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- #6 Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base: (a) 23.00 mL pH = (b) 39.40 mL pH = (c) 54.00 mL pH =II. Titrating HCI Solution with NaOH Solution 1. Prepare a titration curve. Plot pH (on the y-axis) versus volume of NaOH solution added (on the x-axis). If your initial buret reading was not 0.00 mL, remember to subtract your actual initial reading from each of your subsequent buret readings before plotting the titration data.4. A pH buffer solution contains 1.383 mole CH3COOH and 1.875 mole CH3COONa. The volume of the pH buffer solution is 250.0 mL. The acid dissociation constant of CH3COOH is 1.799x10-5. Please answer the following questions. A B. C. What is the pH of the solution? pH = Your answer follows. If you add 5.000 mL, 1.431 M of HCl to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. Your answer follows. If you add 5.000 mL, 1.431 M of Ba(OH)2 to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive.
- Question 7 of 14 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 × 10 6. 4 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H2NNH:(aq) H(aq) H.NNH (aq) Before (mol) Change (mol) After (mol) 5 RESET 0.100 0.200 + x 0.200 - x +x 0.200 0.100 - x 1.00 x 10-3 -1.00 x 10-3 2.00 x 103 -2.00 x 10 6.00 x 103 -6.00 x 103 0.100 + x 7.00 x 10-3 -7.00 x 10-3 8.00 x 103 -8.00 x 103 4:50 PM 4/15/2021 68 e to search Ins 近In Part C of Lab 8, you will prepare a phosphate buffer of a certain pH using the direct method. The questions below are to give you practice carrying out the necessary calculation for preparing the buffer from the correct phosphate compound. When you next come to lab to complete Part C of Lab 8, you will need to carry out this calculation again based on the actual mass of Na₂HPO4 7 H₂O that you weigh out. (a) Select a pH for your buffer solution. (Please make sure you and your lab partner(s) select the same pH, or someone will need to redo their calculations in lab.) --Select- (b) Based on the pH selected, will you need to use Na3PO4 12 H₂O or NaH2PO4 H₂O in order to generate a buffer of the desired pH? 2- 3- Hint: To answer this, you will need to determine pK values corresponding to the mixtures of the HPO anion with both phosphate anions PO4 and H2PO4 and evaluate which of these mixtures is closer to your target pH value. Na3PO4 12 H₂O NaH2PO4 H₂O • (c) Assuming you use exactly…5:51 1 .ll LTE Search Question 16 of 20 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH, with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 Based on the result of the acid-base reaction, set up the unknown. ICE table in order to determine the H2NNH3*(at H2O(1) =H;O*(aq) H2NNH2(aq + Initial (M) Change (M) Equilibrium (M) RESET 0.100 0.200 0.0333 0.0667 +x -X 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x www
- This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.73. If 50.00 mL of 1.00 M HC,H,O, (K, = 1.8 x 10) is titrated with 1.00M NAOH. What is the pH of the solution after the following volumes of NaOH have been added? a) 0.00 mL b) 25.00 mL c) 49.90 mL d) 50.10 mL
- Titration of unknown acid 1.trial 2.trial 15.0 mL of unknown acid + 12.2 mL NaOH 15.0 mL of unknown acid + 12.4 mL NaOH Calculation of the moles and molarity of the unknown acid solution;A 0.2386-g sample contained only NaCl and KBr was dissolved in water and required 50.00 mL of 0.04500 M AgNO3 for complete titration of both halides. If we assume there is x mol of NaCl in the original sample, which of the following statements are CORRECT? There are multiple correct answers. MW(NaCl) = 58.44 g/mol. MW(KBr) = 119.002 g/mol. There is x mol of KBr in the original sample. x+(0.2386-58.44x)/119.002-50.00*0.04500 There is (0.002250 - x) mol of KBr in the original sample. 58.44x+119.002(0.002250-x)=0.2386For the determination of basic species in 0.1878 g Talcid sample; 20 mL of 0.1009 M HCl solution was added to the sample and the necessary procedures were carried out and titrated with 0.1097 M NaOH solution. Since 10.2 mL of base solution is consumed at the end of the titration, what is the% base amount in CaCO3? (CaCO3: 100,087 g / mol)