11. Calculate the concentrations of all species, pH and % ionization for each of the following.a) 0.20 M HC2H3O2(Ka = 1.75×105)b) 1.5 M HNO₂c) 0.10 M NH3d) 0.25 M HN3(Ka = 7.10×105)(Kb = 1.75×105)(Ka = 2.20×105)

(a) 0.20 M HC₂H₃O₂ (Ka = 1.75 × 10⁻⁵)Step 1. Write the ionization equation:HC2H3O2⇌H++C2H3O2−…

Answered: 11. Calculate the concentrations of all…

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...

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1) Calculate the molar H3O+ ion concentration of a solution that has a pH of A) 3.73 B) 0.59 C) 11.29 D) -0.76 2) Convert the following p -functions to molar concentrations: A) pOH = 0.0057 B) pCa= -0.221 C) pCl = 8.92
Enough of a monoprotic acid is dissolved in water to produce a 0.0040 M solution. The pH of the resulting solution is 3.50. What is the Ka of the acid? Be careful any approximations you may implicitly assuming are true. A) 0.0790 B) 40,000 C) 2.500 × 10-5 D) 2.715 × 10-5 E) 36,832
Calculate the pH of the following: 5) A solution that contains 0.10 M ammonium hydrochloride and 0.010 M HCl
7. A 0.050 M solution of an organic acid has a [H*] = 5.9 x 103 M. a) Calculate the pH of the solution. b) What is the % ionization? c) Calculate the Ka of the acid.
Which of the following solutions would be expected to have a pH of 7.00? Unanswered and currently due f Weak Acid K₁ HON HNO. HIO HBrO C.H.COOH A) CSlo B) NaF C) LICIO, D) KNO₂ 4.9 x 10-1 4.5 x 10-1 2.3 x 10-11 2.5 x 10. 6.3 x 10-5 Weak Base HÌNH, NH, CHINH, H.NNH C.H.N Kb 11x10: 1.8 x 10-5 4.3 x 10-19 1.3 x 10 1.7 x 10-1
11. A 0.0900 M solution of a monoprotic acid is 11.5 percent ionized. Calculate the ionization constant (Ka) of the acid. a) 2.46 x 10-7 b) 7.82 % 10-2 c) 7.34 x 10-5 d) 1.67 x 10-5 e) 1.34 x 10-3 f) 3.35 x 10-3 g) 2.78 × 10-3
Determine the pH of an HF solution of each of the following concentrations. The KA value of HF is 6.86.8 ×10−4×10−4. a) 0.290M b) 4.50×10−2 M c) 2.20×10−2 M d) in which cases can you not make the simplifying assumption that x is small?
What is the pH of a solution that is 0.250 M formic acid and 1.75 M sodium formate? Ka= 1.8x104 А) 6.74 В) 5.43 4.59 3.74
The SO3 (gaseous) produced is bubbled in water, until getting a solution of H2SO4 68 % mass/mass density= 1.06 g/cm3 a) calculate the volume of said solution to make 1.5 dm3 of a solution 0.3% mass/volume b) what will be the pH of the more diluted solution? c) what will be the resulting pH of mixing 300 ml of a diluted solution with 250 ml of a NaOH 0.1 molar solution d) calculate the molar concentration of sulfate ions in the final mixture
Help with parts D-F please

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11. Calculate the concentrations of all species, pH and % ionization for each of the following. a) 0.20 M HC2H3O2 (Ka = 1.75×105) b) 1.5 M HNO₂ c) 0.10 M NH3 d) 0.25 M HN3 (Ka = 7.10×105) (Kb = 1.75×105) (Ka = 2.20×105)