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So pH = -2.207
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1" . I TV a OH Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa = 3.5, in equilibrium....
Predicting pH Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with...
Predicting pH
Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H+) = /K,C, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H2 Hint: First figure out what happens to the concentrations HA(aq) + H2O(0) A (aq)...
Exam Question Example #2 OH Imagine you have a 0.125 M aqueous solution of as pirin, an acid drug with pKg 3.5, in...
Exam Question Example #2 OH Imagine you have a 0.125 M aqueous solution of as pirin, an acid drug with pKg 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try [H*]= /KaCo or [OH] = /KbCo b) Predict what would happen to the pH when you add more H20 Hint: First figure out what happens to the concentrations HA(aq) + H20(I)...
a OH Old Exam Question Example #2 Imagine you have a 0.125 M aqueous solution of...
a OH Old Exam Question Example #2 Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pk, = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H*] = KC, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H20 Hint: First figure out what happens to the concentrations...
Please enan wak one (hightel), Thamkyou! Let's Think OH Imagine you have a 0.125 M aqueous...
Please enan wak one (hightel), Thamkyou! Let's Think OH Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa 3.5, in equilibrium. Predict what would happen to the pH when: you add more A"; you add OH you add more H20; Use both, kinetic and thermodynamic arguments. Chemical Thinking
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than...
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...
A 0.100 molar solution of weak acid HA has pH of 2.45 What is pka? Hint,...
A 0.100 molar solution of weak acid HA has pH of 2.45 What is pka? Hint, find [H+] from pH and plug it into into ICE as 'X' HA (+H20) А" <> H30* 0.100 M 0 0 С E 0.100 - X х х solve for Ka, then pka Ka = [H30*1 [A]/[HA] 39 24 6.1 45 5.4 Consider the titration of 25.00 ml of 0.100 MHA with 25.0 0.100 M NaOH. HA +H20 --> A™ + H307 The Ka...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions A) KOH, HNO2 B) H2S03. KHSO3 C) HONH2, HONH3CI D) NaCI, HCI E) RbOH, HF 10) The Henderson-Hasselbalch equation is acid) acid] A) pH- pKa log basel base] D) pH - pKaobase [acid 11) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kp for A- A) A (aq) H30+ (aq) HA (aq) H20 0) B) HA (aq) + OH-(aq) 근...
20. You need to prepare an acetate buffer of pH5.24from-a: 0.810Macetic acid solution and a 2.29MKOHsolution....
20. You need to prepare an acetate buffer of pH5.24from-a: 0.810Macetic acid solution and a 2.29MKOHsolution. If you have 880mL of the acetic acid solution, how many milliliters of the KOHsolution do you need to add-to- make a buffer of pH95.24? The pKa of acetic acid is 4.76.1 T mLmLT 21.-1f-a-buffer solution-is-0.450.M-in-a-weak-acid-(Ka=7.3x10^-6)-and-0.110-M-in-its-conjugated base. what-is-the-ph Ph=1 13.A monoprotic weak acid, HAHA, dissociates in water according to the reactionſ HA(aq)---H-(aq)+A-(aq)HA(aq)---H+(aq)+A-(aq) The equilibrium concentrations of the reactants and products are [HAl=0.290M[ [H-]=2.00X10-4M. and...
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...
Need help on questions 1-3 Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka...
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
Predicting pH
Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H+) = /K,C, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H2 Hint: First figure out what happens to the concentrations HA(aq) + H2O(0) A (aq)...
Exam Question Example #2 OH Imagine you have a 0.125 M aqueous solution of as pirin, an acid drug with pKg 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try [H*]= /KaCo or [OH] = /KbCo b) Predict what would happen to the pH when you add more H20 Hint: First figure out what happens to the concentrations HA(aq) + H20(I)...
a OH Old Exam Question Example #2 Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pk, = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H*] = KC, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H20 Hint: First figure out what happens to the concentrations...
Please enan wak one (hightel), Thamkyou! Let's Think OH Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa 3.5, in equilibrium. Predict what would happen to the pH when: you add more A"; you add OH you add more H20; Use both, kinetic and thermodynamic arguments. Chemical Thinking
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...
A 0.100 molar solution of weak acid HA has pH of 2.45 What is pka? Hint, find [H+] from pH and plug it into into ICE as 'X' HA (+H20) А" <> H30* 0.100 M 0 0 С E 0.100 - X х х solve for Ka, then pka Ka = [H30*1 [A]/[HA] 39 24 6.1 45 5.4 Consider the titration of 25.00 ml of 0.100 MHA with 25.0 0.100 M NaOH. HA +H20 --> A™ + H307 The Ka...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions A) KOH, HNO2 B) H2S03. KHSO3 C) HONH2, HONH3CI D) NaCI, HCI E) RbOH, HF 10) The Henderson-Hasselbalch equation is acid) acid] A) pH- pKa log basel base] D) pH - pKaobase [acid 11) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kp for A- A) A (aq) H30+ (aq) HA (aq) H20 0) B) HA (aq) + OH-(aq) 근...
20. You need to prepare an acetate buffer of pH5.24from-a: 0.810Macetic acid solution and a 2.29MKOHsolution. If you have 880mL of the acetic acid solution, how many milliliters of the KOHsolution do you need to add-to- make a buffer of pH95.24? The pKa of acetic acid is 4.76.1 T mLmLT 21.-1f-a-buffer solution-is-0.450.M-in-a-weak-acid-(Ka=7.3x10^-6)-and-0.110-M-in-its-conjugated base. what-is-the-ph Ph=1 13.A monoprotic weak acid, HAHA, dissociates in water according to the reactionſ HA(aq)---H-(aq)+A-(aq)HA(aq)---H+(aq)+A-(aq) The equilibrium concentrations of the reactants and products are [HAl=0.290M[ [H-]=2.00X10-4M. and...
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...
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
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