Homework Answers
The conjugate base is the one which is obtained after acid loses its one proton. When base accepts one proton then that compound will be known as conjugate acid.
Thus CH3COOH is a weak acid which upon a loss of one proton gives CH3COO- ion. This ion will be called now as conjugate base of acetic acid.
Water is weak base and H2O is conjugate base of H3O+.
Thus correct ans will be option (e).
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The following equilibrium is established in water solution: CH3COOH + H20 = CH3COO +H30+ K a...
The following equilibrium is established in water solution: CH3COOH + H20 = CH3C00+H307 Ka=1.8 x 10-5...
The following equilibrium is established in water solution: CH3COOH + H20 = CH3C00+H307 Ka=1.8 x 10-5 Which of the following is false? a CH3COO is the conjugate acid of CH3COOH. b. Hydroxide concentration is negligible with respect to hydrogen ion concentration. OO H2O is a weak base. Od. H2O is the conjugate base of H307 De CH3COOH is a weak acid.
The following equation represents the dissociation of propionic acid in water. HC3H502(aq) + H20(1) = H30+(aq)...
The following equation represents the dissociation of propionic acid in water. HC3H502(aq) + H20(1) = H30+(aq) + C3H502 (aq) The value for the acid-dissociation constant for propionic acid (HC3H502) is 1.3x10-5 at 25°C. Calculate the hydronium ion concentration present in a propionic acid solution that has the following equilibrium concentrations. 3.24x10-2 mol/L HC3H502 3.06x10-4 mol/L for propionic acid's conjugate base, C3H5027 The general form of the acid-dissociation constant is Ka = [H30'A ], where Ka is the acid-dissociation constant, [HA]...
4. Calculate [H30*], [OH-], pH and pOH of a 0.5 M CH3COOH solution, K. = 1.8...
4. Calculate [H30*], [OH-], pH and pOH of a 0.5 M CH3COOH solution, K. = 1.8 x 10-5. 5. Write the acid ionization equations in water of the weak acid H PO4, and the expressions of K.
If the hydroxide concentration of a CH3COOH/CH3COO- buffer system is 0.000045 M, what is the acetate...
If the hydroxide concentration of a CH3COOH/CH3COO- buffer system is 0.000045 M, what is the acetate concentration if the acetic acid concentration is 0.74 and the dissociation constant, Ka, of CH3COOH is 6 x 10-9 ? A hot piece of metal at 450K is placed in pure water that has a volume of 55.0 mL which has an initial temperature of 25.3°C. After five minutes, equilibrium is established and a final temperature of 44.4°C is reached . What is the...
Need Help on 1-6 please 1. Mercury ions exit as the mercurous dimer Hg22+ and Hgt....
Need Help on 1-6 please
1. Mercury ions exit as the mercurous dimer Hg22+ and Hgt. If Hg22+ is in contact with liquid mercury, Hg (1), the following equilibrium is established: Hgt(aq) → Hg22+(aq) + Hg(1) K= 2.24x10-5 If a 0.15 M solution of Hgt is put in contact with liquid mercury, what will be the resulting equilibrium concentration of Hg22+? Show work a. 3.36 x 10-6 M b. 1.83 x 10-3 M c. 1.14 x 10-2 M d. 0.83...
Equilibrium constants for four weak acids are given below. • carolinic acid: 6.2 x 105 •...
Equilibrium constants for four weak acids are given below. • carolinic acid: 6.2 x 105 • isabellic acid: 4.9 x 107 • jackic acid: 3.1 x 103 • pennic acid: 7.2 x 10-9 Weak acids (referred to as HA below) react with water per the reaction below to form their conjugate base (A™) and hydronium ion (H30"); HA (aq) + H20 (liquid) = A (aq) +H30* (aq) Each acid is reacted with water and allowed to reach equilibrium. When the...
Determine the [CH3COO") of the following aqueous solution. Initial concentrations are given. [CH3COOH] = 0.250 M,...
Determine the [CH3COO") of the following aqueous solution. Initial concentrations are given. [CH3COOH] = 0.250 M, [HI] = 0.120 M Ka (acetic acid)= 1.8 x 10-5 O 1.88 10-5m O 0.37 M 0 3.8 × 10-5m 0 8,6x10-6M 0.25 M
please help l, will rate! thabk you!! Why does a solution of a weak acid and...
please help l, will rate! thabk you!!
Why does a solution of a weak acid and its conjugate base act as a better buffer than does a solution of the weak acid alone? The presence of both the acid and the base provides a significant concentration of both an acid and a base, making it harder to change the pH A solution of a weak acid alone has no base present to absorb added acid. The presence of both the...
A 1.00 liter solution contains 0.35M acetic acid and 0.26 M potassium acetate. If 35.0 mL...
A 1.00 liter solution contains 0.35M acetic acid and 0.26 M potassium acetate. If 35.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water) A. The concentration of CH3COOH will decrease. True False B. The concentration of CH3COO" will remain the same C. The equilibrium concentration of H30* will increase D. The pH will increase E. The ratio of [CH3COOH]/ [CH3coo]...
please help >< Polyprotic acids have more than one proton to donate to water, therefore have...
please help ><
Polyprotic acids have more than one proton to donate to water, therefore have more than one equilibrium constant for proton donation. For phosphoric acid, there is a three-step equilibrium: H, PO +H,0 5 H2PO4 + H30* H,PO," +H,0 5 HPO - +H30* HPO 2- +,0 5 PO.- +,0* Kai = 7.11 x 10-3 Ka2 = 6.32 x 10-8 Ka; = 4.5 x 10-13 For all conjugate acid base pairs: K, XKK where K is for the reaction...
The following equilibrium is established in water solution: CH3COOH + H20 = CH3C00+H307 Ka=1.8 x 10-5 Which of the following is false? a CH3COO is the conjugate acid of CH3COOH. b. Hydroxide concentration is negligible with respect to hydrogen ion concentration. OO H2O is a weak base. Od. H2O is the conjugate base of H307 De CH3COOH is a weak acid.
The following equation represents the dissociation of propionic acid in water. HC3H502(aq) + H20(1) = H30+(aq) + C3H502 (aq) The value for the acid-dissociation constant for propionic acid (HC3H502) is 1.3x10-5 at 25°C. Calculate the hydronium ion concentration present in a propionic acid solution that has the following equilibrium concentrations. 3.24x10-2 mol/L HC3H502 3.06x10-4 mol/L for propionic acid's conjugate base, C3H5027 The general form of the acid-dissociation constant is Ka = [H30'A ], where Ka is the acid-dissociation constant, [HA]...
4. Calculate [H30*], [OH-], pH and pOH of a 0.5 M CH3COOH solution, K. = 1.8 x 10-5. 5. Write the acid ionization equations in water of the weak acid H PO4, and the expressions of K.
Need Help on 1-6 please
1. Mercury ions exit as the mercurous dimer Hg22+ and Hgt. If Hg22+ is in contact with liquid mercury, Hg (1), the following equilibrium is established: Hgt(aq) → Hg22+(aq) + Hg(1) K= 2.24x10-5 If a 0.15 M solution of Hgt is put in contact with liquid mercury, what will be the resulting equilibrium concentration of Hg22+? Show work a. 3.36 x 10-6 M b. 1.83 x 10-3 M c. 1.14 x 10-2 M d. 0.83...
Equilibrium constants for four weak acids are given below. • carolinic acid: 6.2 x 105 • isabellic acid: 4.9 x 107 • jackic acid: 3.1 x 103 • pennic acid: 7.2 x 10-9 Weak acids (referred to as HA below) react with water per the reaction below to form their conjugate base (A™) and hydronium ion (H30"); HA (aq) + H20 (liquid) = A (aq) +H30* (aq) Each acid is reacted with water and allowed to reach equilibrium. When the...
Determine the [CH3COO") of the following aqueous solution. Initial concentrations are given. [CH3COOH] = 0.250 M, [HI] = 0.120 M Ka (acetic acid)= 1.8 x 10-5 O 1.88 10-5m O 0.37 M 0 3.8 × 10-5m 0 8,6x10-6M 0.25 M
please help l, will rate! thabk you!!
Why does a solution of a weak acid and its conjugate base act as a better buffer than does a solution of the weak acid alone? The presence of both the acid and the base provides a significant concentration of both an acid and a base, making it harder to change the pH A solution of a weak acid alone has no base present to absorb added acid. The presence of both the...
A 1.00 liter solution contains 0.35M acetic acid and 0.26 M potassium acetate. If 35.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water) A. The concentration of CH3COOH will decrease. True False B. The concentration of CH3COO" will remain the same C. The equilibrium concentration of H30* will increase D. The pH will increase E. The ratio of [CH3COOH]/ [CH3coo]...
please help ><
Polyprotic acids have more than one proton to donate to water, therefore have more than one equilibrium constant for proton donation. For phosphoric acid, there is a three-step equilibrium: H, PO +H,0 5 H2PO4 + H30* H,PO," +H,0 5 HPO - +H30* HPO 2- +,0 5 PO.- +,0* Kai = 7.11 x 10-3 Ka2 = 6.32 x 10-8 Ka; = 4.5 x 10-13 For all conjugate acid base pairs: K, XKK where K is for the reaction...
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