Ibuprofen is a weak acid with a solubility in water of 21 mg/L and a pKa of 4.91. What is the pH of a saturated solution of ibuprofen in water? The chemical formula of ibuprofen is C13H18O2.
Ibuprofen is a weak acid with a solubility in water of 21 mg/L and a pKa...
help! thank you! Ibuprofen, a non-steroidal anti- inflammatory drug, is a weak acid with pKa of 5.2. The structure of ibuprofen is shown below. 2. bosiccare. Compare tor ibuprofen ablets 200 mg Reducer NAD) 500 COATED TABLETS a. What is the pH when 150 mL of 0.4 M NaOH is added to 150 mL of 1.5 M ibuprofen solution? b. What is the pH when 150 mL of 1.5M ibuprofen solution is added to 5L of water?
Phenobarbital is a weak acid. Its intrinsic solubility is 1g /L. Its pKa is 7.4 and Mol Wt : 232.32 Calculate the pH of the buffer required to prepare a clear homogeneous solution.of phenobarbital 1 g/100 mL.
PART A. Determine the pH of a 9.553 mM weak acid solution that has a pKa of 8.83 PART B. Calculate the pH of a 319 mM weak base solution with a pKb of 9.04. PART C. Determine the pKa of a weak acid solution that has an initial concentration of 0.334 M and a pH of 4.54. Hint: You know the pH of the solution, so you can easily determine x in your ICE table PART D. Calculate the...
In a solution of the weak acid DNP (pKa 4.11) in water, [H3O+] = 9.4 x 10^-4 M and DNX, the conjugate base, has a concentration of 0.00180 M. A.) What is the concentration of DNP in the above solution? B.) What is the pH of the solution?
A 0.27 −mol sample of a weak acid with an unknown pKa was combined with 12.0 mL of 2.80 M KOH and the resulting solution was diluted to 1.500 L. The measured pH of the solution was 3.85. What is the pKa of the weak acid? Express your answer using two decimal places.
Calculate and compare the molar solubility of Mg(OH)2 in water and in a solution buffered at a pH of 4.5. Part 1: (a) Determine the molar solubility of Mg(OH)2 in water and the pH of a saturated Mg(OH)2 solution. molar solubility =1.39 × 10^-4 M pH = 10.45 Part 2 out of 3 (b) Determine the molar solubility of Mg(OH)2 in a solution buffered at a pH of 4.5. molar solubility =_____× 10_____M
4. (15) A saturated solution of phenol, C6H5OH, a very weak acid with pKa=10.00, has pH=4.90. What is the molarity of phenol in this solution?
You dissolve 25.19 mg of arsenious acid (H3ArO3 , F.W. = 125.94) in 1.00 L of water. Arsenious acid is weak, with Ka = 5.1 × 10−10. Calculate the equilibrium concentrations of H3AsO3 and H2AsO – 3 and the pH of the solution. Assume that the activity coefficients are all 1, but you must include the autoprotolysis of water.
The pka of a weak acid is useful for identification of an unknown acid because it is a constant (as long as temperature remains the same). When a weak acid is titrated with a strong base, the pka of the weak acid equals the pH at the half-equivalence point. A 0.3210 g sample of weak monoprotic acid is delivered into laboratory glassware. It will be used for titratation against 0.1254 M NaOH. If the molar mass of the weak acid...
In a weak acid when [HA]=[A-]the pH = the pKa. What is the pH after adding 0.50 moles HCl to a solution of HA =1 mole and A- = 1 mole. The pKa of the weak acid = 4