choices 0.15 M KOH (aq) 0.1 M Mg(OH)2(aq) 0.05 M NH3 (aq) 0.25 M H2SO4 (aq) 0.1 M HCl (aq)