lab titration assignment quizlet

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Titration Lab Quiz

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Erlenmeyer Flask

Bunsen Burner

Graduated Cylinder

Erlenmeyer Flasks

What is the correct measurement on this graduated cylinder?

Which is best for measuring volume?

Graduated Cylinders

Volumetric Flask

• 5. Multiple Choice Edit 45 seconds 1 pt acid + base ₋> salt + hydrogen salt + water salt + carbon dioxide + water salt
• 6. Multiple Choice Edit 30 seconds 1 pt What does pH measure? Amount of Oxygen Ions Amount of Hydrogen Ions The amount of salt in a solution The density
• 7. Multiple Choice Edit 45 seconds 1 pt HCl + NaOH →  NaH + ClOH NaCl + H 2 NaCl + H 2 O NaCl + Cl 2

What is the endpoint of a titration

The point at which the indicator that is used in a titration changes color

Where there is no base

• 9. Multiple Choice Edit 45 seconds 1 pt I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need? 2.5mL 5mL 25mL 50mL

What is the correct measurement on this burette?

• 12. Multiple Choice Edit 1 minute 1 pt I have 25mL   of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH? 0.8 M 1 M 1.25 M
• 13. Multiple Choice Edit 3 minutes 1 pt Identify the products of the chemical equation 3 LiOH + H 3 PO 4 → Li 3 PO 4 + 3 H 2 O LiPO 4  + 3 H 2 O Li(PO 4 ) 3  + 3 H 2 O BOY + La + N 2
• 14. Multiple Choice Edit 3 minutes 1 pt What acid and what base would you choose to prepare the salt potassium chlorate? KOH and HClO 3 KOH and HClO 2 HK and OHClO 3 HK and OHClO 2

A 10.00 mL sample of HBr is neutralized by 5.0 mL of 0.253 M LiOH solution. Calculate the molarity of the HBr solution.

• 16. Multiple Choice Edit 45 seconds 1 pt How many moles of Ca(OH) 2 are needed to neutralize three moles of HCl?  8 1.5 6 3
• 17. Multiple Choice Edit 3 minutes 1 pt For the acid-base titration combination of NaOH with 0.79 mol HCl, find the number of moles of NaOH that would be the chemically equivalent amount of HCl. 0.79 mol 1.6 mol 0.38 mol 3.2 mol
• 18. Multiple Choice Edit 45 seconds 1 pt Changes the color of indicators. Acids Bases All
• 19. Multiple Choice Edit 1 minute 1 pt If phenolphthalein turns bright pink, it indicates an acid  a base a neutral
• 20. Multiple Choice Edit 3 minutes 1 pt Which of the following is a conjugate acid/base pair? HCl/OCl - H 2 SO 4 /SO 4 2- NH 4 + /NH 3 H 3 O + /OH -

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Question: Titration of Acids and Bases 20 Pre-lab Questions Before beginning this experiment following questions. in the laboratory, you should be able to answer the Define standardization and state how you would go about doing it 2. Define the term ritration 3. Define the term molarity 4. Why do you determine a mass by difference? 5. What are equivalence points and

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To define standardization, start by explaining that it is the process of determining the exact concentration (molarity) of a solution.

1) Standardization is the process of determining the exact concentration (molarity) of a solution. Titration is one type of analytical procedure often used in standardization. In a titration, an exact volume of one substance is reacted with a known a …

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Pre lab Titration of Acids and Bases

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A chemical analysis that is performed primarily by using volumetric glassware is called volumetric analysis. During a volumetric analysis procedure, a known quantity or a carefully measured amount of one substance reacts with a to-be-determined amount of another substance with the reaction occurring in aqueous solution. The volumes are measured carefully with volumetric glassware. The known amount of substance is generally measured and available in two ways:

• As a primary standard: A precise mass (and moles) of a solid substance is measured on a balance, dissolved in water, and reacted with the substance that's being analyzed. A compound used as a primary has a known high degree of purity, a relatively large molar mass, is non-hygroscopic, and reacts in a predictable way.
• As a standard solution: A measured number of moles of substance is present in a measured volume of solution - a solution of known concentration, generally expressed as the molar concentration (or molarity) of the substance. A measured volume of the standard solution then reacts with the substance being analyzed. A standard solution is a solution having a very well-known concentration of a solute. The reaction of the known substance with the substance to be analyzed is conducted using a titration procedure The titration procedure requires a burette to dispense liquid, called the titrant, into a flask containing the analyte (Figure 1a). The titrant may be a solution of known or unknown concentration. The analyte may be a solution whose volume is measured with a pipet or it may be a dissolved solid with a very accurately measured mass. For the acid-base titration studied in this experiment, the titrant is a sodium hydroxide solution and the analyte is an acid. A reaction is complete when stoichiometric amounts of the substances are combined. In a titration this is the stoichiometric point (The stoichiometric point is also called the equivalence point, indicating the point at which stoichiometrically equivalent quantities of the reacting substances are combined.) In this experiment the stoichiometric point for the acid-base titration is detected with a penolphthalein indicator. Phenolphthalein is colorless in an acidic solution but red (or pink) in basic solution. The point in the titration when the phenolphthalein changes color is called the endpoint of the indicator (Figure 13b). Indicators are selected so that the stoichiometric point in the titration matches the endpoint of the indicator Stoichiometric amounts: amounts corresponding to the mole ratio of the balanced equation Acid-base indicator: a substance having an acidic structure with a different color than its basic structure pH: the negative logarithm of the molar concentration of H3O+, pH = -log[H3O+] pH 7 = -log[1 x 10-7] (the hydronium ion has a concentration of 1 x 10-7 M) Standardization of a Sodium Hydroxide Solution Solid sodium hydroxide is very hygroscopic (able to absorb water vapor readily); therefore, its mass cannot be measured accurately to prepare asolution with a well-known molar concentration. Another problem with the use of NaOH is that carbon dioxide, CO2, from the atmosphere reacts with the base NaOH to form the less soluble salt, Na2CO3. The CO2 is an acidic anhydride (meaning that when CO dissolves in water, it forms an acidic solution). CO 2 +2NaOH -- Na 2 CO 3 + H 2 O

To prepare a NaOH solution with an exact molar concentration, it must be standardized with an acid that is a primary standard. In Part A of this experiment, dry potassium hydrogen phthalate, KHC8H4O4, or KHP, is used as the primary acid standard for determining the molar concentration of a sodium hydroxide solution. Potassium hydrogen phthalate is a white, crystalline, acidic solid. It has the properties of a primary standard because of its high purity, relatively high molar mass, and because it is only very slightly hygroscopic. The amount of KHP used for the analysis is calculated from its measured mass and molar mass (204 g/mol): mass (g)KHC 8 H 4 O 4 × 1mol KHC 8 H 4 O 4 /204 KHC8H4O4 = mol KHC8H4O

From the balanced equation for the reaction, one mole of KHP reacts with one mole of NaOH according to the net ionic equation: HC 8 H 4 O- 4 + OH- → H 2 O + C 8 H 4 O2- 4

In the experimental procedure, an accurately measured mass of dry potassium hydrogen phthalate is dissolved in deionized water. A prepared NaOH solution is then dispensed from a burette into the KHC8H4O4 solution until the stoichiometric point is reached, signaled by the colorless to pink change of the phenolphthalein indicator. At this point the dispensed volume of NaOH is noted and recorded. The molar concentration of the NaOH solution is calculated using: molar concentration (M) NaOH (mol/L)= mol NaOH/L NaOH solution Once the molar concentration of the sodium hydroxide is calculated, the solution is said to be "standardized" and the sodium hydroxide solution is called a secondary standard solution. Molar Concentration of an Acid Solution In this part the percentage mass of an unknown acid inside a solid is determined. The standardized NaOH solution is used to titrate an accurately measure volume of acid to the stoichiometric point. Knowing the volume and molar concrentration of NaOh, we can calculate the number of moles of NaOh using volume (L) × molar concentration (mol/L) =mol NaOH From the stoichiometry of the reaction (your lab instructor (Matt) will inform you of the acid unknown type, HA or H2A), the moles of acid neutralized in the reaction can be calculated.

Procedure overview. A NaOH solution was prepared for you with an approximate concentration.

You will determine a more accurate molar concentration of the naoh solution (as the titrant) using, dry potassium hydrogen phthalate as a primary standard. you will then use the naoh solution, now, a secondary standard solution, to determine the molar concentration of an acid solution., part a. standardization of a sodium hydroxide solution you are to complete at least three "good", trials (± 1% reproducibility) in standardizing the naoh solution. prepare three clean 125-ml or 250-, ml erlenmeyer flasks for the titration., 1. obtain approximately 150 ml of the ~ 0 m naoh solution in a beaker. label the beaker. you, will use this naoh for your titrations., 2. prepare the primary standard acid, khp. a. calculate the mass of, khc8h4o4 that will require about 15-20 ml of your ~0 m naoh solution to reach the, stoichiometric point. check this calculation with your ta., b. accurately measure the amount you previously calculated (±0 g) of khc8h4o4 on weighing, paper and transfer it to a labeled erlenmeyer flask. prepare two more samples in the same way,, keeping track of the amount of khp in each flask. dissolve the khc8h4o4 in about 50 ml of, deionized water and add 1 or 2 drops of phenolphthalein., 3. rinse the burette with tap water and rinse several times with deionized water. rinse the burette, with three 5-ml portions of the diluted naoh solution, making certain that the solution wets the, entire inner surface. drain each rinse through the burette tip. collect the waste in a 400 ml beaker., at the end of your experiment, dispose of the waste in the basic aqueous waste carboy., 4. using a clean funnel or by carefully pouring from the beaker, fill the burette with the naoh, solution. read the volume by viewing the bottom of the meniscus. record this initial volume using, all certain digits (from the labeled calibration marks on the glassware) plus one uncertain digit (the, last digit which is the best estimate between the calibration marks). as you titrate, you can swirl the, erlenmeyer flask by hand or use a magnetic stirring rod and a hot plate. you can check-out a, magnetic stirring bar from your ta. place the hot plate beneath the burette. use only the stir, function and not the heat function on the hot plate., 5. slowly add the naoh titrant to the first acid sample prepared in step 2. swirl the flask after each, addition. initially, add the naoh solution in 0-1 ml increments. as the stoichiometric point nears,, the color fade of the indicator occurs more slowly. use the wash bottle filled with deionized water, to rinse any drops of naoh hanging from the burette tip into the flask. occasionally rinse the wall of, the flask with deionized water from your wash bottle. continue addition of the naoh titrant until, the endpoint is reached. the endpoint in the titration should be within one- half drop of a slight, pink color. the color should persist for at least 30 seconds. read and record the final volume of, naoh in the burette., 6. repeat the analysis with the remaining standard acid samples. refill the burette as needed., 7. use a table to record your titration data in the data and observations section of your lab, 8. calculate the molar concentration of the diluted naoh solution. the molar concentrations of the, naoh solution from the three analyses should be within ±1%. determine the mean and calculate, the standard deviation and rsd of your results. the mean molarity of your standardized naoh will, be used in the next part., part i - standardization of, trial 1 trial 2 trial 3, mass of flask (g), mass of flask and khp (g), final buret reading at equil., initial buret reading (ml), volume of 0 m naoh used, to reach equilibrium. (final -, column1 column2 column3 column, mass of khp (g), final buret reading at, endpoint (ml), volume of 0 m naoh, used to reach equilibrium.

• Multiple Choice

Course : Chemical Principles Laboratory I (CHEM 1215)

University : utah state university.

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