Scroll Lock Pause Break Pg Up Num Lock ACID-BASE TITRATION PRELAB QUESTIONS NAME Rachel MacDowel 1. A 4.00 mL sample of vinegar (active ingredient, acetic acid) was titrated with 0.1250M NaOH according to the following equation: HC₂H3O2 + NaOH NaC₂H3O₂ + HOH 25.19 mL of base was needed to reach the end point. Calculate the molarity of the acetic acid. 2. Calculate the grams of acetic acid in one liter of the vinegar.

Q: Which of the following is/are expected to be soluble in aqueous HCl? OH NH2 HN. Ph A D E Compound A…

A: HCl in water dissociate into H3O+ and Cl-. HCl + H2O = H3O+ + Cl-

Q: > Calculate the percent of acetic acid in a 20 mL vinegar sample. Titration was used, and it took…

A: Given data is Volume of the vinegar sample = 20 mL  Volume of NaOH used in the titration= 35.19 mL…

Q: 2. In Part A of this experiment you will prepare 0.1 M solutions of sodium carbonate (NazCO3),…

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Q: Calculate the concentration of KCL in grams per liternofnsolution. Divided the mass of the KCL…

A: mass of KCl = 1.433 gVolume of the solution = 5 mL = (5/1000) L = 0.005 LConcentration of KCl…

Q: 30 mL of an unknown concentration of phosphoric acid (triprotic) was titrated with 10 mL 0.05 M…

A: We have to predict the concentration of the acid

Q: Your lab assignment presentation involves putting together a presentation to show other students on…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Q: What volume of a 1.00 M barium hydroxide solution is required to neutralize 15.7 mL of a 0.231 M…

A: Given concentration of barium hydroxide = 1.00 M concentration of hydroiodic acid = 0.231 M volume…

Q: If you start with a solid acid that can be dissolved in water, you can determine the molar mass of…

A: Given that : Mass of acid = 0.447  Volume of water = 10 mL = 0.01 L Volume of base (NaOH) = 18.57 mL…

Q: An analytical chemist weighs out 0.165 g of an unknown triprotic acid into a 250 mL volumetric flask…

A: The unknown acid is triprotoic acid, hence the balanced chemical reaction between the acid and NaOH…

Q: Calculate the percent of acetic acid in a 20 mL vinegar sample. Titration was used, and it took…

A: Given ,  Volume of the vinegar sample, V = 20 mL  Volume of NaOH used in the titration= 35.19 mL…

Q: An experiment is carried out by titrating 31.8 mL of a 0.340 M potassium hydroxide solution with…

A: Reaction involved is : KOH + HBr ---> H2O + KBr Volume of KOH = 31.8 ml  Molarity of KOH = 0.340…

Q: A student is designing an experiment to test water from various sources for the presence of lead (a…

A: Pb is a heavy metal.  Its most common oxidation state is +2. Pb2+ is present in group II-A metal…

Q: A chemistry student weighs out 0.261 g of citric acid (H,C,H,O,), a triprotic acid, into a 250. mL…

A: Given-> Weight of citric acid = 0.261 gm Volume of citric acid = 250 ml  Molarity of NaOH =…

Q: In a titration, suppose 20.00 mL of 0.275 M oxalic acid solution required 21.72 mL of NaOH solution…

A: H2C2O4(aq) + 2NaOH(aq) -------> Na2C2O4(aq) +2H2O(l)

Q: What volume of 0.220 M HBr solution (in mL) is required to obtain 0.060 moles of HBr? A) 3.67 L B)…

A: Given, Number of moles of HBr = 0.060 moles Molarity = 0.220 M

Q: 1. A titration was performed using NaOH and a fruit juice. Suppose 31.3 mL of 0.250 M NaOH was used…

A:

Q: A student combined 37.2 mL of 1.69 M KMNO4 solution with 16.10 mL of a 0.891 M KMNO4 solution.…

A: First solution: The volume of KMnO4 solution =37.2 mL  Molarity of KMnO4 solution =1.69 M  Second…

Q: Consider the reaction of 75.0 mL of 0.350 M C5H5N (Kb = 1.7 x 10-9) with 100.0 mL of 0.449 M HCI. a)…

A: Since your question has multiple sub parts, we will solve only first three sub parts for you. If you…

Q: acid. What is the minimum amount of water of boiling water, you would need to fully dissolve 60 mg…

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Q: What volume of 1.2M potassium hydroxide is needed to neutralize 150mL of 3.2M sulfuric acid? Write a…

A: The balanced chemical reaction between potassium hydroxide (KOH) and sulfuric acid (H2SO4) is, 2KOH…

Q: When 20.00 ml of sulfuric acid of unknown concentration is titrated with 0.1249 M NaOH,  32.50 ml of…

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Q: Draw two different reactants that result in the product

A: We know, We can make alcohol from alkene by treating alkene with acids such as H2SO4 and water…

Q: ne molarity of

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Q: 21. When 20.00 ml of sulfuric acid of unknown concentration is titrated with 0.1249 M NaOH, 32.50 ml…

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Q: How many milliliter of 10.0 M HCI(aq) are needed to prepare 425.0mL of 1.00 M HCI(aq)?

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Q: A laboratory technician needs to make a 135 liter batch of a 20% acid solution. How can the…

A: Total volume of final acid mixture = 135LFor pure acid,concentration (v/v) = 100%For 10% (v/v)…

Q: For an experiment, I titrated NaOH with an unknown sample that had acetylsalicylic acid. In my few…

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Q: 150.0 mL of 0.500 mol/L sodium hydroxide, NaOH (aq), is required to titrate 125.0 mL of hydrochloric…

A: This is strong acid HCl - strong base NaOH titration. And give neutralization reactionNaOH(aq) +…

Q: A student is designing an experiment to test water from various sources for the presence of lead (a…

A: Hypothesis is a statement that presents an assumption that forms the basis of an argument. It may or…

Q: in a titration to determine the concentration of hydronium ions in a test solution, the test…

A: Given: In a titration to determine the concentration of hydronium ions in a test solution: The test…

Q: A 45.15 mL sample of phosphoric acid required 215mL of 1.000 M sodium hydroxide to reach the…

A: A balanced molecular equation is one in which the ionic reactions are represented as neutral…

Q: 75.00 mL sample of a HCL (acid) solution is placed in a flask with a few drops of phenolphthalein…

A:

Q: 3) In a far away land and long ago, a series of experiments were carried out. Three samples of…

A: In 2) Use law of constang proportion Divide the both Kalium and pyron masses We see that A same and…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.