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- The chemistry of finding/choosing the right spfA 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…
- CHEMISTRY RATE WILL BE GIVEN! NO LONG EXPLANATION NEEDED. ANSWER #3Explain the meaning of the relative sizes of the two shaded areas to the right of the dark vertical line in Figure 18.28.For 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. sp compound BaCO3 NaBr KC1 Does solubility change with pH? yes no yes no yes no pH = 7 highest solubility pH = 6 X pH = 5
- For 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. sp compound Cu Br Zn S Cal₂ Does solubility change with pH? ο οίο ο yes no yes no yes no pH = 4 highest solubility pH = 5 X pH = 6Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1) find Ka and use the value of Ka to calculate the initial pH of each trial 2) calculate Kb for the C8H4O4^-2 anion from the value of Ka that you obtained for KHP.Pls help ASAP ON ALL ASKED QUESTIONS PLS PLS
- Pls help ASAP pls. SHow all your work.#3 plzStandardization of 1N H2SO4 Titration 1 Titration 2 Titration 3 Titration 4 Mass of flask and Sodium Carbonate 1.5067 g 1.5098 g 1.5076 g 1.5077 Final buret reading (mL) 22 mL 22mL 21.5 mL 22.5 mL Volume of Sulphuric acid used (mL) 30 mL 30 mL 30 mL 30 mL What is the result of my titration?
