Using the reagents, prepare 100mL solution with a concentration of 25.0 mM Tris buffer at a final pH of 7.70. •Solid Tris, FW = 121.1 • Solid Tris-C1, the conjugate acid of Tris. It has a pKa of 8.30 (at 25° C) and a FW of 157.6. •deionized water
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Using the reagents, prepare 100mL solution with a concentration of 25.0 mM Tris buffer at a final pH of 7.70.
•Solid Tris, FW = 121.1
• Solid Tris-C1, the conjugate acid of Tris. It has a pKa of 8.30 (at 25° C) and a FW of 157.6.
•deionized water
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- What will be the appropriate pH of a buffer prepared by mixing 100 ml of 0.1 M Na2HPO4 and 100 ml of 0.1 M NaH2PO4? (For H3PO4, pKa1 = 2.1; pKa2 = 6.8; pKa3 = 12.5) Ans in 2 significant figuresWhat will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?1.00 L of an aqueous solution containing 0.1026M of compound B and 0.0296M of its conjugate acid HB* was prepared to form a buffer solution with a pH of 8.61 (pKą 8.072). Upon addition of a 12.0mL of 1.00M HCI to the solution, the pH changed from 8.61 to 8.41. Had there been no buffer, the addition of the same amount and concentration of HCl would have lowered the pH to 1.93. Select ALL statements from the choices that are true. (Make sure to check all applicable answers to get a full points.) The added HC will be consumed by B and result to the formation of BH+. This will then cause the slight decrease in pH as predicted by the Henderson-Hasselbalch equation. Based on the Henderson-Hasselbalch equation, the HCl will increase the H+ concentration, thereby increasing the pH by itself because pH = - log [H+]. The added HCI will not factor in the calculations for the pH, as the Henderson-Hasselbalch equation only accounts for the concentrations of B and BH+. Check this only if NONE of the…
- Salts containing the phosphate ion are added to municipalwater supplies to prevent the corrosion of lead pipes. (a) Basedon the pKa values for phosphoric acid (pKa1 = 7.5 x 10 - 3,pKa2 = 6.2 x 10 - 8, pKa3 = 4.2 x 10 - 13) what is the Kbvalue for the PO43 - ion? (b) What is the pH of a 1 x 10 -3 M solution of Na3PO4 (you can ignore the formation ofH2PO4- and H3PO4)?Commercial phosphate buffers are sold to maintain fish tanks at a pH of 7. Use a table of acid dissociation equilbrium constants to find all the K, values for H, PO,. AjA BIUS Calculate the pka values from the Ka values. Remember that pX = -logX. pKi = pK = pk3 = What two chemical species are primarily found in solution in a phosphate buffer with a pH of 7? о Н РО, аnd PО H,PO, and HPo HPO; and PO- о Н РО, and H,РО,A solution contains both NaHCO3 and Na2CO3. Titration of a 50.00 mL portion to a phenolphthalein end point requires 21.25 mL of 0.1385 M HCl. A second 50.00 mL aliquot requires 45.48 mL of the HCl solution when titrated to a bromocresol green end point. Calculate the molar concentration of Na2CO3 in the original solution. (Do not include the unit for molarity. Enter your answer to three significant figures.)
- Calculate the pH of a buffer in which [HC4H7O2] = 0.36 M and [C4H7O2 –] = 0.31 M. How do you calculate pKa acid dissociation constant？？A buffer was created using ascorbic acid and sodium ascorbate. What is the pH of the buffered solution if at equilibrium [H₂C6H6O6] = 5.5 X 10-5 M, [HC6HO6¹¹] = 3.5 X 104 M, and K₂ = 8.00 x 10-5 ? everything is based upon the acid dissolving in water: H₂C6H6O6 + H₂O HC6H6O6¹¹ + H3O+1 [ |][ Ka = [ solve for [H3O+¹] then put in the numbers Ka [ [H3O+¹] = [ [H3O+¹] = pH = -log a. H30+1 b. OH-1 h. HCzH3O2 i. C₂H3O₂-¹ = c. H₂C6H6O6 q. 3 r. 0.5000 s. 5.5 X 10-5 x. 5.5 x 10-² dd. 0.7100 ] y. 0.7000 z. 1.60 x 10-5 ee. 1.26 x 10-5 ff. 4.901 ( d. HC6H606¹¹ j. H₂S k. HS-1 t. 3.5 X 10-4 -1 e. HSO3¹¹ 1. S-² X( m. HX f. SO3² n. X-1 g. H₂SO3 o. 1 p. 2 W. 1.11 x 10-8 u. 8.00 x 10-5 v. 1.75 x 10-6 aa. 1.143 x 105 bb. 0.4900 cc. 1.104 x 10-5 gg. 7.93 hh. 4.942 ii. 4.957How many grams of dipotassium succinate trihydrate (K2C4H4O4-3H,O, MW = 248.32 g/mol) must be added to 610.0 mL of a 0.0587 M succinic acid solution to produce a pH of 5.835? Succinic acid has pKa values of 4.207 (pKal) and 5.636 (pK42). mass: g
- A weak acid solution with concentration 0.020 M has a pH of 3.7, what is the pKa of this acid?The following is list of weak acids and their pką values weak acid pKa benzoic acid 4.20 hydrogen citrate 6.40 hydrocyanic acid 9.31 hydrogen phosphate 12.38 Which would be the best buffer to use at pH 7 ? For benzoic acid, a 50:50 mixture of benzoic acid and its conjugate base, the benzoate ion, would have pH = The buffering capacity of a benzoic acid:benzoate buffer would be at pH = 7 A. 4.20 B. 6.40 C. 9.31 D. 12.38 E. benzoic acid F. hydrogen citrate G. hydrocyanic acid H. hydrogen phosphate I. good J. bad3. Calculate the pKa value of hydroxylammonium cation (HO-H3N*)(protonated on nitrogen hydroxyl amine) if it is known that dissolving the hydroxyl amine H2N-OH in a buffered aqueous solution with pH = 6.0 results in 50 molar % of hydroxylammonium cation in the solution. %3D (i) Write the dissociation equation of hydroxylammonium cation and (ii) show your calculations in details.