When 10.00 mL of 0.240 M HX (Ka = 4.31 10-5) is titrated with 0.120 M...
When 10.00 mL of 0.240 M HX (Ka = 4.31
10-5)
is titrated with 0.120 M KOH, the pH will increase. Calculate the
pH of the solution at each point in the titration. The
pKw is 14.000 at this temperature.
| Volume of KOH (mL) | pH |
|---|---|
| 0.00 | |
| 2.00 | |
| 4.00 | |
| 6.00 | |
| 8.00 | |
| 10.00 | |
| 12.00 | |
| 14.00 | |
| 16.00 | |
| 18.00 | |
| 20.00 | |
| 22.00 | |
| 24.00 | |
| 26.00 | |
| 28.00 |
Homework Answers
![6.24 M . [salt] e solution 10ml w HX + KOH KX + H₂O 2.4 milindes 0.12M So where Untill 20 ml of kon is added there will be we](http://img.homeworklib.com/questions/4590acc0-c957-11eb-b21b-15a17c088587.png?x-oss-process=image/resize,w_560)
![volume tme) • 10 pn = 4.36 + log [1:2] • 12 → pu- 4.36 + lug [1.44] = 4.536 To:96] 1.14 P 1.16 . 18 - ph = 4.36 + log [ 1.68]](http://img.homeworklib.com/questions/463d6570-c957-11eb-bac7-f5506fb2d032.png?x-oss-process=image/resize,w_560)
![volume 24 aml of Nokon o left [ou] = ruxo 127 = opona -log(48012] ч РИs - go 12.15 - 1.85 86 %) Гбх6-12-12 fоr -- т с ко - (](http://img.homeworklib.com/questions/46f38b30-c957-11eb-b947-0949fcb4a753.png?x-oss-process=image/resize,w_560)
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When 10.00 mL of 0.240 M HX (Ka = 4.31
10-5)
is titrated with 0.120 M...
When 10.00 mL of 0.240 M HX (Ka = 2.29 x 10') is titrated with 0.120...
When 10.00 mL of 0.240 M HX (Ka = 2.29 x 10') is titrated with 0.120 M KOH, the pH will increase. Calculate the pH of the solution at each point in the titration. The pkw is 14.000 at this temperature. pH Volume of KOH (mL) 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 26.00 28.00
Following the Procedure of this experiment, a student titrated 0.653 g of an unknown weak, monoprotic...
Following the Procedure of this experiment, a student titrated 0.653 g of an unknown weak, monoprotic acid with 0.100 M NaOH and monitored the titration with a pH meter. His titration data were: Volume of NaOH solution added, mL /// pH 0.00 | 3.30 2.00 | 4.22 4.00 | 4.55 6.00 | 4.76 8.00 | 4.92 10.00 | 5.06 12.00 | 5.18 14.00 | 5.29 16.00 | 5.40 18.00 | 5.51 20.00 | 5.62 22.00 | 5.74 24.00 | 5.88...
1) A student titrated 20.0 mL of 0.410 M HCl with 0.320 M NaOH and collected...
1) A student titrated 20.0 mL of 0.410 M HCl with 0.320 M NaOH and collected the following data: Number V of NaOH solution added, mL PH # V of NaOH added, mL PH 1 0.00 .39 12 22.00 1.56 2 2.00 .46 13 24.00 1.93 3 4.00 .54 14 24.50 2.09 4 6.00 .62 15 25.00 2.35 5 8.00 .70 16 25.50 3.06 6 10.00 .78 17 26.00 11.40 7 12.00 .87 18 26.50 11.80 8 14.00 .96 19...
Monitosing.Acid-Base Titrations wih a pH Meter 3. student titrated 20.0 mL of 0.410M HCI with 0.320M...
Monitosing.Acid-Base Titrations wih a pH Meter 3. student titrated 20.0 mL of 0.410M HCI with 0.320M NaOH and collected the following data. Pre-Laboratory Assignment 1. Briefly explain: (a) why you must use caution when with HCI solutions 0.32 A working volume NaOH solution added, mLpH 0.39 0.46 0.54 0.62 0.70 0.78 0.87 0.96 1.07 1.19 1.35 1.56 1.93 2.09 2.35 3.06 11.40 11.80 12.00 12.20 12.30 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 24.50...
please help with question 3 part b on the first picture? please step by step explain...
please help with question 3 part b on the first picture?
please step by step explain thank you
he leo the acid 3. Following the Procedure of this experiment, a student monoprotic acid with 0.100M NaOH and monitored the titration with a pH meter. His titration titrated 0.653 g of an unknown weak, monoprotic acid with data were: volume of NaOH solution added, mL volume of NaOH solution added, mL pH 0.00 2.00 4.00 6.00 3.30 22.00 24.00 26.00 28.00...
wame S tation Date CHM 112 - Acid-Base Titration using pH Sensor Pre-lab Questions 1. Calculate...
wame S tation Date CHM 112 - Acid-Base Titration using pH Sensor Pre-lab Questions 1. Calculate [H,O') and JOH) in solutions of the following pls. [H30") (OH) PH 4.18 5.70 8.56 2. A student titrated 20.00 mL of 0.410 M HCl with 0.320 M NaOH and collected the following data. Volume NaOH added, mL 0.00 0.39 0.46 4.00 0.54 6.00 0.62 8.00 0.70 10.00 0.78 12.00 0.87 14.00 0.96 16.00 1.07 18.00 20.00 1.35 22.00 1.56 24.00 1.93 24.50 2.09...
A 42.0 mL sample of 0.120 M HNO2 is titrated with 0.214 M KOH. (Ka for...
A 42.0 mL sample of 0.120 M HNO2 is titrated with 0.214 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH.
pH be at the equivalence point? Volume NaOH added pH 0.39 The student collected the following...
pH be at the equivalence point? Volume NaOH added pH 0.39 The student collected the following data: Plot the data above in excel with pH values on the Y axis and the volume of NaOH added on the X axis Graphically determine the equivalence point and indicate the pH on the graph. b. 0.00 2.00 4.00 0.46 0.54 ii. 0.62 6.00 8.00 10.00 0.7 0.78 Show the following calculations on a separate sheet of paper: 0.87 12.00 0.96 1.07 14.00...
A 20.00-mL solution of 0.120 M nitrous acid (Ka = 4.0 × 10–4) is titrated with...
A 20.00-mL solution of 0.120 M nitrous acid (Ka = 4.0 × 10–4) is titrated with a 0.215 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution at the equivalence point of titration? (if needed: Kw = 1.00 × 10–14)
Hydrofluoric acid has a Ka of 6.8 x 10-4. In this titration, 20.00 mL of 0.120...
Hydrofluoric acid has a Ka of 6.8 x 10-4. In this titration, 20.00 mL of 0.120 MHF is titrated against 0.080 M KOH. Calculate the pH when 40.00 mL of base has been added. 12.12 O 7.88 12.73 12.41
When 10.00 mL of 0.240 M HX (Ka = 2.29 x 10') is titrated with 0.120 M KOH, the pH will increase. Calculate the pH of the solution at each point in the titration. The pkw is 14.000 at this temperature. pH Volume of KOH (mL) 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 26.00 28.00
Monitosing.Acid-Base Titrations wih a pH Meter 3. student titrated 20.0 mL of 0.410M HCI with 0.320M NaOH and collected the following data. Pre-Laboratory Assignment 1. Briefly explain: (a) why you must use caution when with HCI solutions 0.32 A working volume NaOH solution added, mLpH 0.39 0.46 0.54 0.62 0.70 0.78 0.87 0.96 1.07 1.19 1.35 1.56 1.93 2.09 2.35 3.06 11.40 11.80 12.00 12.20 12.30 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 24.50...
please help with question 3 part b on the first picture?
please step by step explain thank you
he leo the acid 3. Following the Procedure of this experiment, a student monoprotic acid with 0.100M NaOH and monitored the titration with a pH meter. His titration titrated 0.653 g of an unknown weak, monoprotic acid with data were: volume of NaOH solution added, mL volume of NaOH solution added, mL pH 0.00 2.00 4.00 6.00 3.30 22.00 24.00 26.00 28.00...
wame S tation Date CHM 112 - Acid-Base Titration using pH Sensor Pre-lab Questions 1. Calculate [H,O') and JOH) in solutions of the following pls. [H30") (OH) PH 4.18 5.70 8.56 2. A student titrated 20.00 mL of 0.410 M HCl with 0.320 M NaOH and collected the following data. Volume NaOH added, mL 0.00 0.39 0.46 4.00 0.54 6.00 0.62 8.00 0.70 10.00 0.78 12.00 0.87 14.00 0.96 16.00 1.07 18.00 20.00 1.35 22.00 1.56 24.00 1.93 24.50 2.09...
pH be at the equivalence point? Volume NaOH added pH 0.39 The student collected the following data: Plot the data above in excel with pH values on the Y axis and the volume of NaOH added on the X axis Graphically determine the equivalence point and indicate the pH on the graph. b. 0.00 2.00 4.00 0.46 0.54 ii. 0.62 6.00 8.00 10.00 0.7 0.78 Show the following calculations on a separate sheet of paper: 0.87 12.00 0.96 1.07 14.00...
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