5) Determine Ka for Phosphoric acid. In a 1.0 M solution of this acid when the...
5) Determine Ka for Phosphoric acid. In a 1.0 M solution of this acid when the acid is 8.3% ionized:
a) Write the acid ionization reaction and the equilibrium expression for this reaction.
b) Using the RICE table, calculate the value of Ka
Homework Answers
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5) Determine Ka for Phosphoric acid. In a 1.0 M
solution of this acid when the...
Determination of the Dissociation Constant ka, of a Weak Acid Part A Phosphoric acid is a...
Determination of the Dissociation Constant ka, of a Weak Acid Part A Phosphoric acid is a triprotic acid (three ionizable hydrogens). The values of its stepwise ionization constants are Kit = 75 x 10°,K6.2 x10, and K. = 4.2 x 10" 1. Write the chemical equation for the first ionization reaction of phosphoric acid with water. 2. Write the equilibrium constant expression Kat for this reaction. 3. What would be the pH of a solution when [H,PO) -(H.PO:] Part B...
An aqueous solution of phosphoric acid, that is 0.500 percent by weight phosphoric acid, has a...
An aqueous solution of phosphoric acid, that is 0.500 percent by weight phosphoric acid, has a density of 1.0010 g/mL. A student determines that the freezing point of this solution is -0.129 °C. Based on the observed freezing point, what is the percent ionization of the acid and the value of Ka1? Assume that only the first ionization of the acid is important. Kf for H2O is 1.86 °C/m. % ionized = % Ka1 =
buffer solutions 1. Determine the volume of 1.0 M tartaric acid, H2CaH&Os, solution that when diluted...
buffer solutions
1. Determine the volume of 1.0 M tartaric acid, H2CaH&Os, solution that when diluted to a total volume of 250.0 mL produces a solution that is 0.050 M in tartaric acid. 2. Determine the mass of potassium hydrogen tartrate, KHC&H4O6, required to prepare 250.0 mL of a solution that is 0.050 M in hydrogen tartrate ion. 3a. Write a balanced equation and corresponding K, expression for the ionization of the weak acid lactic acid (HC3HsO3, Ka 1.62 x...
1. Determine the volume, in mL, of 2.00 M HC2H3O2 stock solution that would need to...
1. Determine the volume, in mL, of 2.00 M
HC2H3O2 stock solution that would
need to be diluted to 50 mL in order to produce a solution that is
0.30 M in HC2H3O2.
2. Write the equilibrium constant expression, Ka, for
the ionization of acetic acid,
HC2H3O2.
3.In the rICE table for the dissociation of acetic acid, what is
the expression for acetic acid taken directly from the equilibrium
line of your ICE table? Do not use the x is...
(3 points) A 0.0730 M solution of a monoprotic acid is 1.07% ionized. What is the...
(3 points) A 0.0730 M solution of a monoprotic acid is 1.07% ionized. What is the pH of the solution? Calculate the Ka of the acid. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? (2 points) Determine the percent ionization of a 0.0028 M HA solution. (Ka of HA = 1.4 x 10-9) (4 points) Lysine is triprotic amino acid (separately loses three H’s in...
please help. 1. (3 polnts) A 0.0730 M solution of a monoprotic acid is 1.07 %...
please help.
1. (3 polnts) A 0.0730 M solution of a monoprotic acid is 1.07 % ionized. What is the pH of the solution? a. b. Calculate the K, of the acid. 2. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? 3. (2 points) Determine the percent ionization of a 0.0028 M HA solution. (K, of HA 1.4 x 10") 4. (4 points) Lysine is...
Calculate the equilibrium concentration of a weak acid HA solution when 20.0 mL of 1.0 M...
Calculate the equilibrium concentration of a weak acid HA solution when 20.0 mL of 1.0 M HA is mixed with 20.0 mL of 1.0 M NaA. (Ka = 1.8x10-5)
5. You have a 5.0 M solution of phosphoric acid, H3PO4 a. Write an equation three...
5. You have a 5.0 M solution of phosphoric acid, H3PO4 a. Write an equation three dissociation equations. b. As the species becomes more negative, the protons are more attracted to the species. What does this do to acid strength? C. Determine the concentration of all species in solution. Below are the needed ka values. • Ka, = 7.5 x 10-3 • Ka, = 6.2 x 10-8 • Ka, = 4.8 x 10-13 I MacBook 3013
the answer i have entered is incorrect Ksp = 1.0 x 10^-25 Ka = Phosphoric acid...
the answer i have entered is incorrect
Ksp = 1.0 x 10^-25
Ka =
Phosphoric acid
H3PO4
7.5×10-3
6.2×10-8
3.6×10-13
Write a balanced net ionic equation to show why the solubility of Ca3(PO4)2 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Consider only the FIRST STEP in the reaction with strong acid. Use the pull-down boxes to specify states such as (aq) or (s)....
The enthaply of neutralization of Phosphoric Acid Please help with 1-5 The Enthalpy of Neutralization of...
The
enthaply of neutralization of Phosphoric Acid
Please help with 1-5
The Enthalpy of Neutralization of Phosphoric Acid DATA TABLE Trial 3 Trial 1 Trial 2 Maximum temperature (c) 3 Initial temperature ("C) Temperature change (AT o C DATA ANALYSIS 1. Write the balanced equation for the reaction of phosphoric acid and sodium hydroxide. 2. Use the equation below to calculate the amount of heat determining the mass, m, of the solution use 1.11 g/mL for the density. Use 4.18...
Determination of the Dissociation Constant ka, of a Weak Acid Part A Phosphoric acid is a triprotic acid (three ionizable hydrogens). The values of its stepwise ionization constants are Kit = 75 x 10°,K6.2 x10, and K. = 4.2 x 10" 1. Write the chemical equation for the first ionization reaction of phosphoric acid with water. 2. Write the equilibrium constant expression Kat for this reaction. 3. What would be the pH of a solution when [H,PO) -(H.PO:] Part B...
buffer solutions
1. Determine the volume of 1.0 M tartaric acid, H2CaH&Os, solution that when diluted to a total volume of 250.0 mL produces a solution that is 0.050 M in tartaric acid. 2. Determine the mass of potassium hydrogen tartrate, KHC&H4O6, required to prepare 250.0 mL of a solution that is 0.050 M in hydrogen tartrate ion. 3a. Write a balanced equation and corresponding K, expression for the ionization of the weak acid lactic acid (HC3HsO3, Ka 1.62 x...
1. Determine the volume, in mL, of 2.00 M
HC2H3O2 stock solution that would
need to be diluted to 50 mL in order to produce a solution that is
0.30 M in HC2H3O2.
2. Write the equilibrium constant expression, Ka, for
the ionization of acetic acid,
HC2H3O2.
3.In the rICE table for the dissociation of acetic acid, what is
the expression for acetic acid taken directly from the equilibrium
line of your ICE table? Do not use the x is...
please help.
1. (3 polnts) A 0.0730 M solution of a monoprotic acid is 1.07 % ionized. What is the pH of the solution? a. b. Calculate the K, of the acid. 2. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? 3. (2 points) Determine the percent ionization of a 0.0028 M HA solution. (K, of HA 1.4 x 10") 4. (4 points) Lysine is...
5. You have a 5.0 M solution of phosphoric acid, H3PO4 a. Write an equation three dissociation equations. b. As the species becomes more negative, the protons are more attracted to the species. What does this do to acid strength? C. Determine the concentration of all species in solution. Below are the needed ka values. • Ka, = 7.5 x 10-3 • Ka, = 6.2 x 10-8 • Ka, = 4.8 x 10-13 I MacBook 3013
the answer i have entered is incorrect
Ksp = 1.0 x 10^-25
Ka =
Phosphoric acid
H3PO4
7.5×10-3
6.2×10-8
3.6×10-13
Write a balanced net ionic equation to show why the solubility of Ca3(PO4)2 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Consider only the FIRST STEP in the reaction with strong acid. Use the pull-down boxes to specify states such as (aq) or (s)....
The
enthaply of neutralization of Phosphoric Acid
Please help with 1-5
The Enthalpy of Neutralization of Phosphoric Acid DATA TABLE Trial 3 Trial 1 Trial 2 Maximum temperature (c) 3 Initial temperature ("C) Temperature change (AT o C DATA ANALYSIS 1. Write the balanced equation for the reaction of phosphoric acid and sodium hydroxide. 2. Use the equation below to calculate the amount of heat determining the mass, m, of the solution use 1.11 g/mL for the density. Use 4.18...
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