Please help me fill out the rest of the chart. Show work. 1:Experiment 9: ACID-BASE TITRATION: STANDARDIZATIONWhat is the frequency of the spectralmoves from n=5 to n=2?ΔΕΞData and ResultsDateNameCHEM 131 Sec:Part I: Using KHP for StandardizationShow all calculations on back of page and attach additional pages as necessary.#2#3#10.369 0.3130.311Mass of KHP (g)1.81x 103 / 1.53 x 10³1.52 x 10#Moles of KHP (moles)1.31 × 10³ | 1.53x10 | 1.52 × 10/³#Moles of NaOH used each trial0.01367 0.011700.01SSVolume of NaOH solution used each trial (L)0.1320.132 0.131Molarity NaOH in each trial On board0.132Average MolarityDeviation from Average Molarity00.001Average Deviation0.0030.25%Percent Average Deviation (RAD)Part II: Concentration of HCI Using Standard NaOHShow all calculations on back of page and attach additional pages as necessary.Molarity of Standard NaOH solution:#1#2#3Volume of NaOH solution in each flask (L)#Moles of NaOH in each flask#Moles of HCl to reach endpointVolume of HCl solution to reach endpoint (L)Molarity HCl in each trialAverage MolarityDeviation from Average MolarityAverage DeviationPercent Average Deviation (RAD)(123 MOITASIOExperiment 9: ACID-BASE TITRATION: STANDAPart II: Concentration of HCI Using Standard NaOH1. Under the "Data" section in your lab notebook, create a data table similar to thefollowing:zeigtebooga sluzootheHOMMolarity of NaOH from Part I =Trial ##2#30.050.00Initial buret reading of HCl (mL)Final buret reading of HCl (mL)Volume of HCI used (mL)106.4221.8210.370.000.00Initial buret reading of NaOH (mL)Final buret reading of NaOH (mL)Volume of NaOH used (mL)Ratio of Volume HCl/Vol NaOH13.7229.00Figure 9.2TilObtain two 50.00-mL burets and set them upon a ring stand fitted with a buret clamp asshown in Figure 9.2. Place gummed labelsprovided on the buret clamp to label one burets HCl and one as NaOH. Next, label a 250-L beaker as HCl and a 250-mL beaker asaOH. Both beakers must be clean and dry.nally, label a 400-mL beaker as "Waste." Itessential that you keep all your equipmentcarly marked#10.00123400.0036.35singosNaOHWWO-EstoHCI

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Chemistry

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Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)
The next 11 questions are related to the titration of 30.00 mL of a 0.1000 M acetic acid solution with 0.0800 M KOH. Assume that the temperature is 25 oC.What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration? How many mmol of acetate are present at the equivalence point? Report the analytical amount, not the equilibrium amount of acetate at the equivalence point. What is the total volume of the solution at the equivalence point?
What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically less than the number of moles of the analyte? pre-equivalence equivalence end stage post-equivalenc
For Ca2+ and Mg2+ determinations in a tap water sample, two 50 mL aliquots were pipetted and placed in different Erlenmeyer flasks. The first of them had the pH adjusted to 12 (Ca2+ titration) and the second to 10 (Ca2+ +Mg2+ titration). The volumes of EDTA (5.07*10-3 mol/L) used in the first and second titrations were 2.40 and 4.80 mL, respectively. Calculate: a) The concentration of Ca2+ in mg/L in the water sampleb) The concentration of Mg2+ in mg/L in the water sample
A 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.0663 M NaOH, requiring 35.18 mL to reach the end point. Determine the compound’s equivalent weight
Consider the titration of 20 mL of 0.10 M base with 0.20 M HCl. The analyte is dibasic withpKb1 = 5.00 and pKb2 = 10.00. Calculate the pH at the following volumes of HCl0 mL, 5 mL, 10 mL, 15 mL, 20 mL
Im doing a lab for chemistry and need help answering numers 1 and 2 below using the data provided. The molar concentration of the sodium for both is .100M. For your coarse titration, record the following results. initial burette volume reading of NaOH titrant at the start (mL) 0.00 final burette volume reading of NaOH titrant before the color change (mL) 29.05 volume of NaOH solution dispensed (mL) 29.05 volume of HCl solution in the flask (mL) 5.00 1) Calculate the molar HCl concentration using your coarse titration results. For your fine titration, record the following results. initial burette volume reading of NaOH titrant at the start (mL) 0.00 burette volume reading of NaOH titrant at the color change (mL) 30.05 volume of NaOH solution dispensed (mL) 30.05 volume of HCl solution in the flask (mL) 5.00 2)Calculate the molar HCl concentration using your fine titration results.
It is necessary to prepare 0.100 liters of buffer pH 4.70 with a concentration of 0.250 M, from a solution of acetic acid at 55.0% m/m (density = 1.010 g/mL) and sodium acetate of purity 97.0 %, how many g of salt do I need? (Ka = 1.78 x 10-5) (Note significant figures).
A 0.4071-g sample of CaCO3 (MM: 100.09 g/mole) is transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. A 50.00-mL aliqout of this solution was mixed with 5 mL of a pH 10 NH3-NH4Cl buffer that contains a small amount of Mg2+--EDTA to adjust the pH to 10. After adding calmagite as an indicator, the solution is titrated with the EDTA, requiring 42.63 mL to reach the end point. Report the molar concentration of EDTA in the titrant. 9.543 x 10-3 M 5.748 x 10-3 M 3.266 x 10-4 M 1.018 x 10-4 M
What volume (in mL) of 0.2968 M NaOH is required to titrate 15.00 mL of 0.2635 M HAc to the equivalence point? (give your answer to 2 decimal places)