Calculate the pH and pOH of the following aqueous solutions: (a) 0.15 mol·L–1 CH3COOH(aq); (b) 0....
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?
Homework Answers
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Calculate the pH and pOH of the following aqueous solutions: (a) 0.15 mol·L–1 CH3COOH(aq); (b) 0....
Calculate the pH and pOH of the following aqueous solutions: (a) 0.15 mol·L–1 CH3COOH(aq); (b) 0.15...
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?
Which of the following 0.10 M aqueous solutions gives the highest pH? A) CH3COOH (pKa =...
Which of the following 0.10 M aqueous solutions gives the highest pH? A) CH3COOH (pKa = 4.75) B) HF (PK:= 3.45) C) H3PO4 (pKal = 2.12) D) HCIQ (Ka=2.00) E) Since all are acids, the pH is the same for all solutions. 5. Which one of the following salts gives an acidic aqueous solution? A) CsNO3 B) CaCl2C ) LiF D) Cr(CIO4)3 E) NaCH3CO2 6. 7. All of the following are strong acids except A) HCIQB) HC104 C) HI D)...
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF)...
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
2. For each of the following aqueous solutions of ionic compounds, calculate the pH and pOH;...
2. For each of the following aqueous solutions of ionic compounds, calculate the pH and pOH; look up Ka and Kb values as needed. a. 0.500 M sodium bromide b. 0.357 M calcium nitrate
1. Calculate the concentration of H3O+ for an aqueous solution with a pH of 1.2 A)...
1. Calculate the concentration of H3O+ for an aqueous solution with a pH of 1.2 A) 6.3 x 10-7M B ) 1.6 x 108 M. C) 1.0 x 10-14 M. D) 6.20 x 10-2 M E) 4.0 x 10-4M 2. Calculate the concentration of OH- for an aqueous solution with a pH of 13.8. A) 0.64 M B) 4.0 x 10-5M C) 1.5 x 10-5M D) 1.0 x 10-14 M E) 2.5 x 10-10 M 3. Which of the following...
11. a) The pH of 0.015 M HNO2(aq) was measured as 2.63. What are the values...
11. a) The pH of 0.015 M HNO2(aq) was measured as 2.63. What are the values of Ka and pKa of nitrous acid? b) The pH of 0.10 M butylamine, CaH,NH2(aq) was measured as 12.04. What are the percentage protonation and the values of Kb and pkb of butylamine?
1. What is the pOH of an aqueous solution of 0.171 M hydrobromic acid? pOH =...
1. What is the pOH of an aqueous solution of 0.171 M hydrobromic acid? pOH = 2. What is the pH of an aqueous solution of 1.77×10-2 M nitric acid? pH = 3. What is the pOH of an aqueous solution of 3.08×10-2 M potassium hydroxide? pOH = 4. What is the pH of an aqueous solution of 3.08×10-2 M potassium hydroxide? pH = 5. Calculate the pH of a 0.409 M aqueous solution of nitrous acid (HNO2, Ka =...
pH LI Calculate the pH of the following solutions: Solution (a) 0.10 M CH3COOH 12.9 (b)...
pH LI Calculate the pH of the following solutions: Solution (a) 0.10 M CH3COOH 12.9 (b) 0.10 M NH3 Mixture of 25.00 mL of 0.10 M HCl + 25.00 mL of 0.10 NaOH Mixture of 20.00 mL of 0.10 M NaOH + 20.00 mL of 0.10 M CHCOOH (e) Mixture of 20,00 mL of 0.10 M HCI + 20.00 mL of 0.10 M NH; Saturated Mg(OH)2 (s) aqueous solution if water's dissociation is negligible K[CH3COOH) = 1.8x10-Kb [NH:] = 1.8*10-9;...
Acetic Acid (CH3COOH) has a Ka value of 8 x 1-5. If I have a 0.15...
Acetic Acid (CH3COOH) has a Ka value of 8 x 1-5. If I have a 0.15 M acetic acid solution, what are the following values? pH pOH [H3O+] [OH-] If I add 0..15 M sodium acetate to the solution what is the pH value here? Remember that pH = pKa + log [A-]/[HA].
Calculate the hydroxide ion concentration and the POH in an aqueous solution with a pH =...
Calculate the hydroxide ion concentration and the POH in an aqueous solution with a pH = 2.3 at 25°C. a. [OH 1 - 2.0 * 10-12M : POH - 2.30 b. [OH 7 -2.0 * 10-11M: POH = 11.70 C[OH 7 -5.0 x 10-3 M : POH = 11.70 d. [OH ) - 2.0 x 10-12 M : POH = 11.70 e.[OH ) - 2.0*10-12M : POH -8.50 Which of the following solutions is a good buffer system? a. A...
Which of the following 0.10 M aqueous solutions gives the highest pH? A) CH3COOH (pKa = 4.75) B) HF (PK:= 3.45) C) H3PO4 (pKal = 2.12) D) HCIQ (Ka=2.00) E) Since all are acids, the pH is the same for all solutions. 5. Which one of the following salts gives an acidic aqueous solution? A) CsNO3 B) CaCl2C ) LiF D) Cr(CIO4)3 E) NaCH3CO2 6. 7. All of the following are strong acids except A) HCIQB) HC104 C) HI D)...
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
2. For each of the following aqueous solutions of ionic compounds, calculate the pH and pOH; look up Ka and Kb values as needed. a. 0.500 M sodium bromide b. 0.357 M calcium nitrate
1. Calculate the concentration of H3O+ for an aqueous solution with a pH of 1.2 A) 6.3 x 10-7M B ) 1.6 x 108 M. C) 1.0 x 10-14 M. D) 6.20 x 10-2 M E) 4.0 x 10-4M 2. Calculate the concentration of OH- for an aqueous solution with a pH of 13.8. A) 0.64 M B) 4.0 x 10-5M C) 1.5 x 10-5M D) 1.0 x 10-14 M E) 2.5 x 10-10 M 3. Which of the following...
11. a) The pH of 0.015 M HNO2(aq) was measured as 2.63. What are the values of Ka and pKa of nitrous acid? b) The pH of 0.10 M butylamine, CaH,NH2(aq) was measured as 12.04. What are the percentage protonation and the values of Kb and pkb of butylamine?
pH LI Calculate the pH of the following solutions: Solution (a) 0.10 M CH3COOH 12.9 (b) 0.10 M NH3 Mixture of 25.00 mL of 0.10 M HCl + 25.00 mL of 0.10 NaOH Mixture of 20.00 mL of 0.10 M NaOH + 20.00 mL of 0.10 M CHCOOH (e) Mixture of 20,00 mL of 0.10 M HCI + 20.00 mL of 0.10 M NH; Saturated Mg(OH)2 (s) aqueous solution if water's dissociation is negligible K[CH3COOH) = 1.8x10-Kb [NH:] = 1.8*10-9;...
Calculate the hydroxide ion concentration and the POH in an aqueous solution with a pH = 2.3 at 25°C. a. [OH 1 - 2.0 * 10-12M : POH - 2.30 b. [OH 7 -2.0 * 10-11M: POH = 11.70 C[OH 7 -5.0 x 10-3 M : POH = 11.70 d. [OH ) - 2.0 x 10-12 M : POH = 11.70 e.[OH ) - 2.0*10-12M : POH -8.50 Which of the following solutions is a good buffer system? a. A...
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