Each of the following salts can be prepared from an acid and a base. Write the balanced molecular equation and the net ionic equation for the preparation of each. Indicate states of the reactants and products [(aq), (s), (1)]. Review solubility rules if necessary to determine the solubility of the reactants. (a) Al(CIO4)3 (aq) (b) BaCl2 (aq) (c) CSCH3CO2 (aq)
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- If Sn3(PO4)2 solution is to be subjected to argentometric titration, a) Write the balanced titration reaction. (products are Ag3PO4(s),, other ions are spectator ions b) Write the stoichiometric relationship (fundamental eqn) between the titrant (AgNO3) and the titrand (Sn3(PO4)2. c) Is this a feasible titration technique? Why?Arsenic in a 1.22 g sample of a pesticide was converted to AsO4^3- by chemical treatment. The ion was then titrated using Ag+ to form Ag3AsO4 as a precipitate. If 25 mL of 0.102 M Ag+ were required to reach the equivalence point in this titration.Calculate the percentage by mass of arsenic in the pesticide.Consider the following acid base titration between H2C3H5O3 (aq) with KOH (aq). A)Write a complete balanced equation. B) If 25.0 mL of the acid required 13.6 mL of 0.0789 M of the base to reach the equivalence point, what is the concentration of the acid? C)Which of the reactant is the limiting reactant?
- The purity of a pharmaceutical preparation of sulfanildamide (C6H4N2O2S), is prolonged oxidizing the sulfur in the sample to SO2 and bubbling this SO2 through a solution of H2O2 which converts it to H2SO4. The acid is titrated with a standard solution of NaOH (0.1251 M) until the end point with bromothymol blue, which changes color when both protons of the acid sulfuric have been neutralized. Calculate the purity of the preparation in % by weight given that a sample of 0.5136 g required 50.00 mL of the NaOH solutionThe molar solubility of Ag2C2O4 increases when it is dissolved in 0.5 M HClO4 (aq) instead of neutral distilled water. Write a balanced, net-ionic equation for the process that occurs between species in solution that contributes to the increased solubility of Ag2C2O4 (aq) in HClO4 (aq).In a precipitation titration of 46.00 mL of a chloride solution of unknown concentration, 31.00 mL of 0.6973 molar AgNO3 were required to reach the equivalence point. What is the molar concentration of the unknown chloride solution?
- A student was performing this experiment with an antacid tablet which contained C a CO3 but forgot to heat the antacid solution prior to starting the back-titration. As sodium hydroxide was added the student noticed the formation of an insoluble white precipitate. Would the presence of this precipitate cause the students experimentally determined volume of N a O H be incorrectly high or incorrectly low? Briefly explain. Hint: Carbon dioxide reacts with water to form carbonic acid. Question 3 options: Incorrectly high, the solution becomes more acidic if not boiled gently Incorrectly high, the solution becomes less acidic if not boiled gently Incorrectly low, the solution becomes more acidic if not boiled gently Incorrectly low, the solution becomes less acidic if not boiled gently7) Write the net ionic equations for the reaction with OH- by whicha) Al3 + forms a complex ionb) Al (OH) 3 dissolvesc) Fe3 + forms a precipitateYou have been provided with a 2.08 x 10-2 L sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?
- What of the following is the expression for the solubility product of Ba3(AsO4)2?Phosphate Buffered Saline (PBS) is a commonly used buffer for experiments in biology because its pH and ion concentrations are similar to those in mammalian organisms. It works in a similar fashion to the blood plasma buffer mentioned in the textbook, but using dihydrogen phosphate ions and hydrogen phosphate ions for buffering through the following chemical reaction: H2PO4- (aq) ⇆ H+(aq) + HPO42--(aq) The equilibrium arrows depict that the phosphate ion (H2PO4- ) is dissociating further into two component ions in solution, but at the same time H+ and HPO42- ions are combining simultaneously to form phosphate in solution. So, at any given point in time, and under the appropriate conditions, there is an equal quantity of dissolved ions and combined ions in solution. There is therefore always a hydrogen ion donor and an acceptor in solution. Based on the equation above, which ion plays the role of hydrogen-ion donor (acid) and which ion plays the role of hydrogen-ion acceptor (base)…A stainless steel alloy is to be analyzed for its chromium content. A 3.30 g sample of the steel is used to produce 250.0 mL of a solution containing Cr2O72−. A 10.0-mL portion of this solution is added to BaCl2(aq). When the pH of the solution is properly adjusted, 0.145 g BaCrO4(s) precipitates. A.) What is the percent Cr, by mass, in the steel sample? Express your answer numerically as a percentage.