A buffer at pH 7.45 is prepared by mixing solutions of KH2PO4 and K2HPO4. Which of the following ratios of [base]/[acid] is required?
For phosphoric acid, Ka1 = 7.5 × 10-3 Ka2 = 6.2 × 10-8 Ka3 = 4.2 × 10-13
[base]/[acid] = 1.75
[base]/[acid] = 1.24
[base]/[acid] = 0.57
[base]/[acid] = 1.27
[base]/[acid] = 0.79
A buffer at pH 7.45 is prepared by mixing solutions of KH2PO4 and K2HPO4. Which of...
A microbiologist is preparing a medium on which to culture E. coli bacteria. She buffers the medium at pH 7.00 to minimize the effect of acid-producing fermentation. What volumes of equimolar aqueous solutions of K2HPO4 and KH2PO4 must she combine to make 750.0 mL of the pH 7.00 buffer? Ka values for phosphoric acid: Ka1 = 7.2 ×10−3 Ka2 = 6.3 ×10−8 Ka3 = 4.2 × 10−13 Volume H2PO4− = ??? mL Volume HPO42− = ??? mL
A buffer is prepared by mixing 50.0mL of 1.0M sodium hydrogen phosphate with 40.0mL of 1.20 M sodium dihydrogen phosphate. (For phosphoric acid, Ka1 = 7.5x10-3, Ka2 = 6.2x10-8, Ka3 = 2.2x10-13) What is the pH of this buffer?
Calculate the ratio of the molar concentrations of HPO42- and H2PO4- ions required to obtain a buffer solution at pH = 7.0. For phosphoric acid, Ka1 = 7.5 × 10-3 Ka2 = 6.2 × 10-8 Ka3 = 4.2 × 10-13
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
1 A) Which of the following pairs of solutions when mixed will form a buffer solution? Group of answer choices H2SO4 and Ca(OH)2 NH3 and NH4Br NaNO3 and HNO3 KOH and KNO2 B)Phosphoric acid, H3PO4, is a triprotic acid with the following Ka values: Ka1 = 7.5 x 10-3; Ka2 = 6.2 x 10-8; Ka3 = 3.6 x 10-13 In a solution of 0.15 M H3PO4, which species will be most abundant? H3O+ H3PO4 HPO42- H2PO4-
Phosphoric acid has the following dissociation constants: Ka1 = 7.5×10-3; Ka2 = 6.2×10-8; and Ka3 =4.8×10-13, how to prepare a buffer solution of pH 7.40?
Phosphoric acid, H3PO4, is a triprotic acid with the following acid dissociation constants: Ka1 = 7.5 × 10-3 Ka2 = 6.2 × 10-8 Ka3 = 4.2 × 10-13 Which of the following combinations would be best for preparing a pH 7 buffer? a. H3PO4 and NaH2PO4 b. H3PO4 and HCl c. Na2HPO4 and Na3PO4 d. NaH2PO4 and Na2HPO4 e. H3PO4 and Na3PO4
Q: What is the pH of a solution containing 0.125 M KH2PO4 and 0.175 K2HPO4 Ka (H2PO4-) = 6.2 x 10-8 Ka (HPO42-) = 4.8 x 10-13 Q: A 0.15 M solution of a weak acid is 3.0 % dissociated. What is the Ka of this acid? Q: A solution of aspirin was prepared that is 0.16 M. The pH of this solution was measured to be 2.43. What is the Ka of aspirin? Q: A solution of formic acid...
Question 15 0/4 pts The acid ionization constants of phosphoric acid (H3PO4) are Ka1 = 7.5 x 10-3. Ka2 = 6.2 x 10-8 and Ka3 - 4.2 x 10-13 at 25.0°C. What is the molar concentration of phosphate ion in a 2.5 M aqueous solution of phosphoric acid?
A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3] = 1.000 M. Determine how much strong acid 1.00M HCI or strong base 1.000 M NaOH must be added to change the pH to 7.40. The step-wise acid dissociation constants for carbonic acid are Ka1= 4.2*10^-7 ; Ka2= 4.8*10^-11.