EXPT 5 HYDROLYSIS OF SALTS Use Ph to calulate H+ and OH- SOLUTION Measured pH Calculated...
EXPT 5 HYDROLYSIS OF SALTS
Use Ph to calulate H+ and OH-
|
SOLUTION |
Measured pH |
Calculated [H+] |
Calculated [OH-] |
|
H2O(boiled) |
7 |
||
|
0.1M NaCl |
7 |
||
|
0.1M Na2CO3 |
13 |
||
|
0.1M NaC2H3O2 |
8.8 |
||
|
0.1M NH4Cl |
4.6 |
||
|
0.1M Al(NO3)3 |
4 |
||
|
0.1M ZnCl2 |
5 |
||
|
0.1M KAl(SO4)2 |
4 |
Homework Answers
![كنند PHL is - negative log: Of H+ ion concentration j.e. PHE -log [ht] . log CH) = -2 :. [H+] = 10^-PH 101PH Malso, piscale](http://img.homeworklib.com/questions/e8628d00-899b-11eb-9f44-85f23172893a.png?x-oss-process=image/resize,w_560)
![Solution Measured pH calculated calculated [47] [04] H20 (boiled) 1 x 10-7M 1x 167M 2 0.1 M Nach 1 x 107M 1x10-7M Na2CO3 13 1](http://img.homeworklib.com/questions/e9392880-899b-11eb-82be-3189eb269c1d.png?x-oss-process=image/resize,w_560)
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EXPT 5 HYDROLYSIS OF SALTS
Use Ph to calulate H+ and OH-
SOLUTION
Measured pH
Calculated...
I need help with number 9 please 9. Using the experimental data for pH and the...
I
need help with number 9 please
9. Using the experimental data for pH and the concentration of the solutions, calculate the K, and Ky for each salt. (SHOW YOUR WORK.) Solution Value of K, or Kb 0.1 ZnCl2 0.1 KAl(SO4)2 0.1 NHACI 0.1 NaC2H302 Value of K, or Kb Solution 0.1 Na2CO3 Part B. Buffer solutions and pH 10. Mass of NaC2H307-3H203.316 11. Measured pH of original buffer solution 4 0 12. Measured pH of buffer + HCI_4.2 13....
pH- Solution [HⓇ]/M* [OH J/M** Wide Range Narrow Range Paper Acidic, basic or neutral H20 (unboiled)...
pH- Solution [HⓇ]/M* [OH J/M** Wide Range Narrow Range Paper Acidic, basic or neutral H20 (unboiled) H20 (boiled) NaCl a Motoci NaAc NH4Cl 5.0 acidic 5.0 acidic 5.0 acidic 6.5 acidic 9 4.5 acidic 7 5.0 acidic 12.5 basic 12.5 basic ZnCl2 KAI(SO4)2 Na2CO3 1 14 *From narrow range pH value. Use [H"] = 10: Usde K, = Use [H (OH) = 1.0 x 10
4-l0.2 Solution 8 10.0 mL of solution 5 + find the limiting reager Calculated pH h...
4-l0.2 Solution 8 10.0 mL of solution 5 + find the limiting reager Calculated pH h Measure 4 (hint-calculate the number of moles o and log On 0006 200 fo.0000 C000s +0000 Should the pH of a buffer change when large quantity of base is added?e Why? Butter is o imitins feasant. ph Should to The Cicnse tue cecid MaRe tue 4. Calculate the pH of the following solutions. Compare these values with the experimental values obtained for Solutions 9...
I know some of the measured pH values are a little off due to error in...
I
know some of the measured pH values are a little off due to error
in the lab, but I need help filling out the “Ion Hydrolyzed” table
and then the “Net Ionic Equation” part. I remember doing net ionic
equations in General Chemistry I, bit don’t see how it applies
here.
Thanks, in advance! (i will rate!)
Learning Objectives: 1. To test the acidic and basic properties of ionic compounds. 2. To create a buffer solution and calculate its...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e)...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e) HSO (d) F (b) Н:0" 6, Use Table 15.2 (page 529) to decide whether the species on the left or those on the right are favored by the reaction. a. NH4 (aq) + H2PO4" (aq) # NH3(aq) + HsPO b. HCN (aq) + HS(aq) CN" (aq) +H2S c. HCO +OH CO2 H2S d. Al(H20)6 3+ +OH = Al(H20) s2+ OH 7. The equilibrium constant...
61.8% Tools F 8. Sign 0.1 molar NH4Cl solution 20. Identify the acid and base which...
61.8% Tools F 8. Sign 0.1 molar NH4Cl solution 20. Identify the acid and base which reacted to form NH CI Identify each as strong or weak. Acid: Strength: Base: Strength 21. Calculate the theoretical pH of the solution. Show your work. If appropriate, write out the hydrolysis reaction equation. 22. Calculate the theoretical Kh value. 23. Measure the pH of the aqueous solution and determine the expenmental K. Show your work. pH of solution Experimental K. 24. How does...
This is from a Study of Buffer Solutions and pH of Salt Solutions Lab. I calculated...
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
1. Which of the followi ch of the following reactions is not readily explained by the...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids a...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
I
need help with number 9 please
9. Using the experimental data for pH and the concentration of the solutions, calculate the K, and Ky for each salt. (SHOW YOUR WORK.) Solution Value of K, or Kb 0.1 ZnCl2 0.1 KAl(SO4)2 0.1 NHACI 0.1 NaC2H302 Value of K, or Kb Solution 0.1 Na2CO3 Part B. Buffer solutions and pH 10. Mass of NaC2H307-3H203.316 11. Measured pH of original buffer solution 4 0 12. Measured pH of buffer + HCI_4.2 13....
pH- Solution [HⓇ]/M* [OH J/M** Wide Range Narrow Range Paper Acidic, basic or neutral H20 (unboiled) H20 (boiled) NaCl a Motoci NaAc NH4Cl 5.0 acidic 5.0 acidic 5.0 acidic 6.5 acidic 9 4.5 acidic 7 5.0 acidic 12.5 basic 12.5 basic ZnCl2 KAI(SO4)2 Na2CO3 1 14 *From narrow range pH value. Use [H"] = 10: Usde K, = Use [H (OH) = 1.0 x 10
4-l0.2 Solution 8 10.0 mL of solution 5 + find the limiting reager Calculated pH h Measure 4 (hint-calculate the number of moles o and log On 0006 200 fo.0000 C000s +0000 Should the pH of a buffer change when large quantity of base is added?e Why? Butter is o imitins feasant. ph Should to The Cicnse tue cecid MaRe tue 4. Calculate the pH of the following solutions. Compare these values with the experimental values obtained for Solutions 9...
I
know some of the measured pH values are a little off due to error
in the lab, but I need help filling out the “Ion Hydrolyzed” table
and then the “Net Ionic Equation” part. I remember doing net ionic
equations in General Chemistry I, bit don’t see how it applies
here.
Thanks, in advance! (i will rate!)
Learning Objectives: 1. To test the acidic and basic properties of ionic compounds. 2. To create a buffer solution and calculate its...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e) HSO (d) F (b) Н:0" 6, Use Table 15.2 (page 529) to decide whether the species on the left or those on the right are favored by the reaction. a. NH4 (aq) + H2PO4" (aq) # NH3(aq) + HsPO b. HCN (aq) + HS(aq) CN" (aq) +H2S c. HCO +OH CO2 H2S d. Al(H20)6 3+ +OH = Al(H20) s2+ OH 7. The equilibrium constant...
61.8% Tools F 8. Sign 0.1 molar NH4Cl solution 20. Identify the acid and base which reacted to form NH CI Identify each as strong or weak. Acid: Strength: Base: Strength 21. Calculate the theoretical pH of the solution. Show your work. If appropriate, write out the hydrolysis reaction equation. 22. Calculate the theoretical Kh value. 23. Measure the pH of the aqueous solution and determine the expenmental K. Show your work. pH of solution Experimental K. 24. How does...
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
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