titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 14.25 mL of 0.150 M NaOH to reach the phenolphthalein endpoint. What is the molarity of acetic acid

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ion The following table shows data from the titration of four 25.0 mL samples of a perchloric acid solution, HCIO4(aq), using a 0.225 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 25.0 mL of HCIO4 with 0.225 mol/L NaOH(aq) final burette reading (mL) initial burette reading (mL) volume of NaOH(aq) added (mL) colour at endpoint Trial 1 Use the data in the table below to answer the next two questions. Trial 2 Trial 3 Trial 4 Trial mL . . . mL mL 1 mL 19.9 0.4 2 Using the chart above, provide the volume of NaOH added for each of the trials. 38.8 3 19.3 19.9 0.2 4 38.4 19.3 blue green green green DELL

5 A chemistry graduate student is given 450. mL of a 0.10M ammonia (NH3) solution. Ammonia is a weak base with K, = 1.8 × 10. What mass of NH4Cl should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.11? You may assume that the volume of the solution doesn't change when the NH4Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ☐ ☐ x10

An HCl solution was titrated to determine its concentration using 15.00 mL  0.02500 M sodium carbonate standard solution. It required exactly 20.000 mL acid to completely neutralize the reaction between the titrant and analyte. What is the concentration of HCl solution?    a 0.06667 M   b 0.03750 M    c 0.01875 M   d 0.03333 M

You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity   Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?

If 2.50 mL of vinegar requires 34.90 mL of 0.0960 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in 500.0 mL of this vinegar? [density of vinegar = 1.01 g mL']

You are running an acid-base titration with hydrochloric acid and calcium hydroxide.  The calcium hydroxide is your titrant; it has a known concentration of 0.0891 M.  You have added 25.0 mL of the hydrochloric acid solution to an Erlenmeyer flask along with 2 drops of phenolphthalein (fee’-nol-thay-leen) indicator.  To begin your first trial, you fill a clean 50 mL buret with the calcium hydroxide solution.  Your starting volume is 0.25 mL. After the addition of solution from the buret, you see a color change in the flask, and the end point of the reaction is reached.  You note the final volume in the buret to be 18.75 mL. You begin again for your second titration trial.  You add 24.8 mL of the hydrochloric acid solution to a clean flask along with 2 drops of indicator.  You refill the buret to an initial volume of 1.42 mL.  When the reaction is complete, you note the final volume in the buret at 16.74 mL. Then you complete a third trial.  You add 25.6 mL of hydrochloric acid solution…

2. A student titrates 30.50 mL of a 4.50 g/L monoprotic acid (HA) with 25.00 mL of 0.10 M NaOH solution. a. Determine the concentration of the monoprotic acid (the ratio of the acid to base is 1:1). Concentration (2) = 4.50 30.50mL b. Determine the molar mass of the acid. = 147.542 M=4-50 = 180 0.0025 3. Determine the K, for a monoprotic weak acid with a pH of 3.5 at half the equivalence point. Ka = 10-3.5 4. What color will the solution turn indicating that the equivalence point has been reached?

A student performed titration to determine the concentration of citric acid with potassium permanganate solution. The net ionic equation is as follows: 5C6H8O7  + 18MnO4-   + 54H+  → 30CO2  + 47H2O  + 18Mn2+ The concentration of potassium permanganate soluiton is 0.266 M. The volume of lemon juice is 25.00 mL. The titration consumed 17.6  mL of potassium permanganate solution to reach the endpoint. Determine the moles of citric acid in the lemon juice sample.