O ACIDS AND BASES1/5Deriving K, from KaComplete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C.conjugate acidconjugate baseformulaK,formulaK,NH,-51.8 x 10- 104.9 x 10HCN-6C,H,ONH2.1 x 10III O KINETICS AND EQUILIBRIUM1/5Calculating equilibrium composition from an equilibrium constantSuppose a 500. mL flask is filled with 1.1 mol of Cl,, 0.20 mol of HCl and 0.80 mol of CCl,. The following reaction becomes possible:Cl,(g) +CHCI, (g) = HCl(g)+CCl, (g)The equilibrium constant K for this reaction is 9.65 at the temperature of the flask.Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.| MII

“Since you have asked multiple question, we will solve the first question for you. If you want any…

Complete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C. conjugate acid conjugate base formula K. formula K, NH, -5 1.8 x 10 HCN -10 4.9 x 10 C,H, ONH -6 2.1 x 10

Complete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C. conjugate acid conjugate base formula K. formula K, NH, -5 1.8 x 10 HCN -10 4.9 x 10 C,H, ONH -6 2.1 x 10

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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Question

O ACIDS AND BASES
1/5
Deriving K, from Ka
Complete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C.
conjugate acid
conjugate base
formula
K,
formula
K,
NH,
-5
1.8 x 10
- 10
4.9 x 10
HCN
-6
C,H,ONH
2.1 x 10
III

O KINETICS AND EQUILIBRIUM
1/5
Calculating equilibrium composition from an equilibrium constant
Suppose a 500. mL flask is filled with 1.1 mol of Cl,, 0.20 mol of HCl and 0.80 mol of CCl,. The following reaction becomes possible:
Cl,(g) +CHCI, (g) = HCl(g)+CCl, (g)
The equilibrium constant K for this reaction is 9.65 at the temperature of the flask.
Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.
| M
II

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