a)If the acetate to acetic acid ratio of a solution is five, what is its pH? The pKa of acetic acid is 4.75.
b)What is the dominant ionic form of phosphoric acid in a solution at pH 8.2?
pH of Buffer solution is calculated by using Henderson's equation as
pH = pKa + log [ salt] / [ Acid]
pH = pKa + log [Acetate] / [Acetic acid]
pH = 4.75 + log 5
pH = 4.75 + 0.6990
pH = 5.45
ANSWER : pH = 5.45
Consider dissociation of Phosphoric acid in water.
H3PO4 (aq) + H2O (l) H3O + (aq) + H2PO4- (aq)
For above reaction, K1 = [H3O +] [H2PO4-] / [H3PO4 ]
We have, pK1 = - log K1 = 2.148
H2PO4- (aq) + H2O (l) H3O + (aq) + HPO42- (aq)
For above reaction, K2 = [H3O +] [HPO42-] / [H2PO4- ]
We have, pK2 = - log K 2 = 7.198
HPO42- (aq) + H2O (l) H3O + (aq) + PO43- (aq)
For above reaction, K2 = [H3O +] [PO43-] / [HPO42-]
We have, pK3 = - log K 3 = 12.375
We know that, 1) if pH < pKa then acidic form predominates and if pH > pKa basic form predominates.
pH of solution is 8.2 . It is in between pKa values 7.198 and 12.375. Hence, predominant form of phosphoric acid is HPO42-.
a)If the acetate to acetic acid ratio of a solution is five, what is its pH?...
What is the ratio of the concentrations of acetate ion and undissociated acetic acid at pH 4.10? (The pKa of acetic acid is 4.76.)
Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic acid is 4.75. How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 4.90 ? ___mL?
Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic acid is 4.75. 1st attempt FeedbackSee HintSee Periodic Table How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 5.05 ?
What is the ratio of undissociated form of acetic acid to acetate at a pH of 5.4? The KA of acetic acid is 10-4.7. Determine a.
A) Calculate the pH of an acetic acid solution. The concentration of acetic acid is 1.0696M and the pKa of acetic acid = 4.75. B) Calculate the pH of a sodium acetate solution of concentration 1.0401M. C) Calculate the pH of a solution made of 100 mL each of the two above solutions (200 mL total) D) Calculate the pH of a solution made of 40 mL of the solution in part C + 160 mL water (200 mL total)...
what is the ph of a solution prepared by dissolving 0.50 mol of acetic acid and 0.2 mol of sodium acetate in water and adjusting the volume of 0.5L if the pka for acetic acid is 4.75. of 0.010 mol of sodium hydroxide is added to the buffer solution from part (a), determine the ph of the new solution
A buffer is prepared containing 3.00 molar acetic acid and 1.00 molar sodium acetate. What is its pH? The pKa of aetic acid = 4.75
Suppose you want to make an acetic acid/acetate buffer to a pH of 5.00 using 10.0 mL of 1.00 M acetic acid solution. How many milliliters of 1.00 M sodium acetate solution would you need to add? The pKa for acetate buffer is 4.75.
You are making a pH 5.0 buffer with acetic acid (pKa = 4.75) and sodium acetate. You want the total concentration of acetate ([acetic acid] + [sodium acetate] ), to be 0.50 M. What concentrations of acetic acid and sodium acetate do you use to make your buffer? acetic acid sodium acetate
2- What is the pH for a 0.0140 M solution of sodium acetate (NaAc). The pKa value for acetic acid is 4.75. ANS: ...