kindy answer asap. i will leave like ones done 18H1.00e"Values of atomic weights are based on the AtomicWeights of the Elements 1995 published by IUPAC13 14 15Не4.003161710LiBe6.941 9.012N16.00 19.00 20.19FNe10.01 12.01 14.011112131415161718NaMgAlSiPCIAr345610 11 1222.99 24.3126.99 20.09 30.97 32.07 35.45 29.95202122242526273132Ge2328293033343536CoNi39.10 40.08 44.96 47.87 50.94 52.00 54.94 55.85 58.93 58.69 63.55 65.39 69.72 72.61 74.92 78.95 79.90 83.80KСаScTiVCrMnFeCuZnGaAsSeBrKr5343To85.47 87.62 88.91 | 91.2292.91 95.94| (98)383940414244464050515254RbSrYZrNbMoRuRhPdAgCdInSnSbTeIXe101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.5 126.9 131.355Cs57La72Hf73Ta7475Re76Os70Pt79Au83Bi5584ВаIrHgTIPbPoAtRn132.9 137.3 138.9 178.5 180.9 183.8| 186.2 190.2 192.2 195.1| 197.0 200.6 204.4 207.2 209.0 (209) (210) | (222)104T05107109110111Sg(223) (226) e) (261) 2 c263)L262) (265) L265) (269) e2)FrRaAc+RfDbBhHsMtDsRg5871Lu140.1 140.9 144.2 (145) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.05960Nd61626364656667686970CePrPmSmEuGdTbDyНоErTmYb"Lanthanides96Am Cm232.0 231.0 238.0 (237) (244) (243) (247) (247) (251) (252) (257) (258) (259) (262)90Th91929394959799100102103LrРаNpPuBkCfEsFmMdNo*Actinides At 25°C, the K, for a certain monoprotic acid HA is 6.2x10-10, what will be the K, value for the givenreaction below?HA(aq) + H2O) AA (aq) + H3Oʻ(aq)O 6.2x10 10O 3.8x10-19O 1.6x10-5O 2.5x10-5

Here we are required to find the dissociation constant for the weak monoprotic acid HA

Answered: At 25°C, the K, for a certain…

At 25°C, the K, for a certain monoprotic acid HA is 6.2x10-10, what will be the K, value for the given reaction below? HA(aq) + H2O) AA (aq) + H3Oʻ(aq) O 6.2x10 10 O 3.8x10-19 O 1.6x10-5 O 2.5x10-5

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 17CR: . a. Write the conjugate acid for each of the following Brønsted-Lowry bases....

See similar textbooks

Similar questions

Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.
For each of the following salts in water, predict whether the pH will be greater than, less than, or equal to 7. (a) KBr (b) NH3NO3 (c) AlCl3 (d) Na2HPO4
Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.
Calculate the pH and the pOH of each of the following solutions at 25 C for which the substances ionize completely: (a) 0.200 M HCl. (b) 0.0143 M NaOH. (c) 3.0 M HNO3. (d) 0.0031 M Ca(OH)2
. a. Write the conjugate acid for each of the following Brønsted-Lowry bases. NO3.HSO4,ClO4,NH3,HCO3b. Write the conjugate base for each of the following Brønsted- Lowry acids. HCI,H2SO4,NH3,NH4,HCO3
Determine Kb for the nitrite ion, NO2-. In a 0.10-M solution this base is 0.0015% ionized.
Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
Ionization of the first proton from H2SeO4 is complete (H2SeO4 is a strong acid); the acid-ionization constant for the second proton is 1.2 102. a What would be the approximate hydronium-ion concentration in 0.150 M H2SeO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.150 M H2SeO4, accounting for the ionization of both protons.
Several acids are listed here with their respective equilibrium constants: C6H5OH(aq) + H2O() H3O+(aq) + C6H5O(aq) Ka = 1.3 1010 HCO2H(aq) + H2O() H3O+(aq) + HCO2(aq) Ka = 1.8 104 HC2O4(aq) H2O() H3O+(aq) + C2O42(aq) Ka = 6.4 105 (a) Which is the strongest acid? Which is the weakest acid? (b) Which acid has the weakest conjugate base? (c) Which acid has the strongest conjugate base?
Calculate [H+] and pH in a solution in which lactic acid, HC3H5O3, is 0.250 M and the lactate ion, C3H5O3-, is (a) 0.250 M (b) 0.125 M (c) 0.0800 M (d) 0.0500 M
For each of the following reactions, indicate the BrĂ¸nsted-Lowry acids and bases. What are the conjugate acid/base pairs? (a) H3 O+(aq)+CN(aq)HCN(aq)+H2O (b) HNO2(aq)+OH(aq)NO2(aq)+H2O (c) HCHO2(aq)+H2OCHO2(aq)+H3 O+(aq)
Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.