Need help with these 2 questions.
Homework Answers
![to find pH, we will use Henderson - Hasselbalch egr pH a pk [salt] [and] since ka= 4,6x104 pka= -log ka = -log to 6 x 10 a =](http://img.homeworklib.com/questions/40365ad0-df69-11eb-9a89-cbc967fd09a9.png?x-oss-process=image/resize,w_560)
Hope it helps...pls do upvote
Add Answer to:
Need help with these 2 questions.
What will happen if we increase the temperature in the...
Need help on questions 1-3 Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka...
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
Needing help answering these two questions. Thank you What will happen to the reaction equilibrium if...
Needing help answering these two questions. Thank
you
What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(g) + 2 HI(g) Calculate the pH of the solution obtained by titrating 40 ml of 0.35 M HNO2(aq) with 0.4 M NaOH(aq) to the equivalence point. Take K = 4.6x10 M.
(Set 2) Practice Problems in Equilibrium All weak acids use this generic equation: HA(aq)+ H2O() A (aq) + H30*(aq) And...
(Set 2) Practice Problems in Equilibrium All weak acids use this generic equation: HA(aq)+ H2O() A (aq) + H30*(aq) And all weak bases use this one: B(aq)+ H2O(I) = BH*(aq)+ OH'(aq) Part A: Finding K, or Kb 3.012? What is the value of Ka for a weak acid if a 1.44 M solution has a pH 1. 2. A weak acid is 0.00987 M, but is found to be 25.5 % ionized. What is the pH? 3. The pH for...
2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H3O+ + NO2 (aq) 3. What will...
2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H3O+ + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) > 2 HI(g)
8. What is the pH of a 5.00 x 102 M Ba(OH)2(aq) solution at room temperature?...
8. What is the pH of a 5.00 x 102 M Ba(OH)2(aq) solution at room temperature? a. 1.00 b. 1.30 c. 12.02 d. 12.70 e. 13.00 9. Assuming equal concentrations of conjugate acid and base, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8? a. CH3COONa/CH3COOH (K = 1.8 x 105) b. NH/NHACI (K = 5.6 x 10-1) c. NaOCI/HOCI (Ka = 3.2 x 108) d. NaNO2/HNO2 (Ka = 4.5...
At a particular temperature, K = 5.7 ✕ 10−6 for the following reaction. 2 CO2(g) 2...
At a particular temperature, K = 5.7 ✕ 10−6
for the following reaction.
2 CO2(g) 2
CO(g) + O2(g)
If 2.9 moles of CO2 is initially placed into a 4.6-L
vessel, calculate the equilibrium concentrations of all
species.
How do you do these problems? I got all of them wrong and don't understand why....
How do you do these problems? I got all of them wrong and
don't understand why.
- 10. Which of the changes will increase the value of K, for the reaction? 2 SO2(g) + O2(g) - 2 SO3(g) AH = -200 kJ/mol A. Lowering the temperature B. Increasing the pressure (CCAdding 02 D. Removing SO, 3. Which reaction describes why the pH is not 7 for the dissolution of NaNO2 in water? ADNa+ + 2 H2O = NaOH + H2O*...
Part 1.) Calculate the pH of each of the following strong acid solutions. (a) 0.00555 M...
Part 1.)
Calculate the pH of each of the following strong acid
solutions.
(a) 0.00555 M HClO4
pH =
(b) 0.314 g of HBrO4 in 21.0 L of solution
pH =
(c) 39.0 mL of 3.50 M HClO4 diluted to 1.90 L
pH =
(d) a mixture formed by adding 59.0 mL of 0.00582 M
HClO4 to 16.0 mL of 0.00676 M HBrO4
pH =
Part 2.)
Using values from Appendix C of your textbook, calculate the
value of Keq...
help with these chemistry questions 1. Explain what happens to the concentration of H,O' ions in...
help with these chemistry questions
1. Explain what happens to the concentration of H,O' ions in an acetic acid solution when solid sodium acetate is added. 2. Determine the pH and pH of a solution that is 0.5 M NaHSO4 and 0.25 M Na2SO4 3. When sodium nitrite is added to HNO2(aq) a) the equilibrium concentration of HCOOH(aq) decreases. b) the pH of the solution increases. c) the K increases. d) the pH of the solution does not change. e)...
Hello i need help with this, thank you s Principle [References) At a particular temperature, K...
Hello i need help with this, thank you
s Principle [References) At a particular temperature, K = 7.0 x 10-6 for the reaction 2 CO2(g) = 2 CO(g) + O2(g) If 4.0 moles of CO2 is initially placed into a 5.0-L vessel, calculate the equilibrium concentrations of all species. (CO2) = (CO) = [02] = Submit Answer Try Another Version 9 item attempts remaining
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
Needing help answering these two questions. Thank
you
What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(g) + 2 HI(g) Calculate the pH of the solution obtained by titrating 40 ml of 0.35 M HNO2(aq) with 0.4 M NaOH(aq) to the equivalence point. Take K = 4.6x10 M.
(Set 2) Practice Problems in Equilibrium All weak acids use this generic equation: HA(aq)+ H2O() A (aq) + H30*(aq) And all weak bases use this one: B(aq)+ H2O(I) = BH*(aq)+ OH'(aq) Part A: Finding K, or Kb 3.012? What is the value of Ka for a weak acid if a 1.44 M solution has a pH 1. 2. A weak acid is 0.00987 M, but is found to be 25.5 % ionized. What is the pH? 3. The pH for...
2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H3O+ + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) > 2 HI(g)
8. What is the pH of a 5.00 x 102 M Ba(OH)2(aq) solution at room temperature? a. 1.00 b. 1.30 c. 12.02 d. 12.70 e. 13.00 9. Assuming equal concentrations of conjugate acid and base, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8? a. CH3COONa/CH3COOH (K = 1.8 x 105) b. NH/NHACI (K = 5.6 x 10-1) c. NaOCI/HOCI (Ka = 3.2 x 108) d. NaNO2/HNO2 (Ka = 4.5...
At a particular temperature, K = 5.7 ✕ 10−6
for the following reaction.
2 CO2(g) 2
CO(g) + O2(g)
If 2.9 moles of CO2 is initially placed into a 4.6-L
vessel, calculate the equilibrium concentrations of all
species.
How do you do these problems? I got all of them wrong and
don't understand why.
- 10. Which of the changes will increase the value of K, for the reaction? 2 SO2(g) + O2(g) - 2 SO3(g) AH = -200 kJ/mol A. Lowering the temperature B. Increasing the pressure (CCAdding 02 D. Removing SO, 3. Which reaction describes why the pH is not 7 for the dissolution of NaNO2 in water? ADNa+ + 2 H2O = NaOH + H2O*...
Part 1.)
Calculate the pH of each of the following strong acid
solutions.
(a) 0.00555 M HClO4
pH =
(b) 0.314 g of HBrO4 in 21.0 L of solution
pH =
(c) 39.0 mL of 3.50 M HClO4 diluted to 1.90 L
pH =
(d) a mixture formed by adding 59.0 mL of 0.00582 M
HClO4 to 16.0 mL of 0.00676 M HBrO4
pH =
Part 2.)
Using values from Appendix C of your textbook, calculate the
value of Keq...
help with these chemistry questions
1. Explain what happens to the concentration of H,O' ions in an acetic acid solution when solid sodium acetate is added. 2. Determine the pH and pH of a solution that is 0.5 M NaHSO4 and 0.25 M Na2SO4 3. When sodium nitrite is added to HNO2(aq) a) the equilibrium concentration of HCOOH(aq) decreases. b) the pH of the solution increases. c) the K increases. d) the pH of the solution does not change. e)...
Hello i need help with this, thank you
s Principle [References) At a particular temperature, K = 7.0 x 10-6 for the reaction 2 CO2(g) = 2 CO(g) + O2(g) If 4.0 moles of CO2 is initially placed into a 5.0-L vessel, calculate the equilibrium concentrations of all species. (CO2) = (CO) = [02] = Submit Answer Try Another Version 9 item attempts remaining
Most questions answered within 3 hours.
-
Where is the error in this code sequence?
String s1 = "Hello";
String s2 = "ello";...
asked 10 months ago -
Financial data for Joel de Paris, Inc., for last year
follow:
Joel de Paris, Inc.
Balance...
asked 10 months ago -
Consider this reaction:
Al2(SO4)3 (aq)+ BaCl3
(aq) Al2Cl6 (aq)- +
3BaSO4(s) . What is the...
asked 10 months ago -
Suppose that Savneet is considering increasing her
recent random sample from 20 car rentals to 40...
asked 10 months ago -
Trucks arrive at an unloading terminal at an average rate of 120
per hour.
Trucks arrive...
asked 10 months ago -
Why are methanol and ethanol completely soluble in water while
octanol is not very little soluble....
asked 10 months ago -
A facilities manager at a university reads in a research report
that the mean amount of...
asked 10 months ago -
When the CuSO4 is rehydrated by adding water to the anhydrous
compound, is this an endothermic...
asked 10 months ago -
A ray of sunlight is passing from diamond into crown glass; the
angle of incidence is...
asked 10 months ago -
A block of mass 0.249 kg is placed on top of a light, vertical
spring of...
asked 10 months ago -
how do the kidneys compensate in the presences of acidosis
a) trigger hyperventilate
b) reserve acid...
asked 10 months ago -
Question 501 pts
The rental rate of capital to the firm increases. Which of the
following...
asked 10 months ago