2.0 mol of methylamine, CH3NH2, are dissolved into 1.0 L of water. Given that its pKb...
2.0 mol of methylamine, CH3NH2, are dissolved into 1.0 L of water. Given that its pKb is 3.38, compose a balanced chemical reaction (equation) for the dissociation, and calculate the fraction of CH3NH2 that dissociates in water (i.e., forms CH3NH3+) and the pH when the dissociation approaches equilibrium.
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2.0 mol of methylamine, CH3NH2, are dissolved into 1.0 L of
water. Given that its pKb...
What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the...
What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2)
solution after the addition of 50 mL of a 0.5 mol/L solution of
HCl?
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCI?
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after...
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCI? Your angwer
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution 2...
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution 2 points after the addition of 50 mL of a 0.5 mol/L solution of HCI? Your answer O BE
If the a mixture of methylamine (CH3NH2, p Kb = 3.32) in water produces a pH...
If the a mixture of methylamine (CH3NH2, p Kb = 3.32) in water produces a pH of 11.8, what is the initial molar concentration of methylamine in the solution? O A 2.6x10-4M O B 7.7x10-2M O c 3.4x10-5M O D 8.3x10-2M Triethylamine (C2H5)3N) has a pKb = 3.25. What is the value of the equilibrium constant K for this reaction: (C2H5)3NH(aq) + H2O(1) = (C2H5)3N(aq) + H3O+(aq)? O A 1.77x10-11 O B 5.62x10-4 o C More information is needed to...
1.0 mol of ethanol and 1.0 mol of acetic acid are dissolved in water and kept...
1.0 mol of ethanol and 1.0 mol of acetic acid are dissolved in
water and kept at 100? degrees C. The volume of the solution is 250
mL. At equilibrium, 0.25 mol of acetic acid has been consumed in
producing ethyl acetate. Calculate Kc? at 100 degrees C
for the reaction: C2H5OH?(aq) +
CH3CO2H(aq)
CH3CO2C2H5(aq)
+ H2O?(l)
When 2.0 moles of KCl is dissolved in 1.0 L of water, the boiling point of...
When 2.0 moles of KCl is dissolved in 1.0 L of water, the boiling point of the solution will be ___ than the boiling point of pure water.
What is the pH of a sample of river water in which (HCO3-) = 2.0 x...
What is the pH of a sample of river water in which (HCO3-) = 2.0 x 10-4 M and the concentration of dissolved CO2 in equilibrium with atmospheric CO2 is 1.0 x 10-5 M? Chemical Equation: H2CO3(aq) + H2O(l) = HCO3-(aq) + H3O+(aq) pka = 6.37 Henderson Hasselbach equation: pH=pka+log [base]/[acid] A/
A 6.0-L vessel was found to contain 1.0 mol BrCly, 2.0 mol Br2 and 6.0 mol...
A 6.0-L vessel was found to contain 1.0 mol BrCly, 2.0 mol Br2 and 6.0 mol Cl2. What is the equilibrium constant, K, for this equilibrium mixture for the reaction 2BrCls(8) Br2(g) + 3C12(8)? O 108 432 18 0.014 12
10. If 1.50 g of solid C.HsNH:Cl is dissolved in 1.0 L of water, what is...
10. If 1.50 g of solid C.HsNH:Cl is dissolved in 1.0 L of water, what is the pH of the solution? Molar Mass CH-NH3CI - 129.59 g/mol A. B. c. D. E. 1.93 3.27 7.00 10.73 14.00
1. At a particular temperature, a 3.0-L flask contains 2.4 mol Cl2, 1.0 mol NOCI, and...
1. At a particular temperature, a 3.0-L flask contains 2.4 mol Cl2, 1.0 mol NOCI, and 4.5 x 10-3 mol NO. Calculate K at this temperature for the following reaction: 2NOCI(g) — 2NO(g) + C13(g) 2. At a particular temperature, 8.0 mol NO2 is placed into a 1.0-L container and the NO2 dissociates by the reaction: 2NO,(8) 2NO(g) + 0,(8) At equilibrium the concentration of NO(g) is 2.0 M. Calculate K for this reaction. 3. Ammonia is produced by the...
What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2)
solution after the addition of 50 mL of a 0.5 mol/L solution of
HCl?
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCI?
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCI? Your angwer
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution 2 points after the addition of 50 mL of a 0.5 mol/L solution of HCI? Your answer O BE
If the a mixture of methylamine (CH3NH2, p Kb = 3.32) in water produces a pH of 11.8, what is the initial molar concentration of methylamine in the solution? O A 2.6x10-4M O B 7.7x10-2M O c 3.4x10-5M O D 8.3x10-2M Triethylamine (C2H5)3N) has a pKb = 3.25. What is the value of the equilibrium constant K for this reaction: (C2H5)3NH(aq) + H2O(1) = (C2H5)3N(aq) + H3O+(aq)? O A 1.77x10-11 O B 5.62x10-4 o C More information is needed to...
1.0 mol of ethanol and 1.0 mol of acetic acid are dissolved in
water and kept at 100? degrees C. The volume of the solution is 250
mL. At equilibrium, 0.25 mol of acetic acid has been consumed in
producing ethyl acetate. Calculate Kc? at 100 degrees C
for the reaction: C2H5OH?(aq) +
CH3CO2H(aq)
CH3CO2C2H5(aq)
+ H2O?(l)
What is the pH of a sample of river water in which (HCO3-) = 2.0 x 10-4 M and the concentration of dissolved CO2 in equilibrium with atmospheric CO2 is 1.0 x 10-5 M? Chemical Equation: H2CO3(aq) + H2O(l) = HCO3-(aq) + H3O+(aq) pka = 6.37 Henderson Hasselbach equation: pH=pka+log [base]/[acid] A/
A 6.0-L vessel was found to contain 1.0 mol BrCly, 2.0 mol Br2 and 6.0 mol Cl2. What is the equilibrium constant, K, for this equilibrium mixture for the reaction 2BrCls(8) Br2(g) + 3C12(8)? O 108 432 18 0.014 12
10. If 1.50 g of solid C.HsNH:Cl is dissolved in 1.0 L of water, what is the pH of the solution? Molar Mass CH-NH3CI - 129.59 g/mol A. B. c. D. E. 1.93 3.27 7.00 10.73 14.00
1. At a particular temperature, a 3.0-L flask contains 2.4 mol Cl2, 1.0 mol NOCI, and 4.5 x 10-3 mol NO. Calculate K at this temperature for the following reaction: 2NOCI(g) — 2NO(g) + C13(g) 2. At a particular temperature, 8.0 mol NO2 is placed into a 1.0-L container and the NO2 dissociates by the reaction: 2NO,(8) 2NO(g) + 0,(8) At equilibrium the concentration of NO(g) is 2.0 M. Calculate K for this reaction. 3. Ammonia is produced by the...
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