Q1 was not answered. My question was why when HCl is added why is…
Q1 was not answered. My question was why when HCl is added why is…
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12:26 . . . Cut allll 33% imaginationb7 Active more than 1 day ago . [CH;COOH] = 0.1 – X .
[CH;COO-] = x + 0.1 . [H+] = x (some used to react with acetate) Addition of HCI
(0.005M): . HCI reacts with acetate ions to form acetic acid. . The concentra…
[CH;COO-] = x + 0.1 . [H+] = x (some used to react with acetate) Addition of HCI
(0.005M): . HCI reacts with acetate ions to form acetic acid. . The concentra…
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12:26 . . . Cut allll 33% imaginationb7 Active more than 1 day ago . [H+ ] = X Addition of
Sodium Acetate (NaCH,COO): . 0.1M of sodium acetate (NaCH,COO) is added. . The
acetate ions (CH,COO-) from sodium acetate react with the protons (H+) fro…
Sodium Acetate (NaCH,COO): . 0.1M of sodium acetate (NaCH,COO) is added. . The
acetate ions (CH,COO-) from sodium acetate react with the protons (H+) fro…
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12:26 okok f . . . Cut alll 33% imaginationb7 Active more than 1 day ago Explanation: Initial
Conditions: . 0.1M acetic acid (CH, COOH) . 0.1M sodium acetate (NaCH,COO) . 0.005M
HCI Reaction of Acetic Acid (CH, COOH): . Acetic acid partially dissociates: …
Conditions: . 0.1M acetic acid (CH, COOH) . 0.1M sodium acetate (NaCH,COO) . 0.005M
HCI Reaction of Acetic Acid (CH, COOH): . Acetic acid partially dissociates: …
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(K = 1.75 x 107), i soluble and will dissociate completely to shift the acid dissociation to the
left, so the equilibrium ecules and acetate ions will be essentially equal to their initial
concentrations, 0.1 / CH, COOH + HO HO+ + CH, COO Na Cl 100 – Nat tong …
left, so the equilibrium ecules and acetate ions will be essentially equal to their initial
concentrations, 0.1 / CH, COOH + HO HO+ + CH, COO Na Cl 100 – Nat tong …
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MCAT GENERAL CHEMISTRY REVIEW 11.8 BUFFER SOLUTIONS A buffer is a solution
that resists changing pH when a small amount of acid or base is added. The buffer ing
capacity comes from the presence of a weak acid and its conjugate base (o…
that resists changing pH when a small amount of acid or base is added. The buffer ing
capacity comes from the presence of a weak acid and its conjugate base (o…
Q1 was not answered. My question was why when HCl is added why is the equilibrium for the equation CH3COOH > CH3COO- + H+
not
0.1-x 0.1+x 0.005+x
And what would it be with the value of x?
What would be the ice table when HCl is added?
Answer & Explanation
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