Please help me fill in the highlighted. I don't know. Please explain how to get the answers. Thank you in advance. Titration of a Weak AcidReport SheetMolarity of NaOH used:0.100 MPart A. Show calculations for 1 trial:Moles of acd = 0.100M X%3DTrial 1Trial 2Trial 3Average18ml18.75ML 18.ST3MLmL OH added at19MLequivalence pointMolarity Titration of a Weak AcidStrong Acid & Strong Base14Read section 16.4 of the textbook before doing this experiment. This section will help youanswer the prelab questions as well as understand the experiment.12Weak Acid & Strong Base14-10Equivalence point8-12-Before oquivalence point10-Objectives:After equivalence point(OH in excess)(buffer range)6.6-Determine the concentration of a weak acid solution by titration.O Determine the molar mass of a weak acid from titratian data.Determine the pKa of a weak acid from titration data.4.Equivalence point(weak conjugate base)4-2-Initial pH (wenk acid)-0-0-10802550Volume of NaOH added (mL)Volume of NaOH added (ml)Background:A neutralization reaction occurs when and acid and base are mixed. Titration is a method todetermine the concentration of an acid or base by following these general steps:Experiment: Titration of a weak acid with a strong baseThe following neutralization reaction occurs when a weak acid and base are mixed:1) a specified volume of acid (or base) of unknown concentration is added to a beaker2) a pH electrode is placed into the beaker and the solution is mixed3) base (or acid) of known concentration is added to the beaker in fixed volumes (one ortwo mL) and the pH is recorded4) the volume of base (or acid) of known concentration added to the beaker required toreach the equivalence point is used to calculate the moles of base (or acid) added5) using stoichiometry, the number of moles of unknown acid (or base) present in the flaskis calculated6) the molarity of the unknown acid (or base) is calculated from the volume of the acid (orbase) added to the beaker.7) the pKa is calculated by finding the volume halfway to the equivalence point. Followover to the pH at this volume and this is the pka.HA + OH → H,0 +A-HA represents a weak acid and A is its conjugate base.At the equivalence (or stoichiometric) point mols OH = mols HASince you know the volume and molarity of added hydroxide, you also know the number ofmoles of hydroxide. Using the stoichiometry, which is 1:1 in this case, the number of moles ofacid will be the same value. Finally, the molarity of the acid can be calculated, taking intoaccount the calculated value of moles and the volume of acid used.A plot of pH vs. added volume of base, is a titration curve and it will have the shape shownPart A: Liquid Weak AcidProcedure:1. You will do three trials of the titration of a weak acid. Pipet 25 ml of unknown acid into a14250 mL beaker and add 50 ml of deionized water using a graduated cylinder. Prepare a totalof three beakers with this mixture.-equivalencepoint2. Prepare a buret by filling it with a standardized NaOH solution of known molarity. Be sure torecord the molarity in your notebook.3. Place one of the beakers on the stir plate, add a stir bar and begin stirring.pKa4 Vease Vpase4. Remove the pH electrode from the storage solution and rinse with deionized water.5. Calibrate the electrode according to the instructions for the MicroLab unit.6. Insert the electrode into the beaker taking care not to hit the bottom or sides of the beaker.Examples of titration curves for strong and weak acids are shown below. Note the differences inshape and the pH at the equivalence point:7. Record the initial pH.8 mL10 mL12ML4.173.984.194.386 mL8mLl0mL12ML 4.5914ML 4.925.148. Add NaOH from the buret in "1 or 2 ml aliquots and record pH after each addition. Keep arunning total of NaOH added when using the MicroLab unit.4.36Asthe titration approaches the equivalence point, the pH will begin to change rapidly so4.579.add the NaOH slowly (drop-wise) at this point.14ML16mL4.7910. Continue to the titration until a pH of ~12 is reached.11. Repeat the analysis with the other two beakers.5.0918ML16ML5.1410.26 8.0PH11.1524 mL l1.41CalculationsPlot all three titration curves on one graph using Excel.Volume of NaOH added in ml on the x-axis and pH on the y-axis20 mL18 mL 5.96622 mL9.4!10. 0e19.5mLDetermine the molarity the unknown acid for each trial.1. Calculate mols of OH added at the equivalence point.2. Calculate mols of acid present.3. Taking into account the volume of acid used, calculate the molarity.20 mL 10.5o22ML 11.2024mL il.4326 mL 11.5428 mL l1.6226ML 11.5328 mL 11.62Calculate the average molarity.Initial3.05Trial 32ml 3.494mL 3.11omL 4.058ML 4.2310 mL 4.4212ML 4.62he aPart B: Solid Weak Acid19.15 mL 10.4220.00ML 10.G022.00 ML I1.2324.00ML l1.4326.00ML l1.5528.00mL Il.633o Jolg Ait theacidProcedure:1. Dissolve 0.5 g of an unknown weak acid in80 mL of deionized water.OH- a2.2. Add 25 ml of the dissolved acid using a volumetric pipet into a 250 mL beaker.mass3. Titrate the acid as in Part A.ddeccurve14ML 4.85I6ML 5201 8mL 6.0218.25 mL 6.404. Repeat the titration two more times.CalculationsPlot all three titration curves on one graph using Excel.Volume of NaOH added in mL on the x-axis and pH on the y-axismolarity of NAOH :0.100 M18.50ML 7.6818.75 mL 9.1 8.0PH.19.00 ML 9.5419.25mL 9.9219.50 ML 10.2IT1T2T3PH BufferDetermine the molar mass of the unknown acid.4.077.001. Calculate mols of OH added at the equivalence point in each trial.2. Calculate mols of acid present in each trial.3. Calculate mols of acid present in all three trials combined4. Taking into account the mass of acid used, calculate the molar mass in the units g/mol.10.01VolumePHInitial PH:28ML 28ML28ML11.62I1.6211.63Calculate the pka of the acid for each trial, and the average pKa for all trials.2962973.05Hd

Question

Please help me fill in the highlighted. I don't know. Please explain how to get the answers. Thank you in advance. Titration of a Weak AcidReport SheetMolarity of NaOH used:0.100 MPart A. Show calculations for 1 trial:Moles of acd = 0.100M X%3DTrial 1Trial 2Trial 3Average18ml18.75ML 18.ST3MLmL OH added at19MLequivalence pointMolarity Titration of a Weak AcidStrong Acid & Strong Base14Read section 16.4 of the textbook before doing this experiment. This section will help youanswer the prelab questions as well as understand the experiment.12Weak Acid & Strong Base14-10Equivalence point8-12-Before oquivalence point10-Objectives:After equivalence point(OH in excess)(buffer range)6.6-Determine the concentration of a weak acid solution by titration.O Determine the molar mass of a weak acid from titratian data.Determine the pKa of a weak acid from titration data.4.Equivalence point(weak conjugate base)4-2-Initial pH (wenk acid)-0-0-10802550Volume of NaOH added (mL)Volume of NaOH added (ml)Background:A neutralization reaction occurs when and acid and base are mixed. Titration is a method todetermine the concentration of an acid or base by following these general steps:Experiment: Titration of a weak acid with a strong baseThe following neutralization reaction occurs when a weak acid and base are mixed:1) a specified volume of acid (or base) of unknown concentration is added to a beaker2) a pH electrode is placed into the beaker and the solution is mixed3) base (or acid) of known concentration is added to the beaker in fixed volumes (one ortwo mL) and the pH is recorded4) the volume of base (or acid) of known concentration added to the beaker required toreach the equivalence point is used to calculate the moles of base (or acid) added5) using stoichiometry, the number of moles of unknown acid (or base) present in the flaskis calculated6) the molarity of the unknown acid (or base) is calculated from the volume of the acid (orbase) added to the beaker.7) the pKa is calculated by finding the volume halfway to the equivalence point. Followover to the pH at this volume and this is the pka.HA + OH → H,0 +A-HA represents a weak acid and A is its conjugate base.At the equivalence (or stoichiometric) point mols OH = mols HASince you know the volume and molarity of added hydroxide, you also know the number ofmoles of hydroxide. Using the stoichiometry, which is 1:1 in this case, the number of moles ofacid will be the same value. Finally, the molarity of the acid can be calculated, taking intoaccount the calculated value of moles and the volume of acid used.A plot of pH vs. added volume of base, is a titration curve and it will have the shape shownPart A: Liquid Weak AcidProcedure:1. You will do three trials of the titration of a weak acid. Pipet 25 ml of unknown acid into a14250 mL beaker and add 50 ml of deionized water using a graduated cylinder. Prepare a totalof three beakers with this mixture.-equivalencepoint2. Prepare a buret by filling it with a standardized NaOH solution of known molarity. Be sure torecord the molarity in your notebook.3. Place one of the beakers on the stir plate, add a stir bar and begin stirring.pKa4 Vease Vpase4. Remove the pH electrode from the storage solution and rinse with deionized water.5. Calibrate the electrode according to the instructions for the MicroLab unit.6. Insert the electrode into the beaker taking care not to hit the bottom or sides of the beaker.Examples of titration curves for strong and weak acids are shown below. Note the differences inshape and the pH at the equivalence point:7. Record the initial pH.8 mL10 mL12ML4.173.984.194.386 mL8mLl0mL12ML 4.5914ML 4.925.148. Add NaOH from the buret in &#34;1 or 2 ml aliquots and record pH after each addition. Keep arunning total of NaOH added when using the MicroLab unit.4.36Asthe titration approaches the equivalence point, the pH will begin to change rapidly so4.579.add the NaOH slowly (drop-wise) at this point.14ML16mL4.7910. Continue to the titration until a pH of ~12 is reached.11. Repeat the analysis with the other two beakers.5.0918ML16ML5.1410.26 >8.0PH11.1524 mL l1.41CalculationsPlot all three titration curves on one graph using Excel.Volume of NaOH added in ml on the x-axis and pH on the y-axis20 mL18 mL 5.96622 mL9.4!10. 0e19.5mLDetermine the molarity the unknown acid for each trial.1. Calculate mols of OH added at the equivalence point.2. Calculate mols of acid present.3. Taking into account the volume of acid used, calculate the molarity.20 mL 10.5o22ML 11.2024mL il.4326 mL 11.5428 mL l1.6226ML 11.5328 mL 11.62Calculate the average molarity.Initial3.05Trial 32ml 3.494mL 3.11omL 4.058ML 4.2310 mL 4.4212ML 4.62he aPart B: Solid Weak Acid19.15 mL 10.4220.00ML 10.G022.00 ML I1.2324.00ML l1.4326.00ML l1.5528.00mL Il.633o Jolg Ait theacidProcedure:1. Dissolve 0.5 g of an unknown weak acid in80 mL of deionized water.OH- a2.2. Add 25 ml of the dissolved acid using a volumetric pipet into a 250 mL beaker.mass3. Titrate the acid as in Part A.ddeccurve14ML 4.85I6ML 5201 8mL 6.0218.25 mL 6.404. Repeat the titration two more times.CalculationsPlot all three titration curves on one graph using Excel.Volume of NaOH added in mL on the x-axis and pH on the y-axismolarity of NAOH :0.100 M18.50ML 7.6818.75 mL 9.1> 8.0PH.19.00 ML 9.5419.25mL 9.9219.50 ML 10.2IT1T2T3PH BufferDetermine the molar mass of the unknown acid.4.077.001. Calculate mols of OH added at the equivalence point in each trial.2. Calculate mols of acid present in each trial.3. Calculate mols of acid present in all three trials combined4. Taking into account the mass of acid used, calculate the molar mass in the units g/mol.10.01VolumePHInitial PH:28ML 28ML28ML11.62I1.6211.63Calculate the pka of the acid for each trial, and the average pKa for all trials.2962973.05Hd

Accepted Answer

Balanced equation for the reaction of weak acid, HA(aq) and NaOH(aq) or OH-(aq) is:
HA(aq) + OH-(aq)…

Titration of a Weak Acid Report Sheet Molarity of NAOH used: 0.100 M Part A. Show calculations for 1 trial: moles of acd = 0.100M X %3D Trial 1 Trial 2 Trial 3 Average 18mL 18.75m 18SC3ML mL OH added at 19ML equivalence point Molarity