Lab 6

Table 1. Titration data   Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48   1.89   1.95   Molarity of NaOH (M) 0.100   0.100   0.100   Volume of vinegar sample (mL) 5.00   5.00   5.00   Final burette reading (mL) 49.32   49.06   49.93   Table 2. Titration data Table view     List view Table 2. Titration data   Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48   1.89   1.95   Molarity of NaOH (M) 0.100   0.100   0.100   Volume of vinegar sample (mL) 5.00   5.00   5.00   Final burette reading (mL) 49.32   49.06   49.93   Expected color at end point Choose...     Choose...     Choose...     Volume of NaOH used (mL)             1. Average Volume of NaOH used in liters 2. Average moles of NaOH used (mol)   3. Average moles of acetic acid (mol)   4. Average molarity of acetic acid (M)   5. Average mass of acetic acid (g)…

Can y'all help me finish solving my calculations please

The molarity of HC2H3O2, M for trail 1,2,3.

Pre Lab Questions: (Each answer is to be written as a complete sentence) What is the reason for washing the precipitate with water in Step 9? Define precipitate. Define filtrate. In Step 2, what is the purpose for rinsing the stirring rod? read the Procedure to answer the questions  Using a balance, mass between 1.50 – 2.00 grams of sodium carbonate in a pre-massed 150mL beaker. Add 20 mL of distilled water and stir thoroughly to make sure all the crystals are dissolved. Rinse the stirring rod with a little distilled water after stirring. Using a balance, mass between 1.50 – 2.00 grams of calcium chloride dihydrate in a pre-massed 50 mL beaker. Repeat Step 2 for the solution in the 50 mL beaker. Pour the calcium chloride solution into the 150mL beaker containing the sodium carbonate solution and stir. Mass a piece of filter paper. Fold the filter paper and place it into the funnel. Wet it with a little distilled water to ensure that it is stuck to the sides of the funnel. Slowly…

3. Titration: Strong Acid / Weak Base. (I warned you to be ready!) Here's the cool chart! Analyte: 20.00 mL 0.100 M Hydrazine (N₂H4) Hd A: initial Vertical (Value) Axis Title 0 B: half equivalence C: equivalence 5 10 15 20 Titrant: mL of 0.100 M HCI added 25 20.00 mL of 0.100 M hydrazine (N₂H4, pKb = 5.77) is titrated with 0.100 M HCl. a) Find the initial pH (point A) and the pH at the equivalence point (point C). b) Find the pH at the half equivalence point (point B).

Please send me the question in 20 minutes it's very urgent plz

help please answer in text form with proper working and explanation for each and every part and steps with concept and introduction no ai no copy paste remember answer must be in proper format with all working

d) please see attached question concentration KOH=20.8325mL pH solution=2.9 beginning of the titration, Vbase = 0.00 mL

Table 2. Titration data   Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19   2.26   2.39   Molarity of NaOH (M) 0.100   0.100   0.100   Volume of vinegar sample (mL) 5.00   5.00   5.00   Final burette reading (mL) 48.55   49.43   49.99   Expected color at end point             Volume of NaOH used (mL)           Average Volume of NaOH used in liters   Average moles of NaOH used (mol)   Average moles of acetic acid (mol)   Average molarity of acetic acid (M)     Average mass of acetic acid (g)   Average mass of vinegar (g) (assume the density of vinegar is 1.00 g/mL)   Average mass % of acetic acid in vinegar   Known mass % of acetic acid in vinegar is 5.45%   Percent Error

based on the data tables provided, what is % CH3COOH in vinegar

Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution  II. Wash the burette with a standardized solution III. Fill the burette to the 50-mL mark IV. Prepare a contrast paper to determine burette volume and titration endpoint

Help please!

Label as KHTar in .01M KCl. Add approximately 100 mL of .01 M KCl and 2 grams of KHTar Solve for [HTar] and amount used.

Please help with explanation. (Gpt/Ai wrong answer not allowed)

0.2061 grams of an unknown organic acid was dissolved in about 50 mL of water in a 250 mL Erlenmeyer flask and titrated against 0.1000 M NaOH solution using bromothymol blue indicator. 15.56 mL of titrant was used to achieve end point. Calculate the Neutralization Equivalent. Write answer with two decimal places only. No units please.

both I and III II only QUESTION 5 In the experiment "Preparation and Standardization of a Sodium Hydroxide Solution", why was the burette rinsed with NAOH before filling it to "zero" for the titration? To remove any residual liquids from the burette To check that the burette works properly To remove any air bubbles and fill the tip of the burette All of the above QUESTION 6 Sav Click Save and Submit to save and submit. Click Save All Answers to save all answers.

Calculate the Molarity

Which product contains a strong base that would most likely completely dissolve in water? O drain cleaner ammonia baking soda antacid Next Save and Exit Mark this and return .com/ContentViewers/AssessmentViewer/Activit.

1. Prepare 50-mL of a 50 mM H,PO, solution in a 50-ml conical tube. Molar mass of NaH2PO4 H2O used is 138 moles 2. Check the pH of this solution and record. 3. A5 M NAOH solution has been provided. 4. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record. 5. Add 205 µl of 5M NaOH into the 50 mM H2PO4 solution. Check the pH and record. 6. Add 205 µL more of 5M NaOH into the 50 mM H2PO, solution. Check the pH and record. 7. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record. Complete the following table "predicted pH." Please show all work on a separate sheet of paper and attach. Note that the pK, of H2PO, is 7.2. What would be the predicted pH's? Would they be similar to the actual pH's from procedure? After 45 µl of 5 | After 205 µl more of 5M NaOH Original After 205 µl more After 45 µl more solution M NaOH of 5M NaOH of 5 M NaOH Actual pH 4.30 6.05 6.90 11.01 11.29 Predicted pH

C. Titration of acid by a base Standardization of NaOH Volume of NaOH Mass of KHP Initial buret Final buret Trial used Molarity of NaOH (g) reading (mL) reading (mL) (mL) (1) (2) (3) (4) (5) 1.2075 0.7 25 24.3 0.243 (6) (7) (8) (9) (10) 1.2062 16.4 40.9 24.49 0.2412

prl 1) Please answer and explain, thank you A diluted solution of NaOH was used to titrate three samples of KHP. Find the concentration of NaOH for each titration and the average concentration. (attached is a photo)

Please correct answer and don't used hand raiting