The voltage measured by the pH meter is linearly proportional to the "H+ concentration" of the analyte solution. True or false? Is H+ concentration correct?
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- A pH meter can measure the concentration of H+ with an uncertainty of 5% between pH 4 and pH 8. What is the uncertainty in pH at pH = 6.00?If the base (NaOH) is standardized to 0.12 M in Part A of this experiment, calculate the amount of oxalic acid dihydrate (H2C2O4•2 H2O, MW = 126.06 g/mol) required to neutralize 35 mL of this NaOH solution.Suppose you did the titration three times and got the following data for the concentration of NaOH: 0.1002, 0.1006, and 0.1010 M. Calculate the relative average deviation of the data in units of ppt and enter the numerical answer below.
- The representation of the potential of an indicator electrode against the logarithm of the analyte activity is...(1). a straight line for all analyte concentrations. (2). a curve with zero slope for any concentration value below a certain limit. (3). an exponential curve. (4). a logarithmic curve.In the titration of 25.00 mL of a water sample, it took 20.840 mL of 4.350x 10−3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures)Diluting the analyte (e.g. by 10 x) will not affect the voltage at any point in the titration. Select one: True False
- Write a schematic representation for each of the cells used in the experiment. (A list appears at the end, with a total of 28 cells.) Cu/Ni Ni/Al Al/Pb Zn/Mg Cu/Zn Ni/Fe Al/Mg Fe/Pb Cu/Pb Ni/Sn Al/Fe Fe/Mg Cu/Mg Ni/Zn Al/Sn Fe/Sn Cu/Al Ni/Pb Zn/Fe Pb/Sn Cu/Fe Ni/Mg Zn/Sn Pb/Mg Cu/Sn Al/Zn Zn/Pb Sn/MgProcedure Preparation of Dilute Solution of Vinegar • Using a 10 mL pipette, transfer 10mL of vinegar into 100 mL volumetric flask. • Dilute to mark of the volumetric flask using distilled water. B. Titration of Diluted Solution of Vinegar • Transfer 25 mL of diluted solution to 250 mL Erlenmeyer flask. • Add 0.5 mL phenolphthalein indicator. Set aside. • Transfer 50mL of 0.110 M NaOH into a 50 mL burette. • Titrate the diluted solution until the phenolphthalein endpoint (very faint pink). • Record volume of NaOH used. Answer the question: What is the experimentally determined concentration of acetic acid in your vinegar solution: (Please give your answer to three significant figures.) ______ M Acetic Acidmix 500 ml of 0.1 M HCl solution with 300 ml of 2 M Ba (OH) 2 solution a) indicate the environment of the solution after mixing b) What color will the detectors, phenophthalein and litmus get?
- 2.1 Calculate the pH of 1.0 M HC2H3O2 solution, using Ka = 1.7 × 10-5 . Begin this calculation by defining the variable x. List the pH answer as “theoretical pH” on the report sheet. Have the instructor check this answer and all subsequent calculations. To test your prediction, obtain about 35 mL 1.0 M HC2H3O2 and add to a clean, dry 50 mL beaker. Measure the pH of this solution. Be sure the electrode is properly submerged and gives a stable reading. Record the pH reading in the “Observed pH” column on the report sheet. The value should be within ± 0.2 pH units of the calculated value. From the experimental pH and beginning concentrations of the solution components, calculate the remainder of the entries across the table to pKa . Save this solution for Sections 2.3 and 2.6. 2.2 Calculate the pH of 0.10 M HC2H3O2 solution. List this answer as “theoretical pH” on the report sheet. Test your prediction by placing 5 mL of 0.10 M HC2H3O2 in a test tube and testing its…In a titration, the following masses were recorded from an unknown substance that contain some amount of KHP in three experimental solutions 0.44, 0.437, and 0.437, if the volume of NaOH IN THE exp are 5, 10, and 8 respectively in order to the masses of unknown substances.1. Find the mass of KHP of each experiment 2.Find % KHP 3. Find average % KHP 4.find standard deviation.( Note; in a previous three 100% KHP experiments the average molarity of NaOH in each experiment are shown below average molarity=5.30x 10^-4+ 4.137x10^-4 + 5.0x10^-4 divided by 3 = 4.81x10^-4 ).What is the measurement in terms of appropriate si for a red blood cell that measured 0.0000071 m
