A 1.32 x 10−3 M solution of quinine, a drug used in treating malaria, has a pH of 9.58. What is the value of Kb?
A 1.32 x 10−3 M solution of quinine, a drug used in treating malaria, has a...
3.) Quinine (C,H,N,0) (Molar Mass = 324.42 g/mol) is an anti-malaria drug. An aqueous solution was mixed containing 88.8 mg (milligrams) of quinine and 1.5 liters of H.O. (assume a total volume of 1.5 L of the solution) (Density of H,0 = 1.01 g/mL) Given this data calculate the following: (Show ALL Work) a.) Mole Fraction of Quinine in Water: (5 pts) b.) The molality of quinine: (again 1.5 L of solution / solvent) (5 pts) c.) ppm of quinine:...
Quinine has been used as an anti-malarial drug for many years. Its aqueous solution in certain acids has been used as a standard in the determination of fluorescence quantum yield of other fluorophores. The structure of quinine is shown below. Quinine in a 1.664-g antimalarial tablet was dissolved in sufficient 0.10 M HCl to give 500 mL of solution. A 10.00 mL aliquot was then diluted to 100.00 mL with the same acid. The fluorescence intensity for the diluted sample...
Quinine (C20H24N2O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine pKb1 = 5.1 and pKb2 = 9.7 (pKb = −log(Kb)). Only 1.0 g of quinine will dissolve in 1900.0 mL of water. Calculate the pH of saturated aqueous solution of quinine. Consider only the reaction Q + H2O equilibrium reaction arrow QH + + OH − described by pKb1, where Q = quinine.
Quinine (C20H24N2O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine pKb1 = 5.1 and pKb2 = 9.7 (pKb = −log(Kb)). Only 1.0 g of quinine will dissolve in 1900.0 mL of water. Calculate the pH of saturated aqueous solution of quinine. Consider only the reaction Q + H2O equilibrium reaction arrow QH + + OH − described by pKb1, where Q = quinine.
Quinine (C_20H_24N_2O_2) is stronger base than quinoline (C_6H_7N). Which solution has a higher pH, 10^-4 M quinine or 10^-4 M quinoline? Which of these solutions has a higher hydroxide ion concentration? Which of these solutions has a higher hydronium ion concentration?
3. A solution is prepared by treating 50 mL of 0.50 M HF (Ka = 6.6x10 ) with 10 mL of 1.15 M NaOH. Calculate the pH of the solution. 4. If enough NaOH is added to the solution in problem 3 to neutralize the HF, what will the pH be? 5. 42.16 mL of a solution of NaOH are required to neutralize 0.7878 g of potassium hydrogen phthalate (Mwt = 204.23 g/mol). Calculate the molar concentration of NaOH in...
codeine is a drug used in painkillers and is a weak
base with kb 1.6X10-6. calculate the ph of a 2.2X10-3M solution of
codeine. calculate % dissociation of codeine.
Question 1: Codeine (CiaH21 NO:) is a drug used in painkillers and is a weak base with a Kb value 1.6 x 106 1 solution of codeine (3 points) b) Calculate the % dissociation of codeine (2 points).
explain 21,22,23
UTILIT In this solution is a. 2.6 x 10-1° M b. 3.8 x 10 M c. 9.58 d. 4.42 e. none of these 21. How many moles of pure NaOH must be used to prepare 1.0 L of a solution that has pH = 12.26? a. 8.2 x 10-16 mol b. 0.018 mol c. 5.5 x 10-13 mol d. 1.74 mol e. none of these 22. Calculate the pH of a 0.045 M HCl solution. K a. 1.23...
7. (3 points) A 0.613 M HX acidic solution has a pH of 2.07. a. Find the percent ionization of the acid in this solution. b. Calculate the Ka value of HX. 8. (3 points) Calculate the pH of a 0.76 M solution of CH3NH2, Kb = 4.4 x 10".
Calculate the pH of a 0.445 M NH, solution. NH, has a Kb = 1.8 x 10-5. pH = The K, of a weak monoprotic acid is 1.59 x 10-5. What is the pH of a 0.0808 M solution of this acid? pH =