A carboxylic acid (ka=1.8*10-5) was extracted from an aqueous solution ir the presence of ether, and the acidity function of the solution = 4, so if you know that the distribution ratio for %3D this system is 9, find the value of the distribution coefficient (KD) for this system
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- Calculate the pH of two HCl solution based on their concentrations of 0.001 and0.0001 M. Then calculate the pH of a solution when you add each of these to a closed carbonicacid system with mcarb-t = mH2CO3 + mHCO3- + mCO32- = 0.01 m and pH = 6. At that pH, mH2CO3 =10-2.16; mHCO3- =10-2.51; mCO32- is negligible.(4c-201) Copy the following equation, and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its conjugate acid. HNO3 + H2O → H30* + NO3¬ For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph Arial 14px A v ... In X2 田由田図 EX: ABC Ť {;} > >Where Kal = 4.20 x 10-7 Ka24.69 × 10-¹1 X (a) Calculate the fraction H₂CO3, HCO3, CO3², use the following table as your template. (b) Plot_p¹ vs. fraction of H₂CO3, HCO3, CO3² using the plotting guidelines all on same chart. pH [H] “H_co, ан,со, анс, а со α α 1.806 2.020 2.235 2.449 2.664 2.878 3.093 3.307 3.522 3.736 3.951 4.165 4.380 4.594 4.809 5.023 5.238 5.452 5.667 5.881 6.096 6.310 6.525 6.739 6.954 7.168 7.383 7.598 7.812 8.027 8.241 8.456 8.670 8.885 9.099 9.314 9.528 9.743 9.957 10.172 10.386 10.601 10.815 11.030 11.244 11.459 11.673 11.888 12.102 12.317 12.531
- Complete the Ka2 expression for H₂CO3 in an aqueous solution. K₁2 = 4.69 x 10-11 = [HCO3] [CO] Answer Bank [H₂0†] [H₂CO3] [H₂O+1²Analysis of an amine using a back-titration Kjeldahl method resulted in the following equation for P, the percent nitrogen in the amine: P = (mmols acid) – (mL base) (molarity base) (14.01) (100) (mg sample) = (4.75 ± 0.03 )- (0.1198) ± 0.0008) (15.00 ± 0.04) (14.01 ) (100) 750.0 ± 0.3 where the uncertainties are all standard deviations for infinite -sized samples. How will you report the value for P?665 mL of 0.875 M aqueous aniline solution CC 2H5 NH2) are boiled gently to reduce the volume to 401 m L. The solution was then left to disociate , and the Kb of this Solution was found to be 3.9X10-10.Estimate the pi of aniline at eguilibrium Identify the conjugated acid-base pair according to Bronste d - Lowry Theory of the dissoci ati on reaction of aniline (CH5 NH2). Calculate the ka value Of the reaction
- What is the pH of an acidic mixture containing 0.062 M hydrazoic acid (Ka = 1.9 * 10-5) and 0.062 M hypobromous acid (Ka = 2.0 * 10-9)?Q3/ A 0.80868 gm sample of a commercial phosphate detergent was ignited at a red heat to destroy the organic matter the residue was then taken up in hot HCl, which converted the P to H3PO4. The phosphate was precipitated as MgNH₂PO4.6H₂O by addition of Mg¹2 followed by aqueous NH3 after being filtered and washed. The precipitate was converted to Mg₂P₂O(222.57gm mol) by ignition at 1000 C this residue weighed represent 61.5% of the total sample mass. Calculate the percent P(30.974gm mol),O (16 gm/mol) and Mg (24.3 gm/mol) in the sample.5. A series of solutions containing NaOH, Na2CO3, and NaHCO3, alone or in compatible combination, was titrated with 0.1202 M HCI. Tabulated below are the volumes of acid needed to titrate 25.00-mL portions of each solution to (1) a phenolphthalein and (2) a bromocresol green end point, separately. Use this information to deduce the composition of the solutions. In addition, calculate the molar concentration of each solute. mL | (1) Vph |(2) Vbcg а. 22.42 22.44 b. 15.67 42.13 с. 29.64 3.42 d. 16.12 32.23 е. 0.000 32.33
- Water sample from different river water was subjected to a qualitative alkaline analysis by titrating against 0.1250 MHC1 and using phenolphthalein and bromocresol green end point. The table below shows the volumes of acid needed to titrate 25.00-mL portions of each sample and their corresponding end point, separately. Use this information to deduce the composition of the solutions. Calculate the molar concentration of each solute. Volume (mL) Phenolphthalein end Bromocresol green Solute identity concentration end point Volume (mL) Molar Sample point 22.40 of solute/s 1 22.41 2 0.00 33.40 3 15.67 42.13 4 29.64 36.42The following results were collected for % sodium carbonate in asample: 4.2, 4.4, 4.9, 4.0, 6.4, 4.3 and 4.1%. The result 29.4% seemsquestionable, if the tabulated Q = 0.568, should it be retained orrejected?Select one or more:The value 6.4 should be omitted (rejected)The calculated Q = 0.625The value 6.4 should be retainedthe calculated Q = 1.69-10. (a) Find the pH of a solution prepared by dissolving 1.00 g of glycine amide hydrochloride plus 1.00 g of glycine amide in 0.100 L. + Cl- H3N H2N. NH2 NH2 Glycine amide hydrochloride (BH†) FM 110.54, pK, = 8.20 Glycine amide (B) FM 74.08 (b) How many grams of glycine amide should be added to 1.00 g of glycine amide hydrochloride to give 100 mL of solu- tion with pH 8.00? (c) What would be the pH if the solution in (a) is mixed with 5.00 mL of 0.100 M HC1? (d) What would be the pH if the solution in (c) is mixed with 10.00 mL of 0.100 M NaOH?