PART A. Standardization of NaOH(aq) Calculate the molar mass of KHP from the molecular formula: __204.22 g/mol______________
Trial | Run 1 | Run 2 | |
Mass of KHP | 0.326g | 0.307g | 0.314g |
Calculate Moles of KHP | |||
Calculate Moles of NaOH needed for the reaction | |||
Initial volume of NaOH(aq) in mL | 11.30ml | 22.20ml | 25.20ml |
Final volume of NaOH(aq) in mL | 21.60ml | 31.60ml | 35.00ml |
Calculate the total volume of NaOH titrated in mL | |||
Convert the total volume of NaOH titrated into L | xxxx | ||
Calculate the concentration of NaOH in moles/L | xxxx |
Calculate the average molarity of NaOH (in mol/L): _____________
PART B. Acetic Acid Concentration in Vinegar:
Trial | Run 1 | Run 2 | |
Volume of vinegar in mL | 2.00ml | 2.00ml | 2.00ml |
Convert the volume of vinegar into L | xxxxx | ||
Initial volume of NaOH(aq) in mL | 12.50ml | 39.50ml | 35.60ml |
Final volume of NaOH(aq) in mL | 22.60ml | 49.80ml | 44.80ml |
Calculate the total volume of NaOH titrated in mL | |||
Convert the total volume of NaOH titrated into L | xxxxx | ||
Calculate the moles of NaOH (use the average M from part A) | xxxxx | ||
Calculate the concentration of vinegar in moles/L | xxxxx |
Calculate the average molarity of vinegar (in mol/L): _______________
Solution:- Part A) Run one: moles are calculated on dividing the moles by molar mass.
Run two:
Run three:
KHP and NaOH react in 1:1 mol ratio which is clear from the below balanced equation:
Since the mol ratio is 1:1, moles of NaOH will also be equivalent to the moles of KHP.
Run one:
Run two:
Run three:
Total Volume of NaOH used is the difference of final and initial volume readings.
Run one:- 21.60 mL - 11.30 mL = 10.30 mL
Run two: 31:60 mL - 22:20 mL = 9.40 mL
Run three:- 35.00 mL - 25.20 mL = 9.80 mL
Since, 1000 mL = 1 L
We divide the above volumes by 1000 to convert to L.
Run one:
Run two:
Run three:
To calculate the moles by Liters to get the molarity.
Run one:
Run two:
Run three:
Average molarity of NaOH =
Part B) For each rune, 2.00 mL of vinegar is used. To convert it to L, we will divide by 1000 same as we did above for NaOH.
so, 2.00/1000 = 0.00200 L
Hence, the volume will be 0.00200 L for each run.
NaOH volume is calculated by taking the difference of final and initial volumes same as we did above for part A.
run one: 22.60 mL - 12.50 mL = 10.1 mL = 0.0101 L
Run two: 49.80 mL - 39.50 mL = 10.3 mL = 0.0103 L
Run three: 44.80 mL - 35.60 mL = 9.20 mL = 0.00920 L
moles of NaOH used are calculated on multiplying the average molarity from part A and the volume in L.
Run one:
Run two:
Run three:
NaOH and vinegar react in 1:1 mol ratio as shown in the below equation:
Since the mole ratio is 1:1, moles of vinegar will be equivalent to the moles of NaOH. and we divide the moles by Liters to get the molarity.
Run one:
Run two:
Run three:
Average molarity of vinegar =
PART A. Standardization of NaOH(aq) Calculate the molar mass of KHP from the molecular formula: __204.22...
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 ml water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the exact number of moles of KHP that will react with...
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 ml water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the exact number of moles of KHP that will react with...
Part A: Standardization of NaOH Solution Data Table: Trial 1 Trial 2 Trial 3 Tared mass of KHP (g) 5065 -S168 so40 Molar mass of KHP (g/mol) 204.23 204.23 204.23 Moles of KHP (mol) Buret Reading:Initial Volume of NaOH (mL) .3 23. 2 나6.2. Buret Reading: Final Volume of NaOH (mL) Volume of NaOH dispensed (mL) Molar concentration of NaOH (mol/L) Average Molar concentration of NaOH 28.3 22.1 1145 O533 ces 3 (mol/L) Experiment: Volumetric Analvsis
I MAINLY NEED HELP ON TABLES PLS HELP THANK YOU Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC2H4O4, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 mL water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the...
1. A solution of sodium hydroxide (NaOH) was standardized against potassium hydrogen phthalate (KHP). A known mass of KHP was titrated with the NaOH solution until a light pink color appeared using phenolpthalein indicator. Using the volume of NaOH required to neutralize KHP and the number of moles of KHP titrated, the concentration of the NaOH solution was calculated. Molecular formula of Potassium hydrogen phthalate: HKC8H404 Mass of KHP used for standardization (g) 0.5100 Volume of NaOH required to neutralize...
STANDARDIZATION OF SOLUTIONS - Worksheet NaOH Volume (ml) Part I: Standardization of NaOH Trial KHP Mass (9) Potassium biphthalate 0.517 2 0.500 VE 0.51 0.71 27.00 27.20 Calculate the molarity of the NaOH solution:
A. Standardization of Sodium Hydroxide (NaOH) Solution Mass of bottle + KHP Mass of bottle Mass of KHP used Final buret reading Initial buret reading mL of NaOH used Molarity of NaOH Trial 1 1.3760 g 1.0369 g 0.2291 8 19.30 ml 4.90 mL 14.40 ml Trial 2 1.40458 1.0369 g 0.36768 35.60 mL 20.10 ml 15.50 ml Trial 3 1.39678 1.0369 g 0.3598 g 45.10 mL 30.10 ml 15.00 ml Average Molarity: Standard Deviation: Show your calculations for molarity...
Lab 11 Acid-Base Titration Part 2: Data Table for H2SO, titration HSO4 (aq) + 2 NaOH(aq) Table 3. Data + Sulfuric Acid Volume Na2SO. (aq) + 2 H2O(1) used - 10.00 m2 - Trial 1 Trial 2 Trial 3 (optional) H2SO4 used (A, B, C) Actual volume of H2SO4 (mL.) Initial buret reading (mL) Final buret reading (mL) 2.52mL 1.50mL 19.40mL 14.6ImL 31.42 m2 19.50ml Table 4. Results Calculations Trial 1 Trial 2 Trial 3 (optional) Volume of NaOH nitrated...
Objective 1: Standardization with KHP Trial 1 Mass of KHP Trial 2 Trial 3 ,5825 9 53539 1.53169 *Moles of KHP: Initial buret reading: 0.00 mL 10.00 Final buret reading: 0.00ML 8 mb 16.5 mL I 10.9 mL *Volume of NaOH solution used: 16.5 mL 8 mL 10.9mL *Molarity of NaOH solution: Show your calculations here: *Average Molarity of NaOH: Percent Range:
Observations: Part 1-Standardization of NaOH Ceho Trial 1 Trial 2 Trial 4 Trial 3 Initial mass weighing vial plus KHP と139 16908 427 IS 4 Final mass weighing vial plus KHP is.118 1s.YT 4.47 Mass of KHP Co 498 Moles of KHP used Moles NaOH used 0.00245% 10.00240円 10.00245 (4 SF) 062453 Initial burette reading of NaOH solution to +/-0.01 mL 00 100 0-00 T10 Final burctte rcading of NaOH solution 19.10 1f 03 02 23.00 to +-0.01 mL. Volume...