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please calculate the value of the equilibrium constant
2. The beaker contains 0.1894 M CHCOOH and...
20.0ml of 0.100M HC2H3O2 solution in a small beaker is titrated with 0.10M NaOH solution from a b...
20.0ml of 0.100M HC2H3O2 solution in a small beaker is titrated with 0.10M NaOH solution from a buret. All experiments are carried out at 25°C 3. a) Write the acid-base reaction that occurs during the titration. b) Calculate the value of the equilibrium constant for the titration reaction written in 3a. Is it reasonable to assume that this titration reaction goes essentially to completion? Explain. c) Predict the pH (acidic, basic, or neutral) after 20.0mL are added during the titration....
Write the chemical reaction for the autoionization of water (equilibrium constant Kw). Look up the numerical...
Write the chemical reaction for the autoionization of water (equilibrium constant Kw). Look up the numerical value for Kw at Tinitial (Use the average of Tinitial from both trials) -Its 6.81x10^-15 How is the equation in Question 1 related to the net ionic equation for the strong acid-strong base neutralization shown below? H3O+(aq) + OH-(aq) → H2O(l) + H2O(l) Use the value of Kw and the relationship between the equations in Questions 1 and 3 to find the numerical value...
20.0ml of 0.100M HC2H3O2 solution in a small beaker is titrated with 0.10M NaOH solution from...
20.0ml of 0.100M HC2H3O2 solution in a small beaker is titrated with 0.10M NaOH solution from a buret. All experiments are carried out at 25°C 3. a) Write the acid-base reaction that occurs during the titration. b) Calculate the value of the equilibrium constant for the titration reaction written in 3a. Is it reasonable to assume that this titration reaction goes essentially to completion? Explain. c) Predict the pH (acidic, basic, or neutral) after 20.0mL are added during the titration....
I'm doing a titration lab tomorrow and I am not sure what the formulas are to...
I'm doing a titration lab tomorrow and I am not sure what the
formulas are to calculate the moles of NaOH, the moles of
HCl, and the molarity of HCl.
The objective of this laboratory is to determine the molarity of
a hydrochloric acid solution using a known concentration of sodium
hydroxide as the titrant.
volume of HCl in flask: 25.00 mL
the net ionic equation for the reaction is:
H+(aq) + OH-(aq) --> H2O(l)
I don't have the data...
Molarity for NaOH = 0.0873 2. In a second titration with the same solution of NaOH as used in Question #1, the student...
Molarity for NaOH = 0.08732. In a second titration with the same solution of NaOH as used in Question #1, the student weighs out a sample of KHP of 0.359 g. Calculate the volume of the NaOH solution needed to neutralize this sample of KHP. 3. A monoprotic weak acid with the general formula of HA will react with a base, such as NaOH. Write the neutralization equation which describes the reaction. 4. If K, for the weak acid, HA is 1.8...
1.A 1.00 liter solution contains 0.28 M acetic acid and 0.36 M sodium acetate. If 0.180...
1.A 1.00 liter solution contains 0.28 M acetic acid and 0.36 M sodium acetate. If 0.180 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of potassium hydroxide.) A. The number of moles of CH3COOH will remain the same. B. The number of moles of CH3COO- will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will increase....
Write a balanced net ionic equation to show why the solubility of Zn(CN)2(s) increases in the pre...
Write a balanced net ionic equation to show why the solubility
of Zn(CN)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.
I really need help with both because I am on my last attempt and
cannot seem to understand exactly how to solve for K. Thank you for
your help! I will be sure to rate your answer if it is correct.
Write a balanced...
16. Each of three beakers contains 25.0 mL of 0.100 M solution at 25°C. Beaker 1...
16. Each of three beakers contains 25.0 mL of 0.100 M solution at 25°C. Beaker 1 Beaker 2 Beaker 3 0.10 M NaOH 0.10 M NaHCO3 0.10 M H2CO3 a. Determine the pH of the solution in beaker 1. Justify your answer. b. In beaker 2, the reaction HCO, (aq) + H2O(1) = H,CO, (aq) + OH(aq) occurs. The value of K, for HCO, (aq) is 2.3x108 at 25°C. i. Write the K, expression for the reaction of HCO, (aq)...
Ca(OH)2(s)+2CH3COOH(aq) -> Ca(CH3COO)2(aq) + 2H2O(aq) 11 (20 points) Please consider the reaction below. Ca(OH)2...
Ca(OH)2(s)+2CH3COOH(aq) -> Ca(CH3COO)2(aq) + 2H2O(aq)
11 (20 points) Please consider the reaction below. Ca(OH)2 (s) +2 CH3COOH (aq) -> Ca(CH3CO0)2 (aq)+ 2H20 (aq) (a) identify the acid 2 CH3C0OH 6identify the base 2H20 (c)write the overall ionic equation Ca(oH)2 Ca (CH3COO)z 2CH3COOH d) vrite the net ionic equation
I need help with solving these two questions Thanks 1?2? 1. The equilibrium constant for the...
I need help with solving these two questions
Thanks
1?2?
1. The equilibrium constant for the following reaction at 100°C is 0.11. If M ethanol (C2H,OH) and 0.810 M acetic acid (CH3COOH) are combined, what is the equilibrium concen- tration of ethyl acetate (CH3CO2C2Hs)? 6.816 2H,OH (aq) +CH,COOH(ag)CH,CO,C2Hs(ag) + H2O() 2. The KM for the decomposition of solid ammonium hydrogen sulfide to ammonia gas and hydrogen sulfide gas is 1.8 × 10-4 at 25°C. If ammonium hydrogen sulfide decomposes in...
20.0ml of 0.100M HC2H3O2 solution in a small beaker is titrated with 0.10M NaOH solution from a buret. All experiments are carried out at 25°C 3. a) Write the acid-base reaction that occurs during the titration. b) Calculate the value of the equilibrium constant for the titration reaction written in 3a. Is it reasonable to assume that this titration reaction goes essentially to completion? Explain. c) Predict the pH (acidic, basic, or neutral) after 20.0mL are added during the titration....
20.0ml of 0.100M HC2H3O2 solution in a small beaker is titrated with 0.10M NaOH solution from a buret. All experiments are carried out at 25°C 3. a) Write the acid-base reaction that occurs during the titration. b) Calculate the value of the equilibrium constant for the titration reaction written in 3a. Is it reasonable to assume that this titration reaction goes essentially to completion? Explain. c) Predict the pH (acidic, basic, or neutral) after 20.0mL are added during the titration....
I'm doing a titration lab tomorrow and I am not sure what the
formulas are to calculate the moles of NaOH, the moles of
HCl, and the molarity of HCl.
The objective of this laboratory is to determine the molarity of
a hydrochloric acid solution using a known concentration of sodium
hydroxide as the titrant.
volume of HCl in flask: 25.00 mL
the net ionic equation for the reaction is:
H+(aq) + OH-(aq) --> H2O(l)
I don't have the data...
Molarity for NaOH = 0.08732. In a second titration with the same solution of NaOH as used in Question #1, the student weighs out a sample of KHP of 0.359 g. Calculate the volume of the NaOH solution needed to neutralize this sample of KHP. 3. A monoprotic weak acid with the general formula of HA will react with a base, such as NaOH. Write the neutralization equation which describes the reaction. 4. If K, for the weak acid, HA is 1.8...
Write a balanced net ionic equation to show why the solubility
of Zn(CN)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.
I really need help with both because I am on my last attempt and
cannot seem to understand exactly how to solve for K. Thank you for
your help! I will be sure to rate your answer if it is correct.
Write a balanced...
16. Each of three beakers contains 25.0 mL of 0.100 M solution at 25°C. Beaker 1 Beaker 2 Beaker 3 0.10 M NaOH 0.10 M NaHCO3 0.10 M H2CO3 a. Determine the pH of the solution in beaker 1. Justify your answer. b. In beaker 2, the reaction HCO, (aq) + H2O(1) = H,CO, (aq) + OH(aq) occurs. The value of K, for HCO, (aq) is 2.3x108 at 25°C. i. Write the K, expression for the reaction of HCO, (aq)...
Ca(OH)2(s)+2CH3COOH(aq) -> Ca(CH3COO)2(aq) + 2H2O(aq)
11 (20 points) Please consider the reaction below. Ca(OH)2 (s) +2 CH3COOH (aq) -> Ca(CH3CO0)2 (aq)+ 2H20 (aq) (a) identify the acid 2 CH3C0OH 6identify the base 2H20 (c)write the overall ionic equation Ca(oH)2 Ca (CH3COO)z 2CH3COOH d) vrite the net ionic equation
I need help with solving these two questions
Thanks
1?2?
1. The equilibrium constant for the following reaction at 100°C is 0.11. If M ethanol (C2H,OH) and 0.810 M acetic acid (CH3COOH) are combined, what is the equilibrium concen- tration of ethyl acetate (CH3CO2C2Hs)? 6.816 2H,OH (aq) +CH,COOH(ag)CH,CO,C2Hs(ag) + H2O() 2. The KM for the decomposition of solid ammonium hydrogen sulfide to ammonia gas and hydrogen sulfide gas is 1.8 × 10-4 at 25°C. If ammonium hydrogen sulfide decomposes in...
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