A solution was made by adding of 2.81 g of ethyl amine (CH3CH2NH2)to water making 500.0...
A solution was made by adding of 2.81 g of ethyl amine (CH3CH2NH2)to water making 500.0 mL of solution. After the solution had come to equilibrium, the concentration of ethyl amine was found to be 0.118 M.
a) What is the pH of the solution?
b) What is the value of Kb for ethyl amine?
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A solution was made by adding of 2.81 g of ethyl amine
(CH3CH2NH2)to water making 500.0...
6 A solution is made by dissolving 35.5 g of Ba(NO2)2 in 500.0 mL of water....
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For each of the following solutions, calculate the initial pH and the final pH after adding...
For each of the following solutions, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH. A.For 210.0 mL of pure water, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH. B. For 210.0 mL of a buffer solution that is 0.245 M in HCHO2 and 0.315 M in KCHO2, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH(Ka=1.8⋅10−4). C. For 210.0 mL of a buffer...
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what is the pH of a solution made by adding 0.25 g of NaOCl to enough water to make 67.3 ml of solution?
Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of...
Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3. Agt reacts with NH3 to form AgNH3* and Ag(NH3)2*: Ag* + NH3 <--> AgNH3* Ki = 2.1 x 103 AgNH3* + NH3 <--> Ag(NH3)2* K2 = 8.2 x 103 The concentration of Ag(NH3)2* at equilibrium is
23. For each solution, calculate the initial pH and the final pH after adding 0.010 mol...
23. For each solution, calculate the initial pH and the final pH after adding 0.010 mol of HCI. a. 500.0 mL of pure water b. 500.0 mL of a buffer solution that is 0.125 M in HC,H,O, and 0.115 M in NaC,H,O, c. 500.0 mL of a buffer solution that is 0.155 M in CH NH, and 0.145 M in CH NH,CI
e. using kb(NO2-)=2.2x10^-11, determine the pH of the solution 19 A solution is made by dissolving...
e. using kb(NO2-)=2.2x10^-11, determine the pH of the
solution
19 A solution is made by dissolving 44.9 g of Ba(NO2)2 in 500.0 mL of water. a Does Ba2+ have any acidic or basic properties? O of 0.2 points earned b Does NO, have any acidic or basic properties? O of 0.2 points earned C As NO, is a base, write the basic equilibrium equation that exists in solution O of 0.2 points earned d What is the value of Kb...
QUESTION 3 A solution is made by adding 25.6 g of KNO3 to water until the...
QUESTION 3 A solution is made by adding 25.6 g of KNO3 to water until the solutions volume is 750.0 mL What is the molarity of the solution? M (give answer to correct sig figs in units of molarity, M)
A buffer solution is made by adding 20.0 mL of a 0.50 M Na2CO3 solution to 10.0...
A buffer solution is made by adding 20.0 mL of a 0.50 M Na2CO3 solution to 10.0 mL of a 0.50 M NaHCO3 solution in a test tube. The pH of this buffer was found to be 10.20. After 2.0 mL of 1.0 M HCl solution is added to this buffer solution, the pH is measured to be 9.95. What is the buffering capacity with respect to a strong acid, βa, of this buffer solution, in units of mol/L per pH unit?...
6 A solution is made by dissolving 35.5 g of Ba(NO2)2 in 500.0 mL of water. Does Ba2+ have any acidic or basic properties? a O of 2 points earned 20 attempts remaining Does NO, have any acidic or basic properties? O of 2 points earned 20 attempts remaining Write the basic equilibrium equation that exists in solution с O of 2 points earned 20 attempts remaining What is the value of Kb for NO2-? The Ka of HNO2 is...
Calculate the pH of a solution made by adding 42 g of sodium acetate, NaCH3COO, to 22 g of acetic acid, CH3COOH, and dissolving in water to make 300. mL of solution. Hint given in feedback. The K, for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. Answer: Calculate the pH of a solution made by adding 59 g of sodium acetate, NaCH3COO, to 22 g of acetic acid, CH3COOH, and dissolving in water...
Calculate the pH of a solution made by adding 25.0 g of sodium formate, NaHCOO, to 400 ml of 0.64 M formic acid, нсоон. Answer: What is the pH of pure water at 25°C? Answer: When a small amount of acid is added to a non-buffered solution, there is a large change in pH. Calculate the pH when 22.2 ml of 0.0020 M HCl is added to 100.0 mL of pure water. Comment and hint in the general feedback Answer:
Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3. Agt reacts with NH3 to form AgNH3* and Ag(NH3)2*: Ag* + NH3 <--> AgNH3* Ki = 2.1 x 103 AgNH3* + NH3 <--> Ag(NH3)2* K2 = 8.2 x 103 The concentration of Ag(NH3)2* at equilibrium is
23. For each solution, calculate the initial pH and the final pH after adding 0.010 mol of HCI. a. 500.0 mL of pure water b. 500.0 mL of a buffer solution that is 0.125 M in HC,H,O, and 0.115 M in NaC,H,O, c. 500.0 mL of a buffer solution that is 0.155 M in CH NH, and 0.145 M in CH NH,CI
e. using kb(NO2-)=2.2x10^-11, determine the pH of the
solution
19 A solution is made by dissolving 44.9 g of Ba(NO2)2 in 500.0 mL of water. a Does Ba2+ have any acidic or basic properties? O of 0.2 points earned b Does NO, have any acidic or basic properties? O of 0.2 points earned C As NO, is a base, write the basic equilibrium equation that exists in solution O of 0.2 points earned d What is the value of Kb...
QUESTION 3 A solution is made by adding 25.6 g of KNO3 to water until the solutions volume is 750.0 mL What is the molarity of the solution? M (give answer to correct sig figs in units of molarity, M)
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