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- A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. The Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0] [0.200 + x] [0.175 + x] [0.200] [0.200 -x] [0.175 -x] 0 1.70 Kb 4.77 x 10-1⁰ = 12.3 [0.0200] [0.100] [0.0200 + x] [0.0200 -x] 10.8 [0.140] 2 [0.100 + x] 2.10 x 10-² A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the…A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > A 40.0 mL of 0.200 M H₂NNH₂ was titrated with 10.0 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. Before (mol) Change (mol) After (mol) 6.00 x 10 Initial (M) Change (M) Equilibrium (M) -X 0.140-x 0 -6.00 x 10³ 0 1 1 0.200 + x H₂NNH₂(aq) 0.200 0.175 + x 7.00 x 10³ H₂NNH₂(aq) + 2 0.200 0.200 - x 0.175-x 0.100 2 -7.00 x 10" A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a…2A student used a pipette to add 25 cm³ of sodium hydroxide of unknown concentration to a conical flask. The student carried out a titration to find out the volume of 0.1 mol/dm3 sulfuric acid needed to neutralise the sodium hydroxide. The following is the table of results obtained. Titration Volume of sulfuric acid used/cm³ 1 27.85 27.30 27.25 27.10 27.30 a. Write down a balanced equation for the reaction between sodium hydroxide and sulfuric acid. b. Describe the titration experimental procedure (details of washings are expected) c. Determine the average titre value and explain your choice of titre values in calculating the average. d. Determine the concentration of sodium hydroxide. e. If instead of sulfuric acid, hydrochloric acid of the same concentration was used what would you expect the average titre value to be and why?
- 7. A student performed an acid-base titration in the lab and recorded the results as shown below. Look very carefully at the results and answer the questions which follow. 演定結果 Nasco +2HC1 →Naclt Ca t H20 試験 流定 終結演定管讀數(cm) 開始演定管讀數(em) 所需演定劑的體積 (cm) 15.40 27.40 15,40 12.00 34.40 27.40 12,00 36 12.30 (1.5 1200 1200 tll5 3. 所間滴定劑的平均體積- 標 0.025/M 25 f 2010 (a) Why do we perform acid-base titrations in our labs? (b) In the titration performed by the student, what was the net ionic equation for the chemical reaction occurring? (c) List all the wrong things that the student did when writing the report on his titration experiment. (d) What good thing did this student do?Pls help ASAP pls. SHow all your work.#3 plz
- What is the pH of the solution at the end of the titration? The pH is very near or equal to 7. The pH is greater than 7. The pH is less than 7.INTRODUCTION LABORATORY SIMULATION 1) Calculate the pH of a solution prepared by dissolving 2.35 g of sodium acetate, CH3COONa, in 78.0 mL of 0.10 Macetic acid, CH;COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5. pH E METHODS O RESET P MY NOTES A LAB DATA SHOW LABELSFor each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. compound NaBr CaBr, PbF₂ Does solubility change with pH? O yes no yes no yes no pH = 6 highest solubility pH = 7 X pH = 8 Ś
