Glutamine (HQ) is a diprotic amino acid with Kal = 6.5 x 10-3 and K2 = 1.00 x 10–9. Determine the pH of each of the solutions. A 0.199 M glutamine hydrochloride (H,Q*cIF) solution. pH = 1.44 Incorrect A 0.199 M glutamine (HQ) solution. pH = 4.85 Incorrect A 0.199 M sodium glutaminate (Na*Q¯) solution. PH
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- One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9please explain the process and answer Mouthwash acts to clean and disinfect mouths. Two important considerations when designing a mouthwash solution are the pH, which should ideally not be too acidic (where saliva has a normal pH range of 6.2–7.6 and below pH 5.5 erosion may occur), and the resistance of the solution to changes in pH. One example of a buffering system used in mouthwash is based on the compound H3PO4 which has PKa values of 2.1, 7.2 and 12.3. i. Hand-draw the structure of the main phosphorus species at pH 7.0, as well as a balanced equilibrium equation showing the structures of the two main phosphoric acid species at pH 7.0.Calculate the pH of a .5M solution of the amino acid, aspargine, that was prepared from the form of asparganine that has a net -1 charge. Ka(-COOH) = 6.92x10^-3 and Ka(-NH3+)=1.86x10^-9 A. 4.52 B. 1.23 C. 5.45 D. 11.22 E. 7.93 F. 10.42
- Calculate the pH, pOH, and fraction of solute protonated or deprotonated in the following aqueous solutions: (a) 0.150 M CH3CH(OH)COOH(aq) (lactic acid), (b) 2.4 x 10-4 M CH3CH(OH)COOH(aq), (c) 0.25 M C6H5SO3H(aq) (benzenesulfonic acid). The appropriate values for pKa or pKb are given inthe table.Consider an aqueous solution containing H+, OH−, Ca2+, “H2CO3” [actually mostly CO2(aq)], HCO3−, CO32−, Ca(HCO3)+, Ca(OH)+, K+, and ClO4−. a)Write the charge balance equation for this solution. b)Which species comes from acid hydrolysis of Ca2+? Write the balanced acid hydrolysis reaction (with physical states) for Ca2+ and calculate Ka c) Which species must be an ion pair? Write the balanced ion pairing reaction, including physical states. Does ion-pair formation increase or decrease the ionic strength? By how much would μ change if 0.0010 M of this ion pair forms?Write down the structure of the amino acid tyrosine and explain whether you can use tyrosine as a physiological buffer at pH 6.7
- 09. Two samples of the same soil is subjected to pH analysis using a pH meter, the first is analysed using 1:1 soil:water ratio and the other with 1:1 soil:KCl ratio, what would be the most probable result? A. Soil analused using 1:1 soil:KCl ratio will register a higher pH compared to that of soil analysed using 1:1 soil water ratio B. Soil analysed using 1:1 soil:KCl will register a lower pH compared to that of soil analysed using 1:1 soil:water ratio C. Soil analysed using 1:1 soil:water ratio will register a lower pH compared to that of soil analysed using 1:1 soil:KCl ratio D. Soil analysed using 1:1 soil:water ratio will have the same pH with that of soil analysed using 1:1 soil:KCl ratioCalculate the pH of a 2.5 M KOH solution at 25 ⁰C. 0.398 -0.398 4.0 x 10⁻¹⁵ 14.4What is the cation exchange capacity (in meq/100 g) and base saturation (in %) of a 150 g soil sample that contains the following amounts of exchangeable cations: 240 mg Ca2+, 69 mg Na+, 234 mg K+, 192 mg Mg2+, 54 mg Al3+, and 10 mg H+. Use the following molar weights: Ca2+ = 40 g/mol; Na+ = 23 g/mol; K+ = 39 g/mol; Mg2+ = 24 g/mol; Al3+ = 27 g/mol and H+ is 1 g/mol.
- You are given 0.5 M solution of the amino acid Arginine. pK1 (α-carboxyl group) = 2.17 pK2 (α- amino group) = 9.03 and pK3 (guanidine group) = 12.48 Answer the following questions. a. Determine the pH of the solution if you add 15 mL 0.25 M HCl to 10 mL of the 0.5 M Arginine. Assume that Arginine is in isotonic state. Show all calculations. Draw the structure of the amino acid at the pH determined in question 1a.Properties of a Buffer The amino acid glycine is often used as the main ingredient of a buffer in biochemical experiments. The amino group of glycine, which has a of 9.6, can exist either in the protonated form or as the free base , because of the reversible equilibrium In what pH range can glycine be used as an effective buffer due to its amino group? In a 0.1 m solution of glycine at pH 9.0, what fraction of glycine has its amino group in the form? How much 5 m KOH must be added to 1.0 L of 0.1 m glycine at pH 9.0 to bring its pH to exactly 10.0? When 99% of the glycine is in its form, what is the numerical relation between the pH of the solution and the of the amino group? Please answer all of these questions, especially C please write in detail.Both functional groups of salicylic acid ionize in water, with Ka = 1.0 × 10^-3 for -CO2H group and 4.2 × 10^-13 for the -OH group. Use these values to calculate the pH of a saturated solution of the acid (solubility = 1.8 g/L).