igand containing four carboxylic acid groups and two amines.Which is TRUE for the acid-base properties of EDTA? EDTA- (60-00-4) - Physical Properties • Chemical Properties • Solubility • Uses/Function • Reactions Thermochemistry I EDTA is a hexaprotic system,H6Y2* when the amines are protonated. II Neutral EDTA,H4Y,is tetraprotic when the amines are not protonated. III Deprotonated EDTA,Y4- IV The fraction of EDTA in any of the six EDTA species is pH dependent. is the most favored form that binds to metal cations. O Only III is TRUE O Only IV is TRUE O Only III, and IV are TRUE 0I, II, III, and IV are all TRUE

igand containing four carboxylic acid groups and two amines.Which is TRUE for the acid-base properties of EDTA? EDTA- (60-00-4) - Physical Properties • Chemical Properties • Solubility • Uses/Function • Reactions Thermochemistry I EDTA is a hexaprotic system,H6Y2* when the amines are protonated. II Neutral EDTA,H4Y,is tetraprotic when the amines are not protonated. III Deprotonated EDTA,Y4- IV The fraction of EDTA in any of the six EDTA species is pH dependent. is the most favored form that binds to metal cations. O Only III is TRUE O Only IV is TRUE O Only III, and IV are TRUE 0I, II, III, and IV are all TRUE

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A student added a total of 75 mL sodium hydroxide to titrate an amino acid solution with 0.5M NaOH. They also calculated that they added a total of 14 mL of sodium hydroxide to arrive at pH 2.6 and a total of 32 mL of sodium hydroxide to arrvive at pH 4.8.What was the initial concentration of the amino acid solution in milimolar (mM)? The calculations must be presented such that those can be recapitulated by the marker. Provide the answer with no decimal places. Show all details of your working out. State the answer in a full sentence.
Calculate the pH of the solution after the addition of each of the given amounts of 0.0603 M HNO3 to a 60.0 mL solution of 0.0750 M aziridine. The p?a of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL HNO3? pH= What is the pH of the solution after the addition of 7.79 mL HNO3? pH= What is the pH of the solution after the addition of a volume of HNO3 equal to half the equivalence point volume?pH= What is the pH of the solution after the addition of 70.5 mL HNO3? pH= What is the pH of the solution after the addition of a volume of HNO3 equal to the equivalence point?pH= What is the pH of the solution after the addition of 77.9 mL HNO3? pH=
At the end of "class", I asked you to consider a triprotic acid with pka's = 2.0, 6.0 and 10.0. What is the equilibrium constant for the reaction H3A + HA²¯ ⇒ 2H₂A? If you need to, assume 25 °C, where Kw = 10-14
Glutamine (HQ) is a diprotic amino acid with K₁1= 6.5 x 10-3 and K₁2 = 1.00 x 10. Determine the pH of each of the solutions. A 0.276 M glutamine hydrochloride (H₂Q*CI) solution. pH = 1.373088781 Incorrect
Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH₂CH₂CO₂H, pKa [HA] pH = = 4.352 || pH = 4.874 Answer Bank [A] + log Using the equation to calculate the quotient [A¯]/[HA] at three different pH values. [A-] [HA] [A-] [HA] - o = pka pH = 4.874).
a)Calculate the ph of 0.565 M solution of ethylamine, and 0.322 M ethylammonium bromide. The base disassociation constant Kb is 6.31 x 10^-4. b)What is the pH if 107 ml of 0.250 M of a strong acid like HCL is added to 100 ml of the buffer solution? c)What if a strong base, like NaOH is added with the same amount instead?
A 0.100 mol L solution of ethylamine (C2H5 NH2) has a pH of 11.87. Calculate the Kp for ethylamine. Express your answer numerically using two significant figures. • View Available Hint(s) ? Kb =
If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic and 12-14 is strongly basic. Then what is seltzer water with a pH of 3.5? If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic and 12-14 is strongly basic. Then what is drain cleaner with a pH of 13? If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic and 12-14 is strongly basic. Then what is a hot tub with pH of 7.8?
When you cool down water to 10°C, Kw = 2.9 x 10-15, as compared to the value of Kw at 25°C which is 1 x 10-14 (a bigger K at a higher temp). Which statement is true? a) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 14.5 b) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 14.5 c) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 7.27 d) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 7.27 e) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 7 f) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 7
An unknown compound, X, is thought to have a carboxyl group with a pK₂ of 2.5 and a second ionizable group with a pKa between 5.0 and 8.0. When 50.0 mL of 0.2 M NaOH is added to 75.0 mL of a 0.2 M solution of X at pH 2.5, the pH increases to 7.13. Calculate the pK₂ of the second ionizable group of X. pK₂ = 6.97 Incorrect