Question 15 The equivalence point of a titration of 350.0 mL of 0.00016 M weak acid with 0.00082 M strong base is reached when 480.0 mL of strong base is added. What is the pKa of the weak acid? You Answered 1.03 Correct Answers 4.32 (with margin: 0.02)
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- 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;Given for nos. 10-11: In an acid-base titration, you were given with a 0.1050 M sodium hydroxide solution placed in a buret and is needed to neutralize 20.0 mL of 0.1500 M sulfuric acid. 10. How much moles of sulfuric acid is found in the 20.0 mL solution of a 0.15M H2SO4? Answer: Computation: 11. What volume of 0.1050 M sodium hydroxide solution is needed to neutralize 20.0 mL of 0.1500 M sulfuric acid? Answer: Computation: 12. Draw and label a complete laboratory set-up of acid-base titration using phenolphthalein as the indicator, using HCl as the analyte/sample, and using NaOH as the standard solution. Cite complete source/(s) if picture will be copied from the internet.What weight of sample should be taken for analysis sos that the volume of 0.1074N NaOH used for titration equals the percentage of potassium acid phthalate (KHC8H4O4) in the sample (Answer 2,193 g)
- #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 =What is the pH at the equivalence point in the titration of a 22.2 mL sample of a 0.320 M aqueous hypchlorous acid solution with a 0.451 M aqueous barium hydroxide solution? Please provide only typed answer solution no handwritten solution needed allowedA 93.0 mL sample of 0.0100 M HIO4 is titrated with 0.0200 M LIOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.4 mL pH = 2.57 (d) 47.4 mL pH = X X (b) 44.2 mL pH = (e) 78.1 mL pH = X X (c) 46.5 mL pH = X
- 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4:32 A) 7 Question 9 of 13 At the equivalence point for the titration of HCN with KOH, the pH is expected to be B) greater than 7 C) less than 7 all? Tap here or pull up for additional resources SubmitUle the Keferences to access important values if needed for this yestinn When a 23.2 mL sample of a 0.386 M aqueous hypochlorous acid solution is titrated with a 0.438 M aqueous bariem hydroside solution. (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 15.3 ml. of barium hydroxide have been added? Submit Answer 2 question attempts remainng
- 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 wwwII. 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.7. 9. A calculate tit HNO3 titration Sketch 50.00 titrated me titration and titration а and potta indicate point. with PH OF added Jample me begins " curve. laber the of 0.100 sketch 9 between potassium PH at 0.100 m . before M HNO3 KOH solution and a titration acetic acid. hydroxide, KOM. the after labelled curve 52.00 тя for CH3 C00 H equivalence