Activity 4.2.2. Let's do this! Answer the following problems. Write your full solution on your answer sheet and box the final answer. 1. What is [H3O+] in a solution of 0.25 M CH3CO₂H and 0.030 M NaCH3CO₂? CH3CO₂H(aq) +H₂O(1) H3O'(aq)+CH3CO₂ (aq) K₂=1.8x10-6 2. What is [OH-] in a solution of 0.125 MCH3NH₂ and 0.130 MCH3NH3CI? CH3NH2(aq) +H₂O1) CH3NH3(aq)+OH (aq) K₂=4.4x104 3. What concentration M solution of NH3? of NH4NO3 is required to make [OH-] = 1.0 x 10-5 in a 0.200-
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- A 0.1220 g vitamin C tablet was dissolved in acid. This required 11.50 mL of 0.01740 M KIO3 to reach the endpoint. Considering these two half-reactions, ???3 + 5 ?? + 6?+ → 3?2 + 6?+ + 3?2? ?6?8?6 + ?2 → ?6?6?6 + 2?− + 2?+ Calculate percent by weight of ascorbic acid in the tablet.A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.The iodine produced when excess of KI was added to the solution containing 0.1259 g K2Cr2O7 required a 41.26 mL titration with Na2S2O3 required a 41.26 mL titration with Na2S2O3. P.S. Be able to answer numbers 3 and 4 ONLY. 1. Determine if it is basic or acidic and write the balance redox reaction for the reaction of dichromate ion with iodide ion in acidic medium. Unbalance equation: Cr2O72- (aq) + I- (aq) → Cr3+ + I2 (aq) 2. Determine if it is basic or acidic and write the balance redox reaction of iodine with sodium thiosulfate in acidic medium. Unbalance equation: S2O3 2- (aq) + I2 (aq) → S4O6 2- (aq) + I- (aq) 3. (i) What are the oxidizing agents in #1 and #2? (ii) What is the stoichiometric ratio between dichromate and thiosulfate? 4. Calculate the molar concentration of the thiosulfate solution.
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