Homework Answers
| NH3 | H3O+ | NH4+ | |
| Before addition (moles) | 5*10-3 | 6*10-4 | 3.986*10-3 |
| addition (moles) | -6*10-4 | 0 | +6*10-4 |
| after addition (moles) | 4.4*10-3 | 0 | 4.586*10-3 |
molarity of ammonia in 50 mL ammonia buffer = 4.4*10-3 / (0.050) = 0.088 M
molarity of ammonium in 50 mL ammonia buffer = 4.586*10-3 / (0.050) = 0.09172 M
pH = 9.25 + log [NH3] / [NH4+]
pH = 9.25 + log (0.088 / 0.09172) = 9.232
Add Answer to:
PH of S0.0 mL acetate buffer+1.00 mL.0.6 M HC1 CH COO CH COOH H,0 before additionIO Addition -C.o...
Solve this last pH question on the page as well as fill in the boxes for...
Solve this last pH question on the page as well as fill in the
boxes for me given this information
Given :
SHOW ALL WORK: Calculations for Ammonia Buffer Solution a Moles of NH,CI in 250.0 mL ammonia buffer 3.491 ncid Molarity of NH.Cl in the ammonia buffer ? 32716 SSL Moles of NHs in 250.0 mL ammonia buffer 670 .00003 120 6 ? Molarity of NHs in ammonia buffer SHOW ALL WORK! pH Calculations (4 pts. for each blank...
Calculate the pH of 100.0 mL of a buffer that is 0.0800 M NH4Cl and 0.100 M NH 3 before and after the addition of 1.00...
Calculate the pH of 100.0 mL of a buffer that is 0.0800 M NH4Cl and 0.100 M NH 3 before and after the addition of 1.00 mL of 5.25 M HNO3- 1st attempt Part 1 (0.5 point) M See Periodic Table See = pH before Part 2 (0.5 point) = pH after
You are given 75 mL of 0.70 M acetic acid/acetate buffer to test. The starting composition...
You are given 75 mL of 0.70 M acetic acid/acetate buffer to test. The starting composition of the two major species are: Concentration of CH,COOH: 0.250 M Concentration of CH,COO: 0.450 M a. Calculate the initial pH of the buffer. Clearly show all work required to arrive at your answer. b. You add 1.0 mL of 2.00 M HCl to the buffer. Calculate the molarity of H, O' added as HCl, and the final molarities of acetic acid and acetate...
Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.230 M pyridine, C5H5N(aq) with 0.230 M HBr(aq) Number 9.3 (a) before addition of any HBr Number 5.23 (b) after additi...
Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.230 M pyridine, C5H5N(aq) with 0.230 M HBr(aq) Number 9.3 (a) before addition of any HBr Number 5.23 (b) after addition of 12.5 mL of HBr With equal concentrations of monoprotic titrant and added volumes are equal (25.0 mL of HBr added) So at point (c), we are 24.0/50.0 = 96.0% of the way to umber analyte, the equivalence point would occur when the...
Check my work Be sure to answer all parts. Report pro Hint Calculate the pH of 1.00 L of the buffer 1.03 M CH,COONa...
Check my work Be sure to answer all parts. Report pro Hint Calculate the pH of 1.00 L of the buffer 1.03 M CH,COONa/0.96 M CH,COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: (b) pH after addition of 0.070 mol NaOH: (e) pH after further addition of 0.100 mol HCI: < Prev 11 of 22 Next >
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH...
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH of this solution. 50.0 mL buffer + 2.0mLION NAOH pH 2. Measured pH of this solution. pH 4.59 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error pH of Buffer after the addition of the Strong Base: ix. Measure out 50.0 ml the buffer in part D and 2.0...
A 41.0-mL sample of 0.217 M CH, COOH solution is titrated with 0.176 M N OH....
A 41.0-mL sample of 0.217 M CH, COOH solution is titrated with 0.176 M N OH. Calculate the pH of the solution (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a before the addition of any NeOH solution pH = b after the addition of 14.3 mL of NeOH solution pH =...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity t...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity to be higher, lower, or the same as the buffer you prepared in Part II of this lab? Be specific and use your data. c. Measure the pH of the Beaker #2 solution, via a pH meter, and record in data sheet. Part II: Dilute Buffer Solution In this section, the pH of a 0.25 M CH3CO2H - 0.25...
Question two A buffer solution is able to maintain a constant pH when small amounts of...
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
I added everything thing. this is the lab question you need to solve. First assigned buffer...
I added everything thing.
this is the lab question you need to solve.
First assigned buffer pH: 2.031 Second assigned buffer pH: 9.171 Available Buffer Systems (acid/ base) pka of Conjugate Acid 2.847 4.757 malonic acid/ monosodium malonate acetic acid/ sodium acetate ammonium chloride/ ammonia triethylammonium chloride/ triethylamine 9.244 10.715 1) Buffer system details: Given pH Name and volume conjugate acid Name and volume conjugate base 2) Calculations for preparation of high capacity buffer system. Introduction In this experiment, you...
Solve this last pH question on the page as well as fill in the
boxes for me given this information
Given :
SHOW ALL WORK: Calculations for Ammonia Buffer Solution a Moles of NH,CI in 250.0 mL ammonia buffer 3.491 ncid Molarity of NH.Cl in the ammonia buffer ? 32716 SSL Moles of NHs in 250.0 mL ammonia buffer 670 .00003 120 6 ? Molarity of NHs in ammonia buffer SHOW ALL WORK! pH Calculations (4 pts. for each blank...
Calculate the pH of 100.0 mL of a buffer that is 0.0800 M NH4Cl and 0.100 M NH 3 before and after the addition of 1.00 mL of 5.25 M HNO3- 1st attempt Part 1 (0.5 point) M See Periodic Table See = pH before Part 2 (0.5 point) = pH after
You are given 75 mL of 0.70 M acetic acid/acetate buffer to test. The starting composition of the two major species are: Concentration of CH,COOH: 0.250 M Concentration of CH,COO: 0.450 M a. Calculate the initial pH of the buffer. Clearly show all work required to arrive at your answer. b. You add 1.0 mL of 2.00 M HCl to the buffer. Calculate the molarity of H, O' added as HCl, and the final molarities of acetic acid and acetate...
Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.230 M pyridine, C5H5N(aq) with 0.230 M HBr(aq) Number 9.3 (a) before addition of any HBr Number 5.23 (b) after addition of 12.5 mL of HBr With equal concentrations of monoprotic titrant and added volumes are equal (25.0 mL of HBr added) So at point (c), we are 24.0/50.0 = 96.0% of the way to umber analyte, the equivalence point would occur when the...
Check my work Be sure to answer all parts. Report pro Hint Calculate the pH of 1.00 L of the buffer 1.03 M CH,COONa/0.96 M CH,COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: (b) pH after addition of 0.070 mol NaOH: (e) pH after further addition of 0.100 mol HCI: < Prev 11 of 22 Next >
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH of this solution. 50.0 mL buffer + 2.0mLION NAOH pH 2. Measured pH of this solution. pH 4.59 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error pH of Buffer after the addition of the Strong Base: ix. Measure out 50.0 ml the buffer in part D and 2.0...
A 41.0-mL sample of 0.217 M CH, COOH solution is titrated with 0.176 M N OH. Calculate the pH of the solution (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a before the addition of any NeOH solution pH = b after the addition of 14.3 mL of NeOH solution pH =...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity to be higher, lower, or the same as the buffer you prepared in Part II of this lab? Be specific and use your data. c. Measure the pH of the Beaker #2 solution, via a pH meter, and record in data sheet. Part II: Dilute Buffer Solution In this section, the pH of a 0.25 M CH3CO2H - 0.25...
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
I added everything thing.
this is the lab question you need to solve.
First assigned buffer pH: 2.031 Second assigned buffer pH: 9.171 Available Buffer Systems (acid/ base) pka of Conjugate Acid 2.847 4.757 malonic acid/ monosodium malonate acetic acid/ sodium acetate ammonium chloride/ ammonia triethylammonium chloride/ triethylamine 9.244 10.715 1) Buffer system details: Given pH Name and volume conjugate acid Name and volume conjugate base 2) Calculations for preparation of high capacity buffer system. Introduction In this experiment, you...
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