HSO4- is a weak acid so k is small for its dissociation and hence G= -RTlnK...
HSO4- is a weak acid so k is small for its dissociation and hence G= -RTlnK >0. since G = H - TS we anticipate dissociation of HSO4- to be endothermic however it is actually exothermic, how do we explain this?
Homework Answers
∆H for the dissociation of HSO4- is positive indeed, which makes it endothermic. But, it dissociates into H+ and sulfate ions. These ions get hydrated in water which is an exothermic process. So, the hydration of these ions releases energy. That's why, the process becomes exothermic.
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HSO4- is a weak acid so k is small for its dissociation and
hence G= -RTlnK...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its potassium salt KA. Unshaded spheres represent H atoms and shaded spheres represent A-ions. (K+, H30, OH-, and solvent H2O molecules have been omitted for clarity.) -HA -A IC (1) 12) Which of these solutions are buffers? A) (1) and (2) C) (1), (2) and (3) B) (1) and (3) D) All are buffer solutions. following pictures represent solutions at various stages in the titration...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its potassium salt KA. Unshaded spheres represent H atoms and shaded spheres represent A-ions. (K, H30, OH", and solvent H2O molecules have been omitted for clarity.) -HA -A (3) (1) 12) 12) Which of these solutions are buffers? A) (1) and (2) C) (1), (2) and (3) B) (1) and (3) D) All are buffer solutions The following pictures represent solutions at various stages in...
IV. Heat of reaction of a weak acid with weak base Total mass of solution Final temp. of solution...
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IV. Heat of reaction of a weak acid with weak base Total mass of solution Final temp. of solution Initial temp. of solutions AT Water AH reaction 40 9 29 C 22"C Calculation: Heat of reaction per mole water formed Moles of water formed AH reaction per mole H,O formed Calculation Heat of dissociation of weak acid and weak base AH dissociation (per mole)- Calculation: [AH Dissociation- AH reaction -AH Neutralization (from II)] IV. Enthalpy of Neutralization of...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its potassium salt KA. Unshaded spheres represent H atoms and shaded spheres represent A-ions. (K, H30, OH", and solvent H2O molecules have been omitted for clarity.) -HA -A (1) 12) 12) Which of these solutions are buffers? A) (1) and (2) C) (1), (2) and (3) B) (1) and (3) D) All are buffer solutions The following pictures represent solutions at various stages in the...
SHORT ANSWER: 11. Hypobromous acid, HBO pobromous acid. HR is a weak acid. Its acid dissociation...
SHORT ANSWER: 11. Hypobromous acid, HBO pobromous acid. HR is a weak acid. Its acid dissociation constant. K is 2.5 x 10 (20 points) a) Calculate the [H") of a 0.14-molar solution of HBrO. b) Write the correctly balanced net ionic equation for the reaction that occurs NaBro is dissolved in water and calculate the numerical value of the equilibrium constant for this reaction. c) Calculate the pH of a solution made by combining 40.0 milliliters of 0.14-molar HBrO and...
Determination of the Dissociation Constant ka, of a Weak Acid Part A Phosphoric acid is a...
Determination of the Dissociation Constant ka, of a Weak Acid Part A Phosphoric acid is a triprotic acid (three ionizable hydrogens). The values of its stepwise ionization constants are Kit = 75 x 10°,K6.2 x10, and K. = 4.2 x 10" 1. Write the chemical equation for the first ionization reaction of phosphoric acid with water. 2. Write the equilibrium constant expression Kat for this reaction. 3. What would be the pH of a solution when [H,PO) -(H.PO:] Part B...
Question HA is a weak acid. Its ionization constant, K, is 3.0 x 10) Calculate the...
Question HA is a weak acid. Its ionization constant, K, is 3.0 x 10) Calculate the pH of an aqueous solution with an initial NaA concentration of 0.060 M. Question 2 We place 0.150 mol of a weak acid, HA, in enough water to produce 100L of solution. The final pH of the solution is 1.18. Calculate the ionization contant, K., HA. Question We place 0.607 mol of a weak acid, HA, and 13.9 g of NaOH in enough water...
A buffer solution is able to maintain a constant pH when small amounts of acid or...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
50.0 mL sample of the weak acid the concentration of the weak acid = 0.15 M...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its potassium salt KA. Unshaded spheres represent H atoms and shaded spheres represent A-ions. (K+, H30, OH-, and solvent H2O molecules have been omitted for clarity.) -HA -A IC (1) 12) Which of these solutions are buffers? A) (1) and (2) C) (1), (2) and (3) B) (1) and (3) D) All are buffer solutions. following pictures represent solutions at various stages in the titration...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its potassium salt KA. Unshaded spheres represent H atoms and shaded spheres represent A-ions. (K, H30, OH", and solvent H2O molecules have been omitted for clarity.) -HA -A (3) (1) 12) 12) Which of these solutions are buffers? A) (1) and (2) C) (1), (2) and (3) B) (1) and (3) D) All are buffer solutions The following pictures represent solutions at various stages in...
need help
IV. Heat of reaction of a weak acid with weak base Total mass of solution Final temp. of solution Initial temp. of solutions AT Water AH reaction 40 9 29 C 22"C Calculation: Heat of reaction per mole water formed Moles of water formed AH reaction per mole H,O formed Calculation Heat of dissociation of weak acid and weak base AH dissociation (per mole)- Calculation: [AH Dissociation- AH reaction -AH Neutralization (from II)] IV. Enthalpy of Neutralization of...
The following pictures represent solutions that contain a weak acid HA (pka = 5.0) and its potassium salt KA. Unshaded spheres represent H atoms and shaded spheres represent A-ions. (K, H30, OH", and solvent H2O molecules have been omitted for clarity.) -HA -A (1) 12) 12) Which of these solutions are buffers? A) (1) and (2) C) (1), (2) and (3) B) (1) and (3) D) All are buffer solutions The following pictures represent solutions at various stages in the...
SHORT ANSWER: 11. Hypobromous acid, HBO pobromous acid. HR is a weak acid. Its acid dissociation constant. K is 2.5 x 10 (20 points) a) Calculate the [H") of a 0.14-molar solution of HBrO. b) Write the correctly balanced net ionic equation for the reaction that occurs NaBro is dissolved in water and calculate the numerical value of the equilibrium constant for this reaction. c) Calculate the pH of a solution made by combining 40.0 milliliters of 0.14-molar HBrO and...
Determination of the Dissociation Constant ka, of a Weak Acid Part A Phosphoric acid is a triprotic acid (three ionizable hydrogens). The values of its stepwise ionization constants are Kit = 75 x 10°,K6.2 x10, and K. = 4.2 x 10" 1. Write the chemical equation for the first ionization reaction of phosphoric acid with water. 2. Write the equilibrium constant expression Kat for this reaction. 3. What would be the pH of a solution when [H,PO) -(H.PO:] Part B...
Question HA is a weak acid. Its ionization constant, K, is 3.0 x 10) Calculate the pH of an aqueous solution with an initial NaA concentration of 0.060 M. Question 2 We place 0.150 mol of a weak acid, HA, in enough water to produce 100L of solution. The final pH of the solution is 1.18. Calculate the ionization contant, K., HA. Question We place 0.607 mol of a weak acid, HA, and 13.9 g of NaOH in enough water...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
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