Form 1 29. Determine the pH of a 0.741 M LiOH solution at 25°C. A) 0.130...
what is the hydronium ion concentration [H3O+] and the ph of a 0.5M acetic acid solution with Ka=1.8x10^-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H2O(l) = H3O + (aq) + CH3CO2-(aq)
1. Calculate the pH of the following solutions. Show all of your work. a. 0.0050 M nitric acid, HNO3 b. 0.50 M hydrocyanic acid, HCN Ka = 4.0 x 10-10 2. A student was given the following problem: Calculate the pH of a 0.50 Mama bromide (NHaBr) solution if the Kb of NH3 is 1.8 x 10. The student provided the fo work. Identify the error(s) and calculate the correct pH. NH; (aq) + H20 (1) = NH3 (aq) +...
a.) Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka= 1.0×10−3. b.) Find the percent dissociation of this solution c.) Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka= 0.11. d.) Find the percent dissociation of this solution.
Calculate the hydronium ion concentration and the pH of the solution that results when 22.6 mL of 0.060 M acetic acid,CH3CO2H (Ka= 1.8 x 10^-5), is mixed with 1.4 mL of 0.17 M NaOH . Hydronium ion concentration = pH =
22) What is the [CH3CO2-1/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.79? Ka = 1.78 x 10-5 for CH3CO2H. A) 0.94:1 B) 2.0:1 C) 1.1:1 D) 0.50:1 23) Which is the best acid to use in the preparation of a buffer with pH = 3.3? A) HNO3 B) HOI (Ka = 2.0 x 10-11) C) HNO2 (Ka = 4.5 x 104) D) HIO3 ((Ka = 1.7 x 10-1) 24) What is the percent dissociation of...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that has Ka = 9.28 x 10 2. Determine the Kb of a weak base if a 2.50 M solution of the base has a pH of 9.595 at 25°C. 3. The overall dissociation of malonic acid, H2C3H2O4, is represented below. The overall dissociation constant is also indicated. H2C3H204 = 2 H+ + C3H2042- K = 3.0 x 10-9 To a 0.025-molar solution of malonic...
Determine eacg of the following for a 0.130 M HBr solution: a) [H3O+] b) pH c)pOH d) write the balanced equation for the reaction with LiOH e) calulate the volume in milliliters, of HBr solution required to nuetralize 35 mL of a .340 M LiOH solution
Calculate the hva hydronium ion. the hydroxide ion concentration in a intration in an aqueous solution that contains 3.50 x 10-3 Min A) 2.86 x 10-12 M B) 2.86 x 10-4 M 20) At what pH is the A) 9.60 what pH is the amino acid glycine with a Ka of 2.51 x 10-10 sixty-six (66%) percent di B) 10.10 C) 10.60 C) 3.50 10-12 M 19) D) 2.86 * 10-11 M ST ANSWER. Write the word or phrase that...
please explain the steps please 5. Determine the Ky for CN at 25°C. The K, for HCN is 4.9 x 10-10. 6. Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. 7. Determine the acid dissociation constant for a 0.020 M formic acid solution that has a pH of 2.74. Formic acid is a weak monoprotic acid and the equilibrium equation of interest is HCOOH(aq) + H20(1) =H30+(aq) + HCO2-(aq).
Question 47 (1 point) Calculate the pH of a solution that is 0.310 Min sodium formate (NaHCO2) and 0.190M in formic acid (HCO2H). The Ką of formic acid is 1.77 x 10-4. 13.79 3.532 3.958 4.975 10.04 MOCRA Question 42 (1 point) What is the hydronium ion concentration of a 0.100 M hypochlorous acid solution with Ka = 35 x 10-87 The equation for the dissociation of hypochlorous acid is: HOCH(aq) + H2011) =H30*(aq) + OCH@g). O 1.9 x 10-5...