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- The commercial production of nitric acid involves thefollowing chemical reactions:4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g22 NO1g2 + O21g2¡2 NO21g23 NO21g2 + H2O1l2¡2 HNO31aq2 + NO1g2 (a) Predict what kind of reaction dopamine is most likely toundergo in water: redox, acid-base, precipitation, or metathesis?Explain your reasoning. (b) Patients with Parkinson’sdisease suffer from a shortage of dopamine and may need totake it to reduce symptoms. An IV (intravenous fluid) bag isfilled with a solution that contains 400.0 mg dopamine per250.0 mL of solution. What is the concentration of dopaminein the IV bag in units of molarity? (c) Experiments withrats show that if rats are dosed with 3.0 mg/kg of cocaine(that is, 3.0 mg cocaine per kg of animal mass), the concentrationof dopamine in their brains increases by 0.75 mM after60 seconds. Calculate how many molecules of dopaminewould be produced in a rat (average brain volume 5.00 mm3)after 60 seconds of a 3.0 mg/kg dose of cocaine.I believe the Henderson-Hasselbalch Equation is supposed to be used here, but I am lost and I am not sure. Pls help. Thank you!Arsenic(III) oxide (As2O3) is available in pure form and is a useful (but carcinogenic) primary standard for oxidizing agents such as MnO4-. The As2O3 is dissolved in base and then titrated with MnO4- in acidic solution. A small amount of iodide (I - ) or iodate (IO3-) is used to catalyze the reaction between H3AsO3 and MnO4-. As2O3 + 4 OH - 2 HAsO32- + H2OHAsO32- + 2 H+ H3AsO35 H3AsO3 + 2 MnO4- + 6 H+ 5 H3AsO4 + 2 Mn2+ + 3 H2O (a) A 3.209 g aliquot of KMnO4 (FM 158.034) was dissolved in 1.000 L of water, heated to cause any reactions with impurities to occur, cooled and filtered. What is the theoretical molarity of this solution if no MnO4- was consumed by impurities? M(b) What mass of As2O3 (FM 197.84) would be just sufficient to react with 25.00 mL of the KMnO4 solution in part (a)? g(c) It was found that 0.146 8 g of As2O3 required 29.98 mL of KMnO4 solution for the faint color of unreacted MnO4- to appear. In a blank titration, 0.03 mL of MnO4- was required to produce enough…
- Open bodies of water can act as carbon sinks due to the ability of carbon dioxide to dissolve in water. The dissolution of carbon dioxide produces carbonic acid (H2CO3) which then partially dissociates in an equilibrium reaction important for controlling water pH. CO2 (g) + H2O (l) H2CO3 (aq) H2CO3 (aq) ↔ H+ (aq) + HCO3- (aq) The equilibrium between carbonic acid (H2CO3) and bicarbonate (HCO3-) is influenced by the presence of dissolved metals from the bedrock underlying a body of water. Calcium from limestone (a type of sedimentary rock formed from marine exoskeletons) is one such metal. The graph below shows how the concentration of dissolved calcium ions (measured in parts per million, or mg/L) affects the concentration of carbon dioxide dissolved in ocean water (measured partial pressure). Based on this graph and your understanding of equilibrium, in what direction does the presence of limestone shift the carbonic acid/bicarbonate equilibrium?What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.310 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 × 10⁻⁴)Nitrous acid is a weak acid and has a concentration of 0.65 mol/L. What is the pH of the solution when equilibrium is established when Ka=4.5x10-4? b) The value of Kb for nitrous acid is ___________________ c) The percent ionization for nitrous acid is ____________%
- MnSO4•H2O is soluble in water at 25°C, with a solubility of 70.0 g per 1000 g of solution. A saturated solution of MnSO4•H2O has a density of 1.02 g mL-1. When MnSO4•H2O dissolves in water, it absorbs roughly 3.05 kJ/mol of energy. MnSO4•H2O = 169.03 g/mol; H2O = 18.02 g/mol; MW: MnSO4•H2O = 169.03 g/mol. Which of the following is TRUE about a 0.32 M solution of MnSO4•H2O in water? a. A 0.32 M solution contains 70.0 g MnSO4•H2O b. A 0.32 M solution of MnSO4•H2O is unsaturated c. A 0.32 M solution of MnSO4•H2O is supersaturated d. A 0.32 M solution of MnSO4•H2O is saturatedMnSO4•H2O is soluble in water at 25°C, with a solubility of 70.0 g per 1000 g of solution. A saturated solution of MnSO4•H2O has a density of 1.02 g mL-1. When MnSO4•H2O dissolves in water, it absorbs roughly 3.05 kJ/mol of energy. MnSO4•H2O = 169.03 g/mol; H2O = 18.02 g/mol; MW: MnSO4•H2O = 169.03 g/mol. What is the mole fraction of MnSO4•H2O in its saturated solution?A solution was made by dissolving 9.0g of hydrated aluminium sulphate Al2(SO)3 in 250cm3 of solution. (R.A.M: Al = 27, O = 16, S = 32, H = 1) Calculate the number of moles of hydrated aluminium sulphate solution the number of moles of sulphate ions in this solution the concentration (moldm-3) of the hydrated aluminium sulphate
- Ca2+ in a drinking water sample was analyzed by the following reactions below: Ca2+(aq) + C2O42-(aq) → CaC2O4 (s) → CaO(s) + CO(g)+ CO2(g) First an excess of C2O42- was added to 0.10 L of the Ca2+ water sample. Then CaC2O4 was precipitated, which was demcomposed into CaO with filtering and some heat. The CaO was measured to be 5.61 mg. What is the concentration of Ca2+ in the original water sample? The MW of CaO is 56.1 g/mol. 0.0100M 0.0010 M 1.00 M 0.100 M The partition coefficient (K) of methylamine (CH3NH2) is 4.50, preferring the organic layer over the aqueous layer in this extraction. The Ka of methylammonium (CH3NH3+) is 2.00 x 10-11. If 10 mL aqueous methylamine solution at pH 11.0 is extracted with 20.0 mL organic solvent, what is the fraction of solute remaining in the water (q)? HINT: methylamine is a weak base. 14.3% 10.0% 18.2% 81.8%The pKa of Cl3CCO2H is 0.64. What is the pH of a 0.580 M solution? What percentage of the Cl3CCO2H is dissociated? pH = ? = ? %A major component of coral is carbonate ions, which is created by the dissociation of bicarbonate ions as follows: HCO3-(aq) ⇌ CO32-(aq) + H+(aq) How will carbonate ion concentrations potentially be affected by an increase in the acidity of the ocean? Please explain the reasoning for your response in 1-2 sentences.
