If the intrinsic solubility of an acidic drug is 20 mM and its pKa is 6, what is the lowest/highest pH at which 2 M of the drug can stay in the solution?

Calculate the sodium acetate/acetic acid ratio to prepare a buffered solution with a pH of 5.06. (pKa = 4.76)

Which of the following would NOT appear in the net ionic equation for the addition of a strong base to a HNO2 and NO2- buffer? O H+ O OH- Ο ΗΝΟ, O H2O O NO2

What volume, in milliliters, of 0.180 M NaOH should be added to a 0.140 L solution of 0.029 M glycine hydrochloride (p Kal = 2.350, pK₁2 = 9.778) to adjust the pH to 2.50? NaOH volume = mL

Which weak acid would be best to use when preparing a buffer solution with a pH of 9.80? an acid with K₂ = 2.5 x 10-5 a an acid with K₂ = 2.0 x 10-6 a an acid with K₂ = 1.0 × 10-¹1 an acid with K₁ = 1.7 x 10-10 a an acid with Ka = 2.5 × 10-8 an acid with K₂ = 3.2 x 10-7 a

Which of the following buffer would work best for making a buffer at pH 7.5? O TAPS, K₂ = 4.0 x10⁹ O HEPES, K₂= 3.2 x10-8 O Acetic acid, K₂ = 1.6x10-5 O CAPS, K₂ = 4.0 x10-¹¹ O PIPES, K₂ = 1.6 x10-7

The pKa of lactic acid is 3.86. What is the pH of a buffer in which the lactic acid concentration is 0.200 M and the sodium lactate concentration is 2.00 M?

A compound has an ionisable groups with a pKa of 2.6. A 200 mL volume of a 0.15 M solution of this compound had an initial pH 2.4. The concentration of the conjugate acid in the initial buffer was 0.092 M. The concentration of the conjugate base in the initial buffer was 0.058 M. What is the final pH of the buffer AFTER you added 5 mL of 1 M NaOH?

PLease help me asap and make sure your answer is correct and rounded only at the final answer !

A 10.00 mL sample of 1.20 M HNO2 (analyte) (pK, = 3.34 and K = 4.57x104) is titrated with 1.20 M NaOH (titrant), what is the pH when 5.00 mL of NaOH are added to the analyte? Question 4 A 10.00 mL sample of 1.20 M HNO2 (analyte) (pK, = 3.34 and K, -4.57x104) is titrated with 1.20 M NaOH (titrant), what is the pH when 10.00 mL of NaOH are added to the analyte? Assume Ku = 1.0 x 10-14 Using the titration curve below for the titration of 10.00 mL of the analyte NH3 with HCl(aq) (titrant) to estimate pKa for NH3 Titration of 10.00 mL Ammonia (ag) with Hydrochloric Acid (ag) 12.0 11.0 10.0 9.0 8.0 7.0 5.0 4.0 3.0 2.0 1.0 0.0 0.0 2.0 4.0 10.0 12.0 140 16.0 180 20.0 6.0 Volume of HCI Added (mL) 8.0